MR. SURRETTE VAN NUYS HIGH SCHOOL CHAPTER 10: CHEMICAL SOLUTIONS WORKSHEET SOLUTIONS 1. Chemical solutions are __________ mixtures of solute and solvent. 1A. homogenous 2. Two or more substances homogenously combined together is a: 2A. solution 3. Gas solutions consist of __________ dissolved in __________ . 3A. gases gases 4. The __________ is the substance least present in a solution. 4A. solute 5. Methanol dissolves best in __________ solutions. 5A. polar 6. The __________ is the substance most present in a solution. 6A. solvent 7. Rock candy is a good example of a __________ solution. 7A. supersaturated 8. Carbon dioxide in soda is an example of a __________ solution. 8A. liquid-gas 9. __________ solutions have a high solute percentage. 9A. Concentrated 10. Solutes __________ by separating into ions or molecules. 10A. dissolve 11. The solubility of most solutions is greatly affected by: 11A. temperature 12. Calculate the % mass of 14.7 grams sucrose dissolved in 412.1 mL water. 12A. (1) 412.1 mL water = 412.1 g water (2) mass of solvent = 412.1 g (3) mass of solute = 14.7 g (4) mass of solution = mass of solute + mass of solvent (5) mass of solution = 14.7 g + 412.1 g (6) mass of solution = 426.8 grams (7) % mass = (mass solute / mass solution) x 100 1|Page CHEMISTRY MR. SURRETTE VAN NUYS HIGH SCHOOL 12A. (continued...) (8) % mass = (14.7 g / 426.8 g) x 100 (9) % mass = 3.44% 13. Soda is 9.5% sucrose. What volume of soda in mL contains 72.7 g sucrose? (Assume the density of soda = (WATER). 13A. (1) 9.5 % sucrose = (9.5 g sucrose / 100 mL) (2) 72.7 g sucrose (100 mL soda) V = ------------------- x ------------------1 (9.5 g sucrose) (3) Volume = 765.3 mL 14. Soda is 9.5% sucrose. How many grams of sucrose are found in 355 mL of soda? 14A. (1) 9.5% sucrose = (9.5 g sucrose / 100 mL soda) (2) 355 mL (9.5 g sucrose) Mass = ----------- x ------------------1 (100 mL) (3) Mass = 33.7 g 15. What is the molarity of a solution that contains 5.5 grams NaCl dissolved in 1.2 liters water? 15A. (1) Na = 22.99 amu (2) Cl = 35.45 amu (3) NaCl = 58.44 g/mol Convert grams NaCl to moles: (4) 5.5 g (1 mol NaCl) NaCl = ------------ x ----------------- = 9.41 x10-2 mol 1 (58.44 g) Compute molarity of solution: (5) (9.41 x10-2 mol) M = -------------------- = 7.84 x 10-2 (1.2 L) 2|Page CHEMISTRY MR. SURRETTE VAN NUYS HIGH SCHOOL 16. How many liters of 0.724 M NaOH solution contain 1.24 moles NaOH? 16A. (1) 0.724 M NaOH = (0.724 mol NaOH / 1 liter) (2) 1.24 mol NaOH (1 liter) Volume = -------------------- x ---------------1 (0.724 mol) (3) Volume = 1.71 L 17. How much 4.0 M NaNO3 is needed to make 0.585 L of 1.2 M NaNO3 solution? 17A. Given: MI = 4.0 M, MF = 1.2 M, VF = 0.585 L Find: VI (1) MIVI = MFVF (2) VI = MFVF / MI (3) VI = (1.2 M)(0.585 L) / (4.0 M) (4) VI = 1.76 x 10-1 L 3|Page CHEMISTRY MR. SURRETTE VAN NUYS HIGH SCHOOL CHAPTER 10: CHEMICAL SOLUTIONS QUIZ SOLUTIONS 1. More solute can dissolve in __________ solutions. 1A. unsaturated 2. Two grams of sugar are added to a sugar water solution and stirred thoroughly. Twenty grams of sugar then form on the bottom of the container. This solution is: 2A. supersaturated 3. Cations and anions in liquid solutions are: 3A. electrolytes 4. By definition, all solutions are: 4A. homogenous 5. Ethyl alcohol dissolves best in __________ solutions. 5A. non-polar 6. Solutes __________ by separating into ions or molecules. 6A. dissolve 7. __________ solutions have a high solute percentage. 7A. Concentrated 8. __________ solutions have a low solute percentage. 8A. Dilute 9. The density of water is: 9A. 1.0 g/ mL 10. Liquid solutions consist of __________ dissolved in liquids. (A) liquids (B) gases (C) solids (D) all of these (E) none of these 11. Pure oxygen in water is an example of a __________ solution. 11A. liquid-gas 12. Unstable solutions that precipitate to the saturation level are: 12A. supersaturated 13. The __________ is the substance most present in a solution. 13A. solvent 4|Page CHEMISTRY MR. SURRETTE VAN NUYS HIGH SCHOOL Questions 14 – 15. An ingot is formed by mixing 102 grams of copper with 112 grams of zinc. 14. What is the percentage of copper based on relative mass? 14A. (1) Mass solution = solute + solvent (2) Mass solution = 102 g + 112 g (3) Mass solution = 214 g For copper: (4) Mass copper / mass solution (5) 102 g / 214 g (6) 0.477 x 100% (7) Cu = 47.7% 15. Re-compute the copper concentration within the ingot using mole fractions. 15A. Moles of zinc: (1) 112 g Zn 1 mole ------------ = 1.71 mole Zn 65.39 g Moles of copper: (2) 102 g Cu 1 mole ----------- = 1.61 mole Cu 63.55 g Total moles: (3) Total moles = Zn moles + Cu moles (4) Total moles = 1.71 moles + 1.61 moles (5) Total moles = 3.32 moles Mole fraction: (6) Cu mole fraction = 1.61 moles / 3.32 moles (7) Cu mole fraction = 0.485 x 100% (8) Cu = 48.5% 16. 231 grams of acetic acid is added to 512 grams of water. What is the molality of acetic acid in the solution? 16A. Molecular weight of acetic acid: (1) 2 x C = 2(12.01 amu) = 24.02 g C (2) 4 x H = 4(1.01 amu) = 4.04 g H (3) 2 x O = 2(16.00 amu) = 32.00 g O ========= CH3COOH molecular weight = 60.06 grams 5|Page CHEMISTRY MR. SURRETTE 16A. (continued…) Moles of acetic acid: (4) 231 g CH3COOH VAN NUYS HIGH SCHOOL 1 mol ----------- = 3.85 mol CH3COOH 60.06 g Molality of acetic acid: (5) 3.85 mol CH3COOH / 0.512 kg water (6) m = 7.51 17. Calculate the relative mass of 19.2 grams potassium fluoride dissolved in 412.1 mL water. 17A. (1) 412.1 mL water = 412.1 g water (2) mass of solvent = 412.1 g (3) mass of solute = 19.2 g (4) mass of solution = mass of solute + mass of solvent (5) mass of solution = 19.2 g + 412.1 g (6) mass of solution = 431.3 grams (7) % mass = (mass solute / mass solution) x 100 (8) % mass = (19.2 g / 431.3 g) x 100 (9) % mass = 4.5% Questions 18 - 19. A solution is 7.5% ethyl alcohol. What volume of solution in mL contains 185.2 g ethyl alcohol? (Assume the density of ethyl alcohol = (WATER). 18A. (1) 7.5 % ethyl alcohol = (7.5 g ethyl alcohol / 100 mL water) (2) 185.2 g ethyl alcohol (100 mL water) Volume = -------------------------- x -----------------------1 (7.5 g ethyl alcohol) (3) Volume = 2469 mL 19. How many grams of ethyl alcohol are found in 355 mL of solution? 19A. (1) 7.5% ethyl alcohol = (7.5 g ethyl alcohol / 100 mL water) (2) 355 mL (7.5 g ethyl alcohol) Mass = ---------- x --------------------------1 (100 mL water) (3) Mass = 26.6 g 6|Page CHEMISTRY MR. SURRETTE VAN NUYS HIGH SCHOOL 20. What is the molarity of a solution that contains 27.2 grams KNO3 dissolved in 0.9 liters water? 20A. (1) KNO3 Molecular Weight: 1 x K = 1 x 39.10 amu = 39.10 g 1 x N = 1 x 14.01 amu = 14.01 g 3 x O = 3 x 16.00 amu = 48.00 g ====== KNO3 = 101.11 g/mol Convert grams KNO3 to moles: (2) KNO3 = 27.2 g (1 mol KNO3 / 101.11 g) (3) NaCl = 2.69 x 10-1 mol Compute molarity of solution: (4) M = (2.69 x 10-1 mol NaCl / 0.9 L) (5) M = 2.99 x 10-1 21. How many liters of 0.154 M Ba(OH)2 solution contain 1.24 moles Ba(OH)2? 21A. (1) 0.154 M = (0.154 mol Ba(OH)2 / 1 liter) (2) 1.24 mol (1 liter) Volume = ------------ x ------------- = 8.05 L 1 (0.154 mol) 22. How much 5.0 M RbNO3 is needed to make 0.585 L of 1.2 M RbNO3 solution? 22A. Given: MI = 5.0 M, MF = 1.2 M, VF = 0.585 L Find: VI (1) MIVI = MF VF (2) VI = MFVF/ MI (3) VI = (1.2 M)(0.585 L) / (5.0 M) (4) VI = 1.40 x 10-1 L 7|Page CHEMISTRY