{"id":582,"date":"2017-12-14T21:41:35","date_gmt":"2017-12-14T21:41:35","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/some-definitions\/"},"modified":"2024-05-01T18:51:22","modified_gmt":"2024-05-01T18:51:22","slug":"some-definitions","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/some-definitions\/","title":{"raw":"9.1 Solutions","rendered":"9.1 Solutions"},"content":{"raw":"<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Describe the fundamental properties of solutions using correct terminology<\/li>\r\n \t<li>Classify solutions according to solubility<\/li>\r\n \t<li>Classify solutions according to conductivity<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div id=\"ball-ch11_s01\" class=\"section\" lang=\"en\">\r\n<h2>Solutions<\/h2>\r\nA <strong>solution<\/strong> is\u00a0defined as homogeneous mixtures of two or more substances.\u00a0Often, one component of a solution is present at a significantly greater concentration, in which case it is called the <strong>solvent<\/strong>. The other component of the solution present in relatively lesser concentrations are called <strong>solute<\/strong>. By major and minor we mean whichever component has the greater presence by mass or by moles. Sometimes this becomes confusing, especially with substances with very different molar masses. However, here we will confine the discussion to solutions for which the major component and the minor component are obvious.\r\n\r\n<\/div>\r\nSugar is a covalent solid composed of sucrose molecules, C<sub>12<\/sub>H<sub>22<\/sub>O<sub>11<\/sub>. When this compound dissolves in water, its molecules become uniformly distributed among the molecules of water:\r\n<p style=\"text-align: center;\">[latex]\\large{\\text{C}}_{12}{\\text{H}}_{22}{\\text{O}}_{11}\\left(s\\right)\\rightarrow{\\text{C}}_{12}{\\text{H}}_{22}{\\text{O}}_{11}\\left(aq\\right)[\/latex]<\/p>\r\nThe subscript \u201c<em>aq<\/em>\u201d in the equation signifies that the sucrose molecules are solutes and are therefore <em>individually dispersed<\/em> throughout the <em>aqueous solution<\/em> (water is the solvent). Although sucrose molecules are heavier than water molecules, they remain dispersed throughout the solution; gravity does not cause them to \u201csettle out\u201d over time.\r\n\r\nPotassium dichromate, K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7<\/sub>, is an ionic compound composed of colorless potassium ions, K<sup>+<\/sup>, and orange dichromate ions, [latex]\\text{C}{\\text{r}}_{2}{\\text{O}}_{7}{}^{2-}\\text{.}[\/latex] When a small amount of solid potassium chromate is added to water, the compound dissolves and dissociates to yield potassium ions and dichromate ions uniformly distributed throughout the mixture (Figure\u00a01), as indicated in this equation:\r\n<p style=\"text-align: center;\">[latex]\\large{\\text{K}}_{2}\\text{C}{\\text{r}}_{2}{\\text{O}}_{7}\\left(s\\right)\\rightarrow 2{\\text{ K}}^{+}\\left(aq\\right)+\\text{C}{\\text{r}}_{2}{\\text{O}}_{7}\\left(aq\\right)[\/latex]<\/p>\r\nAs for the mixture of sugar and water, this mixture is also an aqueous solution. Its solutes, potassium and dichromate ions, remain individually dispersed among the solvent (water) molecules.\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"883\"]<img class=\"\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23212122\/CNX_Chem_11_01_K2Cr2O7_11.jpg\" alt=\"The first photo shows a small mound of an orange crystalline solid. There is a right-facing arrow. The second photo shows a translucent, colorless liquid in a clear container. There is a right-facing arrow. The third photo shows a translucent orange liquid in a clear, covered container.\" width=\"883\" height=\"172\" \/> Figure\u00a01. When (left) potassium dichromate (K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7<\/sub>) is mixed with (middle) water, it forms (right) a homogeneous orange solution. (credit: modifications of work by Mark Ott)[\/caption]\r\n\r\n<div class=\"textbox\">Visit the <a href=\"http:\/\/phet.colorado.edu\/en\/simulation\/sugar-and-salt-solutions\" target=\"_blank\" rel=\"noopener\">PhET Sugar and Salt Solutions\u00a0virtual lab<\/a> to view simulations of the dissolution of common covalent and ionic substances (sugar and salt) in water.<\/div>\r\nWater is used so often as a solvent that the word solution has come to imply an aqueous solution to many people. However, almost any gas, liquid, or solid can act as a solvent. Many <strong>alloys<\/strong> are solid solutions of one metal dissolved in another; for example, US five-cent coins contain nickel dissolved in copper. Air is a gaseous solution, a homogeneous mixture of nitrogen, oxygen, and several other gases. Oxygen (a gas), alcohol (a liquid), and sugar (a solid) all dissolve in water (a liquid) to form liquid solutions. Table\u00a01\u00a0gives examples of several different solutions and the phases of the solutes and solvents.\r\n<table id=\"fs-idp13681744\" summary=\"The table provides solutes and solvents for a variety of solutions. In air, the solute is O subscript 2 g and the solvent is N subscript 2 g. In soft drinks, the solute is C O subscript 2 g and the solvent is H subscript 2 O l. In hydrogen in palladium, H subscript 2 g is the solute and P d s is the solvent. In rubbing alcohol, H subscript 2 O l is the solute and C subscript 3 H subscript 8 O l or 2 \u2013 propanol is the solvent. In saltwater, N a C l s is the solute and H subscript 2 O l is the solvent. In brass, Z n s is the solute and C u s is the solvent.\">\r\n<thead>\r\n<tr>\r\n<th colspan=\"3\">Table\u00a01. Different Types of Solutions<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr valign=\"top\">\r\n<th>Solution<\/th>\r\n<th>Solute<\/th>\r\n<th>Solvent<\/th>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td>air<\/td>\r\n<td>O<sub>2<\/sub>(<em>g<\/em>)<\/td>\r\n<td>N<sub>2<\/sub>(<em>g<\/em>)<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td>soft drinks[footnote]If bubbles of gas are observed within the liquid, the mixture is not homogeneous and, thus, not a solution.[\/footnote]<\/td>\r\n<td>CO<sub>2<\/sub>(<em>g<\/em>)<\/td>\r\n<td>H<sub>2<\/sub>O(<em>l<\/em>)<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td>hydrogen in palladium<\/td>\r\n<td>H<sub>2<\/sub>(<em>g<\/em>)<\/td>\r\n<td>Pd(<em>s<\/em>)<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td>rubbing alcohol<\/td>\r\n<td>H<sub>2<\/sub>O(<em>l<\/em>)<\/td>\r\n<td>C<sub>3<\/sub>H<sub>8<\/sub>O(<em>l<\/em>) (2-propanol)<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td>saltwater<\/td>\r\n<td>NaCl(<em>s<\/em>)<\/td>\r\n<td>H<sub>2<\/sub>O(<em>l<\/em>)<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td>brass<\/td>\r\n<td>Zn(<em>s<\/em>)<\/td>\r\n<td>Cu(<em>s<\/em>)<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nSolutions exhibit these defining traits:\r\n<ul>\r\n \t<li>They are homogeneous; that is, after a solution is mixed, it has the same composition at all points throughout (its composition is uniform).<\/li>\r\n \t<li>The physical state of a solution\u2014solid, liquid, or gas\u2014is typically the same as that of the solvent, as demonstrated by the examples in Table\u00a01.<\/li>\r\n \t<li>The components of a solution are dispersed on a molecular scale; that is, they consist of a mixture of separated molecules, atoms, and\/or ions.<\/li>\r\n \t<li>The dissolved solute in a solution will not settle out or separate from the solvent.<\/li>\r\n \t<li>The composition of a solution, or the concentrations of its components, can be varied continuously, within limits.<\/li>\r\n<\/ul>\r\n<div class=\"textbox examples\">\r\n<h3>Example 1: <strong>Solutions<\/strong><\/h3>\r\nA solution is made by dissolving 1.00 g of sucrose (C<sub class=\"subscript\">12<\/sub>H<sub class=\"subscript\">22<\/sub>O<sub class=\"subscript\">11<\/sub>) in 100.0 g of liquid water. Identify the solvent and solute in the resulting solution.\r\n\r\n[reveal-answer q=\"467425\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"467425\"]\r\n\r\nEither by mass or by moles, the obvious minor component is sucrose, so it is the solute. Water\u2014the majority component\u2014is the solvent. The fact that the resulting solution is the same phase as water also suggests that water is the solvent.\r\n\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\nA solution is made by dissolving 3.33 g of HCl(g) in 40.0 g of liquid methyl alcohol (CH<sub class=\"subscript\">3<\/sub>OH). Identify the solvent and solute in the resulting solution.\r\n\r\n[reveal-answer q=\"444976\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"444976\"]solute: HCl(g); solvent: CH<sub class=\"subscript\">3<\/sub>OH[\/hidden-answer]\r\n\r\n<\/div>\r\n<div id=\"ball-ch11_s01\" class=\"section\" lang=\"en\">\r\n<h2>Classifying Solutions According to Solubility<\/h2>\r\nImagine adding a small amount of salt to a glass of water, stirring until all the salt has dissolved, and then adding a bit more. You can repeat this process until the salt concentration of the solution reaches its natural limit. You can be certain that you have reached this limit because, no matter how long you stir the solution, undissolved salt remains. The concentration of salt in the solution at this point is known as its solubility.\r\n\r\nThe <strong>solubility<\/strong> of a solute in a particular solvent is the maximum concentration that may be achieved under given conditions when the dissolution process is <em>at equilibrium<\/em>. Referring to the example of salt in water:\r\n<p style=\"text-align: center;\">[latex]\\large\\text{NaCl}\\left(s\\right){\\rightleftharpoons}{\\text{ Na}}^{+}\\left(aq\\right)+{\\text{Cl}}^{-}\\left(aq\\right)\\text{.}[\/latex]<\/p>\r\nWhen a solute\u2019s concentration is equal to its solubility, the solution is said to be <strong>saturated<\/strong> with that solute. If the solute\u2019s concentration is less than its solubility, the solution is said to be <strong>unsaturated<\/strong>. A solution that contains a relatively low concentration of solute is called dilute, and one with a relatively high concentration is called concentrated.\r\n\r\nIf we add more salt to a saturated solution of salt, we see it fall to the bottom and no more seems to dissolve. In fact, the added salt does dissolve, as represented by the forward direction of the dissolution equation. Accompanying this process, dissolved salt will precipitate, as depicted by the reverse direction of the equation. The system is said to be at equilibrium when these two reciprocal processes are occurring at equal rates, and so the amount of undissolved and dissolved salt remains constant. Support for the simultaneous occurrence of the dissolution and precipitation processes is provided by noting that the number and sizes of the undissolved salt crystals will change over time, though their combined mass will remain the same.\r\n<div class=\"textbox\">Use this <a href=\"http:\/\/phet.colorado.edu\/en\/simulation\/soluble-salts\" target=\"_blank\" rel=\"noopener\">PhET\u00a0interactive simulation\u00a0on Salts and Solubility<\/a> to prepare various saturated solutions.<\/div>\r\nIn some circumstances, it is possible to dissolve more than the maximum amount of a solute in a solution. Usually, this happens by heating the solvent, dissolving more solute than would normally dissolve at regular temperatures, and letting the solution cool down slowly and carefully. Such solutions are called <strong>supersaturated <\/strong>solutions and are not stable; given an opportunity (such as dropping a crystal of solute in the solution), the excess solute will precipitate from the solution.\r\n<div id=\"ball-ch11_s01_t01\" class=\"table block\">\r\n<p class=\"title\"><span class=\"title-prefix\">Table 1.<\/span> Solubilities of Some Ionic Compounds<\/p>\r\n\r\n<table style=\"width: 409px;\" cellpadding=\"0\">\r\n<thead>\r\n<tr>\r\n<th style=\"width: 71px;\">Solute<\/th>\r\n<th style=\"width: 338px;\" align=\"right\">Solubility (g per 100 g of H<sub class=\"subscript\">2<\/sub>O at 25\u00b0C)<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<thead><\/thead>\r\n<tbody>\r\n<tr>\r\n<td style=\"width: 71px;\">AgCl<\/td>\r\n<td style=\"width: 338px;\" align=\"right\">0.00019<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 71px;\">CaCO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td style=\"width: 338px;\" align=\"right\">0.0006<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 71px;\">KBr<\/td>\r\n<td style=\"width: 338px;\" align=\"right\">70.7<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 71px;\">NaCl<\/td>\r\n<td style=\"width: 338px;\" align=\"right\">36.1<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 71px;\">NaNO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td style=\"width: 338px;\" align=\"right\">94.6<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>Example 2: <strong>Classifying Solutions according to solubility\r\n<\/strong><\/h3>\r\nSodium acetate has a solubility of 123.3 g\/100 g of water\u00a0 at 20 \u00b0C.\u00a0 Is a solution containing 45.0 g of sodium acetate per 100 g of H<sub class=\"subscript\">2<\/sub>O is unsaturated, saturated, or supersaturated.\r\n\r\n[reveal-answer q=\"4674215\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"4674215\"]\r\n\r\nSince the mass of sodium acetate (45 g) is lower than the total amount that can dissolve (123.3 g) the solution is unsaturated.\u00a0 Thus, all the sodium acetate will have dissolved.\r\n\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\nSodium nitrate has a solubility of 94.6 g\/100 g of water\u00a0 at 20 \u00b0C. If 97.8 g of sodium nitrate is added to 100 g of water, the resulting solution will be unsaturated, saturated, or supersaturated?\r\n\r\n[reveal-answer q=\"4449716\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"4449716\"]saturated[\/hidden-answer]\r\n\r\n<\/div>\r\n<\/div>\r\n<h2>Classifying Solutions According to Conductivity<\/h2>\r\nWhen some substances are dissolved in water, they undergo either a physical or a chemical change that yields ions in solution. These substances constitute an important class of compounds called <strong>electrolytes<\/strong>. Substances that do not yield ions when dissolved are called <strong>nonelectrolytes<\/strong>. If the physical or chemical process that generates the ions is essentially 100% efficient (all of the dissolved compound yields ions), then the substance is known as a <strong>strong electrolyte<\/strong>. If only a relatively small fraction of the dissolved substance undergoes the ion-producing process, it is called a <strong>weak electrolyte<\/strong>.\r\n\r\nSubstances may be identified as strong, weak, or nonelectrolytes by measuring the electrical conductance of an aqueous solution containing the substance. To conduct electricity, a substance must contain freely mobile, charged species. Most familiar is the conduction of electricity through metallic wires, in which case the mobile, charged entities are electrons. Solutions may also conduct electricity if they contain dissolved ions, with conductivity increasing as ion concentration increases. Applying a voltage to electrodes immersed in a solution permits assessment of the relative concentration of dissolved ions, either quantitatively, by measuring the electrical current flow, or qualitatively, by observing the brightness of a light bulb included in the circuit (Figure\u00a01).\r\n\r\n[caption id=\"attachment_2137\" align=\"aligncenter\" width=\"700\"]<img class=\" wp-image-2137\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23212131\/CNX_Chem_11_02_electrolyt1-1024x509.jpg\" alt=\"This diagram shows three separate beakers. Each has a wire plugged into a wall outlet. In each case, the wire leads from the wall to the beaker and is split resulting in two ends. One end leads to a light bulb and continues on to a rectangle labeled with a plus sign. The other end leads to a rectangle labeled with a minus sign. The rectangles are in a solution. In the first beaker, labeled \u201cEthanol No Conductivity,\u201d four pairs of linked small green spheres suspended in the solution between the rectangles. In the second beaker, labeled \u201cK C l Strong Conductivity,\u201d six individual green spheres, three labeled plus and three labeled minus are suspended in the solution. Each of the six spheres has an arrow extending from it pointing to the rectangle labeled with the opposite sign. In the third beaker, labeled \u201cAcetic acid solution Weak conductivity,\u201d two pairs of joined green spheres and two individual spheres, one labeled plus and one labeled minus are shown suspended between the two rectangles. The plus labeled sphere has an arrow pointing to the rectangle labeled minus and the minus labeled sphere has an arrow pointing to the rectangle labeled plus.\" width=\"700\" height=\"348\" \/> Figure\u00a01. Solutions of nonelectrolytes such as ethanol do not contain dissolved ions and cannot conduct electricity. Solutions of electrolytes contain ions that permit the passage of electricity. The conductivity of an electrolyte solution is related to the strength of the electrolyte.[\/caption]\r\n\r\nMost ionic compounds we come across in this course will be strong electrolytes.\u00a0 However, to truly know if an ionic compound dissociates in water we must rely on the solubility rules (Table 2).\r\n<p class=\"title\"><span class=\"title-prefix\">Table 2.<\/span> Solubility Rules<\/p>\r\n\r\n<table cellpadding=\"0\">\r\n<tbody>\r\n<tr>\r\n<td><strong class=\"emphasis bold\">These compounds generally dissolve in water (are soluble):<\/strong><\/td>\r\n<td><strong class=\"emphasis bold\">Exceptions:<\/strong><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>All compounds of Li<sup class=\"superscript\">+<\/sup>, Na<sup class=\"superscript\">+<\/sup>, K<sup class=\"superscript\">+<\/sup>, Rb<sup class=\"superscript\">+<\/sup>, Cs<sup class=\"superscript\">+<\/sup>, and NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup><\/td>\r\n<td>None<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>All compounds of NO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">\u2212<\/sup> and C<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">\u2212<\/sup><\/td>\r\n<td>None<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Compounds of Cl<sup class=\"superscript\">\u2212<\/sup>, Br<sup class=\"superscript\">\u2212<\/sup>, I<sup class=\"superscript\">\u2212<\/sup><\/td>\r\n<td>Ag<sup class=\"superscript\">+<\/sup>, Hg<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">2+<\/sup>, Pb<sup class=\"superscript\">2+<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Compounds of SO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">2<\/sup><\/td>\r\n<td>Hg<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">2+<\/sup>, Pb<sup class=\"superscript\">2+<\/sup>, Sr<sup class=\"superscript\">2+<\/sup>, Ba<sup class=\"superscript\">2+<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td><strong class=\"emphasis bold\">These compounds generally do not dissolve in water (are insoluble):<\/strong><\/td>\r\n<td><strong class=\"emphasis bold\">Exceptions:<\/strong><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Compounds of CO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">2\u2212<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212<\/sup><\/td>\r\n<td>Compounds of Li<sup class=\"superscript\">+<\/sup>, Na<sup class=\"superscript\">+<\/sup>, K<sup class=\"superscript\">+<\/sup>, Rb<sup class=\"superscript\">+<\/sup>, Cs<sup class=\"superscript\">+<\/sup>, and NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Compounds of OH<sup class=\"superscript\">\u2212<\/sup><\/td>\r\n<td>Compounds of Li<sup class=\"superscript\">+<\/sup>, Na<sup class=\"superscript\">+<\/sup>, K<sup class=\"superscript\">+<\/sup>, Rb<sup class=\"superscript\">+<\/sup>, Cs<sup class=\"superscript\">+<\/sup>, NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup>, Sr<sup class=\"superscript\">2+<\/sup>, and Ba<sup class=\"superscript\">2+<\/sup><\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n&nbsp;\r\n<div id=\"ball-ch11_s01\" class=\"section\" lang=\"en\">\r\n<div id=\"ball-ch11_s01_n04\" class=\"key_takeaways editable block\">\r\n<div class=\"bcc-box bcc-success\">\r\n<h3>Key Takeaways<\/h3>\r\n<ul id=\"ball-ch11_s01_l02\" class=\"itemizedlist\">\r\n \t<li>Solutions are composed of a solvent (major component) and a solute (minor component).<\/li>\r\n \t<li>Concentration is the expression of the amount of solute in a given amount of solvent and can be described by several qualitative terms.<\/li>\r\n \t<li>Solubility is a specific amount of solute that can dissolve in a given amount of solvent.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"bcc-box bcc-info\">\r\n<h3>Exercises<\/h3>\r\n<div id=\"ball-ch11_s01_qs01\" class=\"qandaset block\">\r\n<ol id=\"ball-ch11_s01_qs01_qd01\" class=\"qandadiv\">\r\n \t<li id=\"ball-ch11_s01_qs01_qd01_qa01\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch11_s01_qs01_p01\" class=\"para\">Define <em class=\"emphasis\">solute<\/em> and <em class=\"emphasis\">solvent<\/em>.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch11_s01_qs01_qd01_qa02\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch11_s01_qs01_p03\" class=\"para\">Define <em class=\"emphasis\">saturated<\/em>, <em class=\"emphasis\">unsaturated<\/em>, and <em class=\"emphasis\">supersaturated<\/em>.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch11_s01_qs01_qd01_qa03\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch11_s01_qs01_p05\" class=\"para\">A solution is prepared by combining 2.09 g of CO<sub class=\"subscript\">2<\/sub> and 35.5 g of H<sub class=\"subscript\">2<\/sub>O. Identify the solute and solvent.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch11_s01_qs01_qd01_qa04\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch11_s01_qs01_p07\" class=\"para\">A solution is prepared by combining 10.3 g of Hg(\u2113) and 45.0 g of Ag(s). Identify the solute and solvent.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch11_s01_qs01_qd01_qa05\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch11_s01_qs01_p09\" class=\"para\">Use\u00a0 Table 1 to decide if a solution containing 45.0 g of NaCl per 100 g of H<sub class=\"subscript\">2<\/sub>O is unsaturated, saturated, or supersaturated.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch11_s01_qs01_qd01_qa06\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch11_s01_qs01_p11\" class=\"para\">Use Table 1 to decide if a solution containing 0.000092 g of AgCl per 100 g of H<sub class=\"subscript\">2<\/sub>O is unsaturated, saturated, or supersaturated.<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<div class=\"question\"><\/div>\r\n<\/div>\r\n[reveal-answer q=\"6525754\"]Show Select Answers[\/reveal-answer]\r\n[hidden-answer a=\"6525754\"]\r\n\r\n1. The solvent is the majority component of a solution, whereas the solute is the minority component of a solution.\r\n\r\n3. solute: CO<sub class=\"subscript\">2<\/sub>; solvent: H<sub class=\"subscript\">2<\/sub>O\r\n\r\n5. supersaturated\r\n\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<h2>Glossary<\/h2>\r\n<strong>dissociation: <\/strong>physical process accompanying the dissolution of an ionic compound in which the compound\u2019s constituent ions are solvated and dispersed throughout the solution\r\n\r\n<strong>electrolyte: <\/strong>substance that produces ions when dissolved in water\r\n\r\n<strong>nonelectrolyte: <\/strong>substance that does not produce ions when dissolved in water\r\n\r\n<strong>saturated: <\/strong>of concentration equal to solubility; containing the maximum concentration of solute possible for a given temperature and pressure\r\n\r\n<strong>solubility: <\/strong>maximum concentration of a solute that may be achieved at a given temperature and pressure\r\n\r\n<strong>strong electrolyte: <\/strong>substance that dissociates or ionizes completely when dissolved in water\r\n\r\n<strong>supersaturated: <\/strong>of concentration that exceeds solubility; a nonequilibrium state\r\n\r\n<strong>unsaturated: <\/strong>of concentration less than solubility\r\n\r\n<strong>weak electrolyte: <\/strong>substance that ionizes only partially when dissolved in water\r\n\r\n<\/div>\r\n<\/div>","rendered":"<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Describe the fundamental properties of solutions using correct terminology<\/li>\n<li>Classify solutions according to solubility<\/li>\n<li>Classify solutions according to conductivity<\/li>\n<\/ul>\n<\/div>\n<div id=\"ball-ch11_s01\" class=\"section\" lang=\"en\">\n<h2>Solutions<\/h2>\n<p>A <strong>solution<\/strong> is\u00a0defined as homogeneous mixtures of two or more substances.\u00a0Often, one component of a solution is present at a significantly greater concentration, in which case it is called the <strong>solvent<\/strong>. The other component of the solution present in relatively lesser concentrations are called <strong>solute<\/strong>. By major and minor we mean whichever component has the greater presence by mass or by moles. Sometimes this becomes confusing, especially with substances with very different molar masses. However, here we will confine the discussion to solutions for which the major component and the minor component are obvious.<\/p>\n<\/div>\n<p>Sugar is a covalent solid composed of sucrose molecules, C<sub>12<\/sub>H<sub>22<\/sub>O<sub>11<\/sub>. When this compound dissolves in water, its molecules become uniformly distributed among the molecules of water:<\/p>\n<p style=\"text-align: center;\">[latex]\\large{\\text{C}}_{12}{\\text{H}}_{22}{\\text{O}}_{11}\\left(s\\right)\\rightarrow{\\text{C}}_{12}{\\text{H}}_{22}{\\text{O}}_{11}\\left(aq\\right)[\/latex]<\/p>\n<p>The subscript \u201c<em>aq<\/em>\u201d in the equation signifies that the sucrose molecules are solutes and are therefore <em>individually dispersed<\/em> throughout the <em>aqueous solution<\/em> (water is the solvent). Although sucrose molecules are heavier than water molecules, they remain dispersed throughout the solution; gravity does not cause them to \u201csettle out\u201d over time.<\/p>\n<p>Potassium dichromate, K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7<\/sub>, is an ionic compound composed of colorless potassium ions, K<sup>+<\/sup>, and orange dichromate ions, [latex]\\text{C}{\\text{r}}_{2}{\\text{O}}_{7}{}^{2-}\\text{.}[\/latex] When a small amount of solid potassium chromate is added to water, the compound dissolves and dissociates to yield potassium ions and dichromate ions uniformly distributed throughout the mixture (Figure\u00a01), as indicated in this equation:<\/p>\n<p style=\"text-align: center;\">[latex]\\large{\\text{K}}_{2}\\text{C}{\\text{r}}_{2}{\\text{O}}_{7}\\left(s\\right)\\rightarrow 2{\\text{ K}}^{+}\\left(aq\\right)+\\text{C}{\\text{r}}_{2}{\\text{O}}_{7}\\left(aq\\right)[\/latex]<\/p>\n<p>As for the mixture of sugar and water, this mixture is also an aqueous solution. Its solutes, potassium and dichromate ions, remain individually dispersed among the solvent (water) molecules.<\/p>\n<div style=\"width: 893px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23212122\/CNX_Chem_11_01_K2Cr2O7_11.jpg\" alt=\"The first photo shows a small mound of an orange crystalline solid. There is a right-facing arrow. The second photo shows a translucent, colorless liquid in a clear container. There is a right-facing arrow. The third photo shows a translucent orange liquid in a clear, covered container.\" width=\"883\" height=\"172\" \/><\/p>\n<p class=\"wp-caption-text\">Figure\u00a01. When (left) potassium dichromate (K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7<\/sub>) is mixed with (middle) water, it forms (right) a homogeneous orange solution. (credit: modifications of work by Mark Ott)<\/p>\n<\/div>\n<div class=\"textbox\">Visit the <a href=\"http:\/\/phet.colorado.edu\/en\/simulation\/sugar-and-salt-solutions\" target=\"_blank\" rel=\"noopener\">PhET Sugar and Salt Solutions\u00a0virtual lab<\/a> to view simulations of the dissolution of common covalent and ionic substances (sugar and salt) in water.<\/div>\n<p>Water is used so often as a solvent that the word solution has come to imply an aqueous solution to many people. However, almost any gas, liquid, or solid can act as a solvent. Many <strong>alloys<\/strong> are solid solutions of one metal dissolved in another; for example, US five-cent coins contain nickel dissolved in copper. Air is a gaseous solution, a homogeneous mixture of nitrogen, oxygen, and several other gases. Oxygen (a gas), alcohol (a liquid), and sugar (a solid) all dissolve in water (a liquid) to form liquid solutions. Table\u00a01\u00a0gives examples of several different solutions and the phases of the solutes and solvents.<\/p>\n<table id=\"fs-idp13681744\" summary=\"The table provides solutes and solvents for a variety of solutions. In air, the solute is O subscript 2 g and the solvent is N subscript 2 g. In soft drinks, the solute is C O subscript 2 g and the solvent is H subscript 2 O l. In hydrogen in palladium, H subscript 2 g is the solute and P d s is the solvent. In rubbing alcohol, H subscript 2 O l is the solute and C subscript 3 H subscript 8 O l or 2 \u2013 propanol is the solvent. In saltwater, N a C l s is the solute and H subscript 2 O l is the solvent. In brass, Z n s is the solute and C u s is the solvent.\">\n<thead>\n<tr>\n<th colspan=\"3\">Table\u00a01. Different Types of Solutions<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr valign=\"top\">\n<th>Solution<\/th>\n<th>Solute<\/th>\n<th>Solvent<\/th>\n<\/tr>\n<tr valign=\"top\">\n<td>air<\/td>\n<td>O<sub>2<\/sub>(<em>g<\/em>)<\/td>\n<td>N<sub>2<\/sub>(<em>g<\/em>)<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td>soft drinks<a class=\"footnote\" title=\"If bubbles of gas are observed within the liquid, the mixture is not homogeneous and, thus, not a solution.\" id=\"return-footnote-582-1\" href=\"#footnote-582-1\" aria-label=\"Footnote 1\"><sup class=\"footnote\">[1]<\/sup><\/a><\/td>\n<td>CO<sub>2<\/sub>(<em>g<\/em>)<\/td>\n<td>H<sub>2<\/sub>O(<em>l<\/em>)<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td>hydrogen in palladium<\/td>\n<td>H<sub>2<\/sub>(<em>g<\/em>)<\/td>\n<td>Pd(<em>s<\/em>)<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td>rubbing alcohol<\/td>\n<td>H<sub>2<\/sub>O(<em>l<\/em>)<\/td>\n<td>C<sub>3<\/sub>H<sub>8<\/sub>O(<em>l<\/em>) (2-propanol)<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td>saltwater<\/td>\n<td>NaCl(<em>s<\/em>)<\/td>\n<td>H<sub>2<\/sub>O(<em>l<\/em>)<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td>brass<\/td>\n<td>Zn(<em>s<\/em>)<\/td>\n<td>Cu(<em>s<\/em>)<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Solutions exhibit these defining traits:<\/p>\n<ul>\n<li>They are homogeneous; that is, after a solution is mixed, it has the same composition at all points throughout (its composition is uniform).<\/li>\n<li>The physical state of a solution\u2014solid, liquid, or gas\u2014is typically the same as that of the solvent, as demonstrated by the examples in Table\u00a01.<\/li>\n<li>The components of a solution are dispersed on a molecular scale; that is, they consist of a mixture of separated molecules, atoms, and\/or ions.<\/li>\n<li>The dissolved solute in a solution will not settle out or separate from the solvent.<\/li>\n<li>The composition of a solution, or the concentrations of its components, can be varied continuously, within limits.<\/li>\n<\/ul>\n<div class=\"textbox examples\">\n<h3>Example 1: <strong>Solutions<\/strong><\/h3>\n<p>A solution is made by dissolving 1.00 g of sucrose (C<sub class=\"subscript\">12<\/sub>H<sub class=\"subscript\">22<\/sub>O<sub class=\"subscript\">11<\/sub>) in 100.0 g of liquid water. Identify the solvent and solute in the resulting solution.<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q467425\">Show Answer<\/span><\/p>\n<div id=\"q467425\" class=\"hidden-answer\" style=\"display: none\">\n<p>Either by mass or by moles, the obvious minor component is sucrose, so it is the solute. Water\u2014the majority component\u2014is the solvent. The fact that the resulting solution is the same phase as water also suggests that water is the solvent.<\/p>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>A solution is made by dissolving 3.33 g of HCl(g) in 40.0 g of liquid methyl alcohol (CH<sub class=\"subscript\">3<\/sub>OH). Identify the solvent and solute in the resulting solution.<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q444976\">Show Answer<\/span><\/p>\n<div id=\"q444976\" class=\"hidden-answer\" style=\"display: none\">solute: HCl(g); solvent: CH<sub class=\"subscript\">3<\/sub>OH<\/div>\n<\/div>\n<\/div>\n<div id=\"ball-ch11_s01\" class=\"section\" lang=\"en\">\n<h2>Classifying Solutions According to Solubility<\/h2>\n<p>Imagine adding a small amount of salt to a glass of water, stirring until all the salt has dissolved, and then adding a bit more. You can repeat this process until the salt concentration of the solution reaches its natural limit. You can be certain that you have reached this limit because, no matter how long you stir the solution, undissolved salt remains. The concentration of salt in the solution at this point is known as its solubility.<\/p>\n<p>The <strong>solubility<\/strong> of a solute in a particular solvent is the maximum concentration that may be achieved under given conditions when the dissolution process is <em>at equilibrium<\/em>. Referring to the example of salt in water:<\/p>\n<p style=\"text-align: center;\">[latex]\\large\\text{NaCl}\\left(s\\right){\\rightleftharpoons}{\\text{ Na}}^{+}\\left(aq\\right)+{\\text{Cl}}^{-}\\left(aq\\right)\\text{.}[\/latex]<\/p>\n<p>When a solute\u2019s concentration is equal to its solubility, the solution is said to be <strong>saturated<\/strong> with that solute. If the solute\u2019s concentration is less than its solubility, the solution is said to be <strong>unsaturated<\/strong>. A solution that contains a relatively low concentration of solute is called dilute, and one with a relatively high concentration is called concentrated.<\/p>\n<p>If we add more salt to a saturated solution of salt, we see it fall to the bottom and no more seems to dissolve. In fact, the added salt does dissolve, as represented by the forward direction of the dissolution equation. Accompanying this process, dissolved salt will precipitate, as depicted by the reverse direction of the equation. The system is said to be at equilibrium when these two reciprocal processes are occurring at equal rates, and so the amount of undissolved and dissolved salt remains constant. Support for the simultaneous occurrence of the dissolution and precipitation processes is provided by noting that the number and sizes of the undissolved salt crystals will change over time, though their combined mass will remain the same.<\/p>\n<div class=\"textbox\">Use this <a href=\"http:\/\/phet.colorado.edu\/en\/simulation\/soluble-salts\" target=\"_blank\" rel=\"noopener\">PhET\u00a0interactive simulation\u00a0on Salts and Solubility<\/a> to prepare various saturated solutions.<\/div>\n<p>In some circumstances, it is possible to dissolve more than the maximum amount of a solute in a solution. Usually, this happens by heating the solvent, dissolving more solute than would normally dissolve at regular temperatures, and letting the solution cool down slowly and carefully. Such solutions are called <strong>supersaturated <\/strong>solutions and are not stable; given an opportunity (such as dropping a crystal of solute in the solution), the excess solute will precipitate from the solution.<\/p>\n<div id=\"ball-ch11_s01_t01\" class=\"table block\">\n<p class=\"title\"><span class=\"title-prefix\">Table 1.<\/span> Solubilities of Some Ionic Compounds<\/p>\n<table style=\"width: 409px;\" cellpadding=\"0\">\n<thead>\n<tr>\n<th style=\"width: 71px;\">Solute<\/th>\n<th style=\"width: 338px;\" align=\"right\">Solubility (g per 100 g of H<sub class=\"subscript\">2<\/sub>O at 25\u00b0C)<\/th>\n<\/tr>\n<\/thead>\n<thead><\/thead>\n<tbody>\n<tr>\n<td style=\"width: 71px;\">AgCl<\/td>\n<td style=\"width: 338px;\" align=\"right\">0.00019<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 71px;\">CaCO<sub class=\"subscript\">3<\/sub><\/td>\n<td style=\"width: 338px;\" align=\"right\">0.0006<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 71px;\">KBr<\/td>\n<td style=\"width: 338px;\" align=\"right\">70.7<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 71px;\">NaCl<\/td>\n<td style=\"width: 338px;\" align=\"right\">36.1<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 71px;\">NaNO<sub class=\"subscript\">3<\/sub><\/td>\n<td style=\"width: 338px;\" align=\"right\">94.6<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<div class=\"textbox examples\">\n<h3>Example 2: <strong>Classifying Solutions according to solubility<br \/>\n<\/strong><\/h3>\n<p>Sodium acetate has a solubility of 123.3 g\/100 g of water\u00a0 at 20 \u00b0C.\u00a0 Is a solution containing 45.0 g of sodium acetate per 100 g of H<sub class=\"subscript\">2<\/sub>O is unsaturated, saturated, or supersaturated.<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q4674215\">Show Answer<\/span><\/p>\n<div id=\"q4674215\" class=\"hidden-answer\" style=\"display: none\">\n<p>Since the mass of sodium acetate (45 g) is lower than the total amount that can dissolve (123.3 g) the solution is unsaturated.\u00a0 Thus, all the sodium acetate will have dissolved.<\/p>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>Sodium nitrate has a solubility of 94.6 g\/100 g of water\u00a0 at 20 \u00b0C. If 97.8 g of sodium nitrate is added to 100 g of water, the resulting solution will be unsaturated, saturated, or supersaturated?<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q4449716\">Show Answer<\/span><\/p>\n<div id=\"q4449716\" class=\"hidden-answer\" style=\"display: none\">saturated<\/div>\n<\/div>\n<\/div>\n<\/div>\n<h2>Classifying Solutions According to Conductivity<\/h2>\n<p>When some substances are dissolved in water, they undergo either a physical or a chemical change that yields ions in solution. These substances constitute an important class of compounds called <strong>electrolytes<\/strong>. Substances that do not yield ions when dissolved are called <strong>nonelectrolytes<\/strong>. If the physical or chemical process that generates the ions is essentially 100% efficient (all of the dissolved compound yields ions), then the substance is known as a <strong>strong electrolyte<\/strong>. If only a relatively small fraction of the dissolved substance undergoes the ion-producing process, it is called a <strong>weak electrolyte<\/strong>.<\/p>\n<p>Substances may be identified as strong, weak, or nonelectrolytes by measuring the electrical conductance of an aqueous solution containing the substance. To conduct electricity, a substance must contain freely mobile, charged species. Most familiar is the conduction of electricity through metallic wires, in which case the mobile, charged entities are electrons. Solutions may also conduct electricity if they contain dissolved ions, with conductivity increasing as ion concentration increases. Applying a voltage to electrodes immersed in a solution permits assessment of the relative concentration of dissolved ions, either quantitatively, by measuring the electrical current flow, or qualitatively, by observing the brightness of a light bulb included in the circuit (Figure\u00a01).<\/p>\n<div id=\"attachment_2137\" style=\"width: 710px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" aria-describedby=\"caption-attachment-2137\" class=\"wp-image-2137\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23212131\/CNX_Chem_11_02_electrolyt1-1024x509.jpg\" alt=\"This diagram shows three separate beakers. Each has a wire plugged into a wall outlet. In each case, the wire leads from the wall to the beaker and is split resulting in two ends. One end leads to a light bulb and continues on to a rectangle labeled with a plus sign. The other end leads to a rectangle labeled with a minus sign. The rectangles are in a solution. In the first beaker, labeled \u201cEthanol No Conductivity,\u201d four pairs of linked small green spheres suspended in the solution between the rectangles. In the second beaker, labeled \u201cK C l Strong Conductivity,\u201d six individual green spheres, three labeled plus and three labeled minus are suspended in the solution. Each of the six spheres has an arrow extending from it pointing to the rectangle labeled with the opposite sign. In the third beaker, labeled \u201cAcetic acid solution Weak conductivity,\u201d two pairs of joined green spheres and two individual spheres, one labeled plus and one labeled minus are shown suspended between the two rectangles. The plus labeled sphere has an arrow pointing to the rectangle labeled minus and the minus labeled sphere has an arrow pointing to the rectangle labeled plus.\" width=\"700\" height=\"348\" \/><\/p>\n<p id=\"caption-attachment-2137\" class=\"wp-caption-text\">Figure\u00a01. Solutions of nonelectrolytes such as ethanol do not contain dissolved ions and cannot conduct electricity. Solutions of electrolytes contain ions that permit the passage of electricity. The conductivity of an electrolyte solution is related to the strength of the electrolyte.<\/p>\n<\/div>\n<p>Most ionic compounds we come across in this course will be strong electrolytes.\u00a0 However, to truly know if an ionic compound dissociates in water we must rely on the solubility rules (Table 2).<\/p>\n<p class=\"title\"><span class=\"title-prefix\">Table 2.<\/span> Solubility Rules<\/p>\n<table cellpadding=\"0\">\n<tbody>\n<tr>\n<td><strong class=\"emphasis bold\">These compounds generally dissolve in water (are soluble):<\/strong><\/td>\n<td><strong class=\"emphasis bold\">Exceptions:<\/strong><\/td>\n<\/tr>\n<tr>\n<td>All compounds of Li<sup class=\"superscript\">+<\/sup>, Na<sup class=\"superscript\">+<\/sup>, K<sup class=\"superscript\">+<\/sup>, Rb<sup class=\"superscript\">+<\/sup>, Cs<sup class=\"superscript\">+<\/sup>, and NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup><\/td>\n<td>None<\/td>\n<\/tr>\n<tr>\n<td>All compounds of NO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">\u2212<\/sup> and C<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">\u2212<\/sup><\/td>\n<td>None<\/td>\n<\/tr>\n<tr>\n<td>Compounds of Cl<sup class=\"superscript\">\u2212<\/sup>, Br<sup class=\"superscript\">\u2212<\/sup>, I<sup class=\"superscript\">\u2212<\/sup><\/td>\n<td>Ag<sup class=\"superscript\">+<\/sup>, Hg<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">2+<\/sup>, Pb<sup class=\"superscript\">2+<\/sup><\/td>\n<\/tr>\n<tr>\n<td>Compounds of SO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">2<\/sup><\/td>\n<td>Hg<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">2+<\/sup>, Pb<sup class=\"superscript\">2+<\/sup>, Sr<sup class=\"superscript\">2+<\/sup>, Ba<sup class=\"superscript\">2+<\/sup><\/td>\n<\/tr>\n<tr>\n<td><strong class=\"emphasis bold\">These compounds generally do not dissolve in water (are insoluble):<\/strong><\/td>\n<td><strong class=\"emphasis bold\">Exceptions:<\/strong><\/td>\n<\/tr>\n<tr>\n<td>Compounds of CO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">2\u2212<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212<\/sup><\/td>\n<td>Compounds of Li<sup class=\"superscript\">+<\/sup>, Na<sup class=\"superscript\">+<\/sup>, K<sup class=\"superscript\">+<\/sup>, Rb<sup class=\"superscript\">+<\/sup>, Cs<sup class=\"superscript\">+<\/sup>, and NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup><\/td>\n<\/tr>\n<tr>\n<td>Compounds of OH<sup class=\"superscript\">\u2212<\/sup><\/td>\n<td>Compounds of Li<sup class=\"superscript\">+<\/sup>, Na<sup class=\"superscript\">+<\/sup>, K<sup class=\"superscript\">+<\/sup>, Rb<sup class=\"superscript\">+<\/sup>, Cs<sup class=\"superscript\">+<\/sup>, NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup>, Sr<sup class=\"superscript\">2+<\/sup>, and Ba<sup class=\"superscript\">2+<\/sup><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>&nbsp;<\/p>\n<div id=\"ball-ch11_s01\" class=\"section\" lang=\"en\">\n<div id=\"ball-ch11_s01_n04\" class=\"key_takeaways editable block\">\n<div class=\"bcc-box bcc-success\">\n<h3>Key Takeaways<\/h3>\n<ul id=\"ball-ch11_s01_l02\" class=\"itemizedlist\">\n<li>Solutions are composed of a solvent (major component) and a solute (minor component).<\/li>\n<li>Concentration is the expression of the amount of solute in a given amount of solvent and can be described by several qualitative terms.<\/li>\n<li>Solubility is a specific amount of solute that can dissolve in a given amount of solvent.<\/li>\n<\/ul>\n<\/div>\n<div class=\"bcc-box bcc-info\">\n<h3>Exercises<\/h3>\n<div id=\"ball-ch11_s01_qs01\" class=\"qandaset block\">\n<ol id=\"ball-ch11_s01_qs01_qd01\" class=\"qandadiv\">\n<li id=\"ball-ch11_s01_qs01_qd01_qa01\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch11_s01_qs01_p01\" class=\"para\">Define <em class=\"emphasis\">solute<\/em> and <em class=\"emphasis\">solvent<\/em>.<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch11_s01_qs01_qd01_qa02\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch11_s01_qs01_p03\" class=\"para\">Define <em class=\"emphasis\">saturated<\/em>, <em class=\"emphasis\">unsaturated<\/em>, and <em class=\"emphasis\">supersaturated<\/em>.<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch11_s01_qs01_qd01_qa03\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch11_s01_qs01_p05\" class=\"para\">A solution is prepared by combining 2.09 g of CO<sub class=\"subscript\">2<\/sub> and 35.5 g of H<sub class=\"subscript\">2<\/sub>O. Identify the solute and solvent.<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch11_s01_qs01_qd01_qa04\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch11_s01_qs01_p07\" class=\"para\">A solution is prepared by combining 10.3 g of Hg(\u2113) and 45.0 g of Ag(s). Identify the solute and solvent.<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch11_s01_qs01_qd01_qa05\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch11_s01_qs01_p09\" class=\"para\">Use\u00a0 Table 1 to decide if a solution containing 45.0 g of NaCl per 100 g of H<sub class=\"subscript\">2<\/sub>O is unsaturated, saturated, or supersaturated.<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch11_s01_qs01_qd01_qa06\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch11_s01_qs01_p11\" class=\"para\">Use Table 1 to decide if a solution containing 0.000092 g of AgCl per 100 g of H<sub class=\"subscript\">2<\/sub>O is unsaturated, saturated, or supersaturated.<\/p>\n<\/div>\n<\/li>\n<\/ol>\n<div class=\"question\"><\/div>\n<\/div>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q6525754\">Show Select Answers<\/span><\/p>\n<div id=\"q6525754\" class=\"hidden-answer\" style=\"display: none\">\n<p>1. The solvent is the majority component of a solution, whereas the solute is the minority component of a solution.<\/p>\n<p>3. solute: CO<sub class=\"subscript\">2<\/sub>; solvent: H<sub class=\"subscript\">2<\/sub>O<\/p>\n<p>5. supersaturated<\/p>\n<\/div>\n<\/div>\n<\/div>\n<h2>Glossary<\/h2>\n<p><strong>dissociation: <\/strong>physical process accompanying the dissolution of an ionic compound in which the compound\u2019s constituent ions are solvated and dispersed throughout the solution<\/p>\n<p><strong>electrolyte: <\/strong>substance that produces ions when dissolved in water<\/p>\n<p><strong>nonelectrolyte: <\/strong>substance that does not produce ions when dissolved in water<\/p>\n<p><strong>saturated: <\/strong>of concentration equal to solubility; containing the maximum concentration of solute possible for a given temperature and pressure<\/p>\n<p><strong>solubility: <\/strong>maximum concentration of a solute that may be achieved at a given temperature and pressure<\/p>\n<p><strong>strong electrolyte: <\/strong>substance that dissociates or ionizes completely when dissolved in water<\/p>\n<p><strong>supersaturated: <\/strong>of concentration that exceeds solubility; a nonequilibrium state<\/p>\n<p><strong>unsaturated: <\/strong>of concentration less than solubility<\/p>\n<p><strong>weak electrolyte: <\/strong>substance that ionizes only partially when dissolved in water<\/p>\n<\/div>\n<\/div>\n\n\t\t\t <section class=\"citations-section\" role=\"contentinfo\">\n\t\t\t <h3>Candela Citations<\/h3>\n\t\t\t\t\t <div>\n\t\t\t\t\t\t <div id=\"citation-list-582\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Shared previously<\/div><ul class=\"citation-list\"><li>Introductory Chemistry- 1st Canadian Edition . <strong>Authored by<\/strong>: Jessie A. Key and David W. Ball. <strong>Provided by<\/strong>: BCCampus. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/opentextbc.ca\/introductorychemistry\/\">https:\/\/opentextbc.ca\/introductorychemistry\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc-sa\/4.0\/\">CC BY-NC-SA: Attribution-NonCommercial-ShareAlike<\/a><\/em>. <strong>License Terms<\/strong>: Download this book for free at http:\/\/open.bccampus.ca<\/li><li>Chemistry. <strong>Provided by<\/strong>: OpenStaxCollege. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/openstaxcollege.org\">http:\/\/openstaxcollege.org<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY: Attribution<\/a><\/em>. <strong>License Terms<\/strong>: Download for free at https:\/\/openstaxcollege.org\/textbooks\/chemistry\/get<\/li><\/ul><\/div>\n\t\t\t\t\t\t <\/div>\n\t\t\t\t\t <\/div>\n\t\t\t <\/section><hr class=\"before-footnotes clear\" \/><div class=\"footnotes\"><ol><li id=\"footnote-582-1\">If bubbles of gas are observed within the liquid, the mixture is not homogeneous and, thus, not a solution. <a href=\"#return-footnote-582-1\" class=\"return-footnote\" aria-label=\"Return to footnote 1\">&crarr;<\/a><\/li><\/ol><\/div>","protected":false},"author":23485,"menu_order":1,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Introductory Chemistry- 1st Canadian Edition \",\"author\":\"Jessie A. 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