{"id":6558,"date":"2020-12-07T18:18:28","date_gmt":"2020-12-07T18:18:28","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/?post_type=chapter&#038;p=6558"},"modified":"2021-01-15T17:48:30","modified_gmt":"2021-01-15T17:48:30","slug":"assignment-11","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/chapter\/assignment-11\/","title":{"raw":"Assignment: 11","rendered":"Assignment: 11"},"content":{"raw":"<ul>\r\n \t<li>1) Predict whether each of these substance would be more soluble in water (polar solvent) or benzene (nonpolar solvent)\r\n<ol>\r\n \t<li>Olive oil (non polar)<\/li>\r\n \t<li>Ethanol or grain alcohol ( polar)<\/li>\r\n \t<li>Table Salt or NaCl (ionic)<\/li>\r\n \t<li>Sugar (Polar covalent)<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>2) Compare the processes that occur when potassium chloride, barium hydroxide and hydrobromic acid (HBr) dissolve in water. Write out the equation and make a sketch of what is happening.<\/li>\r\n \t<li>3) What is the expected conductivity of electricity of each of these substances?\r\n<ol>\r\n \t<li>Acetic acid (Vinegar)<\/li>\r\n \t<li>Butane (C<sub>4<\/sub>H<sub>8<\/sub>)<\/li>\r\n \t<li>Ammonia (NH<sub>3<\/sub>)<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>4) At standard pressure (1 atm) and 0\u00b0C, diatomic oxygen (O<sub>2<\/sub>) can dissolve in water at a rate of 0.70 g\/ 1 L of water. At the same temperature, but at a new pressure of 0.25 atm, how much oxygen can dissolve in water?<\/li>\r\n \t<li>5) Calculate mole fraction for each of these solutes and solvents:\r\n<ol>\r\n \t<li>120 g of NH<sub>4<\/sub>NO<sub>3<\/sub> in 300 g of water<\/li>\r\n \t<li>25g of Br<sub>2<\/sub> in 150 g of ethanol, C<sub>2<\/sub>H<sub>5<\/sub>OH<\/li>\r\n \t<li>25g of NaCl in dichloromethane, CH<sub>2<\/sub>Cl<sub>2<\/sub><\/li>\r\n \t<li>Methanol, Ethanol and water in a solution that is 35% methanol, 40% Ethanol and 15% water<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>6) Practice calculating molarity:\r\n<ol>\r\n \t<li>875 g of H<sub>2<\/sub>SO<sub>4<\/sub> in 2kg of water<\/li>\r\n \t<li>Cyanic acid (HCN) in a solution that is 74% HCN by mass<\/li>\r\n \t<li>A 26% solution (mass) of potassium carbonate (K<sub>2<\/sub>CO<sub>3<\/sub>) with a density of 1.09 g\/cm3.<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>7) Predict which compound would depress freezing point the most, and explain why:\r\n<ol>\r\n \t<li>NaCl<\/li>\r\n \t<li>Glucose<\/li>\r\n \t<li>Na<sub>2<\/sub>CO<sub>3<\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>8) If a solution of MgBr<sub>2<\/sub> in water freezes at -1.28\u00b0C, what is the boiling point of the solution?. Assume ideal solution behavior.<\/li>\r\n \t<li>9) Explain two major differences between colloids and solutions.<\/li>\r\n \t<li>10) How would you prepare a 4.5 <em>m<\/em> aqueous solution of glycerol (C<sub>3<\/sub>H<sub>8<\/sub>O<sub>3<\/sub>)? Calculate freezing point for this solution. This is often used by scientists to freeze bacteria- why might this molecule be a good choice?<\/li>\r\n<\/ul>","rendered":"<ul>\n<li>1) Predict whether each of these substance would be more soluble in water (polar solvent) or benzene (nonpolar solvent)\n<ol>\n<li>Olive oil (non polar)<\/li>\n<li>Ethanol or grain alcohol ( polar)<\/li>\n<li>Table Salt or NaCl (ionic)<\/li>\n<li>Sugar (Polar covalent)<\/li>\n<\/ol>\n<\/li>\n<li>2) Compare the processes that occur when potassium chloride, barium hydroxide and hydrobromic acid (HBr) dissolve in water. Write out the equation and make a sketch of what is happening.<\/li>\n<li>3) What is the expected conductivity of electricity of each of these substances?\n<ol>\n<li>Acetic acid (Vinegar)<\/li>\n<li>Butane (C<sub>4<\/sub>H<sub>8<\/sub>)<\/li>\n<li>Ammonia (NH<sub>3<\/sub>)<\/li>\n<\/ol>\n<\/li>\n<li>4) At standard pressure (1 atm) and 0\u00b0C, diatomic oxygen (O<sub>2<\/sub>) can dissolve in water at a rate of 0.70 g\/ 1 L of water. At the same temperature, but at a new pressure of 0.25 atm, how much oxygen can dissolve in water?<\/li>\n<li>5) Calculate mole fraction for each of these solutes and solvents:\n<ol>\n<li>120 g of NH<sub>4<\/sub>NO<sub>3<\/sub> in 300 g of water<\/li>\n<li>25g of Br<sub>2<\/sub> in 150 g of ethanol, C<sub>2<\/sub>H<sub>5<\/sub>OH<\/li>\n<li>25g of NaCl in dichloromethane, CH<sub>2<\/sub>Cl<sub>2<\/sub><\/li>\n<li>Methanol, Ethanol and water in a solution that is 35% methanol, 40% Ethanol and 15% water<\/li>\n<\/ol>\n<\/li>\n<li>6) Practice calculating molarity:\n<ol>\n<li>875 g of H<sub>2<\/sub>SO<sub>4<\/sub> in 2kg of water<\/li>\n<li>Cyanic acid (HCN) in a solution that is 74% HCN by mass<\/li>\n<li>A 26% solution (mass) of potassium carbonate (K<sub>2<\/sub>CO<sub>3<\/sub>) with a density of 1.09 g\/cm3.<\/li>\n<\/ol>\n<\/li>\n<li>7) Predict which compound would depress freezing point the most, and explain why:\n<ol>\n<li>NaCl<\/li>\n<li>Glucose<\/li>\n<li>Na<sub>2<\/sub>CO<sub>3<\/sub><\/li>\n<\/ol>\n<\/li>\n<li>8) If a solution of MgBr<sub>2<\/sub> in water freezes at -1.28\u00b0C, what is the boiling point of the solution?. Assume ideal solution behavior.<\/li>\n<li>9) Explain two major differences between colloids and solutions.<\/li>\n<li>10) How would you prepare a 4.5 <em>m<\/em> aqueous solution of glycerol (C<sub>3<\/sub>H<sub>8<\/sub>O<sub>3<\/sub>)? Calculate freezing point for this solution. This is often used by scientists to freeze bacteria- why might this molecule be a good choice?<\/li>\n<\/ul>\n","protected":false},"author":17533,"menu_order":9,"template":"","meta":{"_candela_citation":"[]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-6558","chapter","type-chapter","status-publish","hentry"],"part":2995,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters\/6558","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/users\/17533"}],"version-history":[{"count":4,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters\/6558\/revisions"}],"predecessor-version":[{"id":8151,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters\/6558\/revisions\/8151"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/parts\/2995"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters\/6558\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/media?parent=6558"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapter-type?post=6558"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/contributor?post=6558"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/license?post=6558"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}