MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) All of the following statements describing solutions are true except A) Solutions are homogeneous. B) Making a solution involves a physical change. C) Solutions are colorless. D) The particles in a solution are atomic or molecular in size. E) Solutions are transparent. 1) 2) Which homogeneous mixture is opaque and has particles large enough to be filtered? A) solution B) suspension C) colloid D) both colloids and suspensions 2) 3) Which is not an example of a solution? A) the mixture of gases in a SCUBA diving tank B) antifreeze in a car radiator C) spring water purchased at a supermarket D) a coin made from nickel and copper 3) 4) The number of components in a solution is A) 3 B) at least 2. C) 5 D) 6 E) 4 4) 5) Which of the following cannot serve as the solvent in a solution? A) a gas B) a liquid C) a mixture of comingled liquids D) a solid E) all of the above 5) 6) In a mixture of 5 ml water, 10 ml alcohol, and 50 ml acetone the solvent(s) is(are). A) acetone and alcohol B) alcohol and water C) water D) alcohol E) acetone 6) 1

7) Which statement best explains the meaning of the phrase ʺlike dissolves likeʺ? A) A solvent will easily dissolve a solute of similar mass. B) A solvent and solute with similar intermolecular forces will readily form a solution. C) The only true solutions are formed when water dissolves a polar solute. D) The only true solutions are formed when water dissolves a non-polar solute. E) None of these statements is correct. 7) 8) When a solid dissolves, each molecule is removed from the crystal by interaction with the solvent. This process of surrounding each ion with solvent molecules is called 8) A) dilution. B) hemolysis. C) crenation. D) electrolysis. E) solvation. 9) Water can be used to dissolve which type of compounds A) nonpolar compounds B) polar compounds C) ionic compounds D) both A and B E) both B and C 9) 10) The dissolving process is exothermic when A) The energy released in solvation is about the same as the energy used in breaking up solute-solute and solvent-solvent interactions. B) the energy released in solvation exceeds the energy used in breaking up solute-solute and solvent-solvent interactions. C) The energy used in solvation is less than the energy released in breaking up solute-solute and solvent-solvent interactions. D) The energy used in solvation is about the same as the energy released in breaking up solute-solute and solvent-solvent interactions. E) The energy used in solvation exceeds the energy released in breaking up solute-solute and solvent-solvent interactions. 10) 2

11) Consider the following four liquids: 1. water: highly polar; H-bonding 2. hexanol: slightly polar; some H-bonding 3. chloroform: slightly polar; no H-bonding 4. octane: non-polar; no H-bonding Which pair of liquids is immiscible? 11) A) water and hexanol B) chloroform and octane C) hexanol and chloroform D) water and octane 12) A substance represented by a formula written as MxLOy zh2o is called a 12) A) colloid. B) solid hydrate. C) suspension. D) solvent. E) solute. 13) An ionic compounded that attracts atmospheric water strongly is said to be A) soluble. B) immiscible. C) miscible. D) diluted. E) hygroscopic. 13) 14) The term miscable is used to describe which type of solution A) liquid/liquid B) liquid/solid C) gas/gas D) gas/liquid E) all of the above 14) 3

15) Which statement about solubility is not true? A) A supersaturated solution is unstable. B) In a solution containing excess solute, an equilibrium exists between dissolved and undissolved solute. C) Solubility of ionic solids increases greatly with temperature. D) No additional solute will dissolve in a saturated solution. E) The solubility of substances is measured as g solute/100 ml solvent. 15) 16) Which of the following statements about the solubility of gases in liquids is not correct? A) A solution stored under an atmosphere of pure nitrogen will contain more dissolved nitrogen than the same solution stored under air because air is only 80% nitrogen. B) A warm can of soda fizzes more than a cold can of soda when opened because gases are less soluble at higher temperature. C) An opened can of soda goes ʺflatʺ because the partial pressure of carbon dioxide is lower in the atmosphere than in the unopened can. D) Fish kills may occur in the summertime because an inadequate amount of oxygen is dissolved in the water. 16) 17) The solubility of gases in liquids A) increases as temperature increases and increases as pressure increases B) increases as temperature increases and decreases as pressure increases C) decreases as temperature increases and increases as pressure increases D) is independent of temperature and increases as pressure increases E) decreases as temperature increases and decreases as pressure increases 17) 18) The solubility of nitrogen in water exposed to the atmosphere, where the partial pressure of nitrogen is 593 mm, is 5.3 10-4 M. At the same temperature, what would be the solubility of pure nitrogen, at a pressure of 760 mm? A) 2400 M B) 1500 M C) 4.1 10-4 M D) 6.8 10-4 M 18) 4

19) All of the statements about molarity are correct except A) The molarity of a diluted solution is less than the molarity of the original solution. B) The abbreviation is M. C) The interpretation of the symbol is ʺmoles of solute per mole of solvent.ʺ D) moles = molarity volume E) volume = moles/molarity 19) 20) How many grams of NaOH are needed to make 750 ml of a 2.5% (w/v) solution? A) 20 g B) 7.5 g C) 19 g D) 3.9 g E) 50 g 20) 21) How much NaCl is needed to make 75 ml of a 12% (w/v) solution? A) 9.0 g B) 6.0 g C) 12 g D) 7.5 g E) 30 g 21) 22) What is the % (w/v) concentration of a solution containing 12 grams of solute in 400 ml of solution? 22) A) 12% B) 6.0% C) 3.0% D) 4.0% E) 1.2% 23) What is the % (w/v) concentration of a solution containing 25.0 g of solute in 400. ml of solution? A) 12.5% B) 6.25% C) 2.50% D) 5.00% E) 25.0% 23) 24) What is the % (w/v) concentration of a solution containing 8.0 grams of alcohol in 50.0 ml of solution? 24) A) 4.0% B) 50% C) 8.0% D) 16% E) 2.0% 25) How much NaOH is present in a 250 ml sample of a 5.00% (w/v) solution? A) 250 g B) 10.0 g C) 5.00 g D) 25.0 g E) 12.5 g 25) 26) How much NaOH is present in a 75.0 ml sample of a 5.00% (w/v) solution? A) 75.0 g B) 5.00 g C) 15.0 g D) 6.67 g E) 3.75 g 26) 27) How much NaCl is present in a 15.0 ml sample of a 12.0% (w/v) solution? A) 1.25 g B) 15.0 g C) 0.800 g D) 1.80 g E) 12.0 g 27) 28) How much NaCl is present in 25.0 ml of a 12.0% (w/v) solution? A) 6.00 g B) 12.0 g C) 3.00 g D) 4.00 g E) 48.0 g 28) 29) How many g of NaOH is needed to make 350. ml of a 2.5% (w/v) solution? A) 100. g B) 21.9 g C) 8.75 g D) 6.25 g E) 35.0 g 29) 5

30) How much NaCl is needed to make 50.0 ml of a 16% (w/v) solution? A) 2.0 g B) 8.0 g C) 4.0 g D) 12 g E) 16 g 30) 31) Which solution is the most concentrated? Each choice refers to the same solute and solvent. A) 30 g solute in 150 ml solution B) 2.4 g solute in 2 ml solution C) 50 g solute in 175 ml solution D) 20 g solute in 50 ml solution E) 2.4 g solute in 5 ml solution 31) 32) Which solution is the least concentrated? Each choice refers to the same solute and solvent. A) 20 g solute in 50 ml solution B) 2.4 g solute in 5 ml solution C) 30 g solute in 150 ml solution D) 2.4 g solute in 2 ml solution E) 50 g solute in 175 ml solution 32) 33) Which information is necessary to determine the molarity of a solution if the chemical formula of the solute is known? 33) A) the molar mass of both the solute and the solvent used B) only the volume of solvent used C) the mass of solute dissolved and the final volume of the solution D) only the mass of solute dissolved E) the mass of solute dissolved and the volume of solvent added 34) What is the molarity of a solution prepared by dissolving 3.50 mol NaCl in enough water to make 1.50 L of solution? 34) A) 5.25 M B) 2.33 M C) 0.429 M D) 87.8 M E) 137 M 35) What is the molarity of a solution prepared by dissolving 0.750 mol CaCl2 in enough water to make 0.500 L of solution? A) 0.667 M B) 1.50 M C) 83.2 M D) 0.375 M E) 166.5 M 35) 36) What is the molarity of a solution prepared by dissolving 10.0 g of acetone, C3H6O, in enough water to make 125 ml of solution? A) 0.0465 M B) 0.0125 M C) 1.38 M D) 0.0214 M E) 4.65 M 36) 6

37) What is the molarity of a solution prepared by dissolving 10.0 g of acetone, C3H6O, in enough water to make 250. ml of solution? A) 0.250 M B) 0.0430 M C) 0.689 M D) 0.172 M E) 0.0160 M 37) 38) What is the molarity of a solution prepared by dissolving 48.0 g of NaOH in enough water to make 1.50 L of solution? 38) A) 32.0 M B) 1.28 M C) 0.556 M D) 0.800 M E) 0.0313 M 39) What is the molarity of a solution prepared by dissolving 36.0 g of NaOH in enough water to make 1.50 L of solution? 39) A) 0.900 M B) 0.0428 M C) 1.35 M D) 0.600 M E) 0.0240 M 40) What is the molarity of a solution prepared by dissolving 1.25 mol of AgNO3 in enough water to make 625 ml of solution? A) 2.00 M B) 0.00200 M C) 0.0118 M D) 0.340 M E) 0.500 M 40) 41) What is the molarity of a solution prepared by dissolving 1.25 mol AgNO3 in enough water to make 2.00 103 ml of solution? A) 0.106 M B) 0.00250 M C) 1.25 M D) 0.625 M E) 2.50 M 41) 42) How many moles of HCl are present in 75.0 ml of a 0.200 M solution? A) 2.67 mol B) 0.375 mol C) 0.275 mol D) 0.0150 mol E) 15.0 mol 42) 43) How many moles of HCl are present in 35.5 ml of a 0.200 M solution? A) 0.178 mol B) 0.00710 mol C) 0.974 mol D) 0.236 mol E) 0.195 mol 43) 44) How many moles of solute are present in 12.0 L of 3.00 M HCl? A) 0.750 mol B) 36.0 mol C) 0.250 mol D) 3.00 mol E) 4.00 mol 44) 45) How many moles of solute are present in 5.00 L of 6.00 M HCl? A) 30.0 mol B) 5.00 mol C) 1.20 mol D) 6.00 mol E) 0.833 mol 45) 7

46) Normal saline is 0.92% (w/v) NaCl in water. How many grams of NaCl are needed to prepare 15.0 L of normal saline? 46) A) 1.38 g B) 16.3 g C) 138 g D) 807 g E) 53.8 g 47) How many g of C6H12O6 are needed to prepare 2.5 L of a 5.00% (w/v) solution? 47) A) 125 g B) 0.200 g C) 12.5 g D) 200. g E) 1.25 g 48) How many ml of a 5.00% (w/v) glucose solution are needed to provide 20.0 g of glucose? A) 4.00 ml B) 5.00 ml C) 200 ml D) 400 ml E) 20.0 ml 48) 49) Calculate the concentration in ppm of a pollutant that has been measured at 450 mg per 150 kg of sample. 49) A) 3000 ppm B) 6 ppm C) 3 ppm D) 330 ppm 50) How many ml of 0.105 M AgNO3 are needed for an experiment that requires 0.00510 mol of AgNO3? 50) A) 18.70 ml B) 17.8 ml C) 20.6 ml D) 48.6 ml E) 0.536 ml 51) Which list includes all the pieces of lab equipment needed to prepare a 0.500 M solution of NaCl from the pure salt and water? 51) A) buret; volumetric flask B) volumetric pipet and bulb; volumetric flask C) buret; electronic balance D) electronic balance; graduated cylinder E) electronic balance; volumetric flask 52) Which list includes all the pieces of lab equipment needed to prepare 0.100 M H3PO4 from a 5.00 M solution of H3PO4? 52) A) buret; electronic balance B) buret; volumetric flask C) electronic balance; graduated cylinder D) electronic balance; volumetric flask E) volumetric pipet and bulb; volumetric flask 8

53) How many grams of FeSO4 are present in a 20 ml sample of a 0.500 M solution? 53) A) 6.08 g B) 3.04 g C) 0.760 g D) 65.8 g E) 1.52 g 54) How many g of Fe(NO3)3 are present in a 20.0 ml sample of a 0.500 M solution? 54) A) 4.84 g B) 2.14 g C) 9.68 g D) 2.42 g E) 1.21 g 55) How many grams of CaCl2 are needed to prepare 125 ml of a 1.50 M solution? 55) A) 1.69 g B) 20.8 g C) 0.188 g D) 37.0 g E) 3.00 g 56) How many g of CaCl2 are needed to prepare 500. ml of a 0.375 M solution? 56) A) 1.69 g B) 3.00 g C) 37.0 g D) 0.188 g E) 20.8 g 57) All of the water in a 0.200 M solution of NaCl was evaporated and 0.150 mole of NaCl was obtained. What was the original volume of the sample? 57) A) 1000 ml (1.00 103 ml) B) 30.0 ml C) 1330 ml D) 750. ml E) 333 ml 58) A 20.0 ml sample of CuSO4 was evaporated to dryness, leaving 0.967 g of residue. What was the molarity of the original solution? A) 0.303 M B) 0.0484 M C) 0.0207 M D) 0.433 M E) 48.4 M 58) 59) How many ml of a 0.200 M KOH solution contains 10.0 g of KOH? A) 11.2 ml B) 281 ml C) 178 ml D) 50.0 ml E) 891 ml 59) 60) How many ml of a 0.200 M HNO3 solution contains 10.0 g of HNO3? 60) A) 2.00 ml B) 159 ml C) 793 ml D) 315 ml E) 31.7 ml 61) How many grams of water are needed to prepare 250 g of a solution that is 5.00% by mass NaCl? A) 5.00 g B) 245 g C) 12.5 g D) 238 g E) 1250 g 61) 9

62) Which procedure will produce 250 ml of a solution that is 4% by volume alcohol in water? A) 10 ml of alcohol is mixed with enough water to make 250 ml of solution. B) 10 ml of alcohol is mixed with 250 ml of water. C) 4 ml of alcohol is mixed with enough water to make 250 ml of solution. D) 4 ml of alcohol is mixed with 250 ml of water. 62) 63) A 50.0 ml sample of a 6.0 M solution of HCl is diluted to 200 ml. What is the new concentration? A) 1.50 M B) 2.00 M C) 6.0 M D) 2.10 M E) 24.0 M 63) 64) What is the final concentration of a solution prepared by adding water to 50.0 ml of 1.5 M NaOH to make 1.00 L of solution? 64) A) 30 M B) 0.030 M C) 7.5 M D) 1.5 M E) 0.075 M 65) A 50.0 ml sample of a 12.0 M solution of HCl is diluted to 250. ml. What is the new concentration? 65) A) 2.40 M B) 10.4 M C) 60.0 M D) 3.00 M E) 12.0 M 66) What is the final concentration if 100 ml of water is added to 25.0 ml of 6.0 M NaCl? A) 1.5 M B) 24 M C) 6.0 M D) 1.2 M E) 30 M 66) 67) How many ml of 16 M NH3 are needed to prepare 2.0 L of a 2.0 M solution? 67) A) 125 ml B) 16 ml C) 250 ml D) 4.0 ml E) 8.0 ml 68) How many ml of 14.5 M NH3 are needed to prepare 2.0 L of a 1.0 M solution? 68) A) 276 ml B) 7.25 ml C) 69.0 ml D) 29.0 ml E) 138 ml 69) How many ml of water should be added to 50.0 ml of a 15.0 M H2SO4 solution to give a final concentration of 0.300 M? A) 2550 ml B) 950 ml C) 2450 ml D) 1000 ml E) 2500 ml 69) 70) What is the final concentration of a solution prepared by using 75.0 ml of 18.0 M H2SO4 to prepare 500. ml of solution? A) 15.7 M B) 2.35 M C) 2.70 M D) 8.33 10-3 M E) 1.20 M 70) 10

71) Which substance is not an electrolyte? 71) A) KOH B) HCl C) NH4NO3 D) NaCl E) CH4 72) Considering 1.0 M solutions of each substance, which contains the largest concentration of ions? A) FeCl3 B) K2SO4 C) NH3 D) KCl E) NaOH 72) 73) Considering 0.1 M solutions of each substance, which contains the smallest concentration of ions? 73) A) (NH4)3PO4 B) Na2SO4 C) FeSO4 D) Ca(NO3)2 E) K2CO3 74) How many grams are contained in one equivalent of iron (III) ion, Fe3+? A) 55.85 g B) 167.6 g C) 0.0537 g D) 18.62 g E) 6.02 x 1023 g 74) 75) How many grams are in 10.0 meq of Ca2+? A) 0.401 g B) 0.201 g C) 20.1 g D) 0.802 g E) 40.1 g 75) 76) How many g in 10.0 meq of Mg2+? A) 0.243 g B) 0.486 g C) 12.3 g D) 0.122 g E) 24.3 g 76) 77) How many milliequivalents of chloride ion are contained in a sample that is determined to contain 0.725 g of chloride ion? 77) A) 48.9 meq B) 10.3 meq C) 41.0 meq D) 25.7 meq E) 20.5 meq 78) If a normal blood sample contains 4.5 meq/l of calcium ion, how many mg of calcium are contained in a 25.0 ml blood sample? 78) A) 9.0 mg B) 1.4 mg C) 2.3 mg D) 2.8 mg E) 5.6 mg 11

79) Which statement comparing solutions with pure solvents is not correct? A) A solution will have a greater mass than an equal volume of pure solvent if the solute has a molar mass greater than the solvent. B) A solution containing a non-volatile solute has a lower vapor pressure than pure solvent. C) A solution containing a non-volatile solute has a lower boiling point than pure solvent. D) A solution containing a non-volatile solute has a lower freezing point than pure solvent. 79) 80) The passage of a solvent across a semipermeable membrane because of concentration differences is called 80) A) hemolysis. B) osmosis. 81) What is the osmolarity of a 0.20 M solution of KCl? A) 0.10 Osmol B) 0.30 Osmol C) 0.40 Osmol D) 0.20 Osmol E) 0.80 Osmol 81) 82) Red blood cells are placed in a solution and neither hemolysis nor crenation occurs. Therefore the solution is 82) A) isotopic. B) isotonic. C) hypertonic. D) concentrated. E) hypotonic. 83) Which has the highest boiling point? A) pure water 83) B) 0.1 M Al(NO3)3 C) 0.1 M Na2SO4 D) 0.1 M MgCl2 E) 0.1 M glucose, C6H12O6 12

84) Which has the lowest boiling point? 84) A) 0.1 M Na2SO4 B) 0.1 M Al(NO3)3 C) pure water D) 0.1 M glucose, C6H12O6 E) 0.1 M MgCl2 85) If ʺAʺ contains 2% NaCl and is separated by a semipermeable membrane from ʺBʺ which contains 10% NaCl, which event will occur? 85) A) NaCl will flow from ʺAʺ to ʺBʺ. B) NaCl will flow from ʺBʺ to ʺAʺ. C) Water will flow from ʺBʺ to ʺAʺ. D) Water will flow from ʺAʺ to ʺBʺ. 86) Which solution will have the highest boiling point? 86) A) 0.10 M C6H12C6 B) 0.050 M KNO3 C) 0.075 M CaCl2 D) 0.020 M Na3PO4 E) 0.025 M NH4NO3 87) Which solution will have the lowest boiling point? 87) A) 0.10 M C6H12C6 B) 0.025 M NH4NO3 C) 0.050 M KNO3 D) 0.020 M Na3PO4 E) 0.075 M CaCl2 MATCHING. Choose the item in column 2 that best matches each item in column 1. Match the following. 88) hydrate 89) hygroscopic A) an ionic compound which attracts water molecules from the atmosphere B) an ionic compound which holds water molecules within its crystalline structure 88) 89) 13

90) saturated 91) unsaturated 92) supersaturated 93) weak electrolyte 94) non-electrolyte 95) hypotonic 96) strong electrolyte A) a substance which does not dissociate in solution and therefore does not conduct electricity B) a solution in which more solute is dissolved than predicted for that particular temperature. C) a solution in which no more solute will dissolve and in which excess solute is visible in the container. D) the shrinking of a red blood cell when placed in a solution of greater osmolarity than the cell itself 90) 91) 92) 93) 94) 95) 96) 97) hemolysis 98) hypertonic 99) crenation 100) isotonic E) a substance which partially dissociates in solution, providing a relatively small number of ions to conduct electricity F) refers to a solution having a greater osmolarity than 0.30 Osmol, the osmolarity of normal red blood cells G) a solution in which more solute can be dissolved. 97) 98) 99) 100) H) refers to two solutions having the same osmolarity I) the swelling and bursting of a red blood cell when placed in a solution of lower osmolarity than the cell itself J) a substance which dissociates completely in solution, providing a relatively large number of ions to conduct electricity K) refers to a solution having a lower osmolarity than 30.0 Osmol, the osmolarity of blood serum 14

Answer Key Testname: UNTITLED8 1) C 2) B 3) E 4) B 5) E 6) E 7) B 8) E 9) E 10) B 11) D 12) B 13) E 14) A 15) C 16) E 17) C 18) D 19) C 20) C 21) A 22) C 23) B 24) D 25) E 26) E 27) D 28) C 29) C 30) B 31) B 32) C 33) C 34) B 35) B 36) C 37) C 38) D 39) D 40) A 41) D 42) D 43) B 44) B 45) A 46) C 47) A 48) D 49) C 50) D 15

Answer Key Testname: UNTITLED8 51) E 52) E 53) E 54) D 55) B 56) E 57) D 58) A 59) E 60) C 61) D 62) A 63) A 64) E 65) A 66) D 67) C 68) E 69) C 70) C 71) E 72) A 73) C 74) D 75) B 76) D 77) E 78) C 79) C 80) B 81) C 82) B 83) B 84) C 85) D 86) C 87) B 88) B 89) A 90) C 91) G 92) B 93) E 94) A 95) K 96) J 97) I 98) F 99) D 100) H 16