SOLUTION 3/3/16. Version 2

Transcription

1 3/3/16 NAME ROW PD 51) A gram sample of an aqueous solution contains gram of NH3. What is the concentration of NH3 in the solution, expressed as parts per million? 1) 5.0 ppm 2) 15 ppm 3) 20. ppm 4) 50. ppm 52) According to your Reference Tables, which substance forms an unsaturated solution when 80 grams of the substance is dissolved in 100 grams of H2O at 10 C? 1) KI 2) KNO3 3) NaNO3 4) NaCl 53) A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolved. Which statement best describes the resulting mixture? 1) The mixture is heterogeneous and can be separated by filtration. 2) The mixture is heterogeneous and cannot be separated by filtration. 3) The mixture is homogeneous and cannot be separated by filtration. 4) The mixture is homogeneous and can be separated by filtration. 54) Given the diagram below that shows carbon dioxide in an equilibrium system at a of 298 K and a pressure of 1 atm: Which changes must increase the solubility of the carbon dioxide? 1) decrease pressure and increase 2) increase pressure and decrease 3) increase pressure and increase 4) decrease pressure and decrease 55) A solution consists of 0.50 mole of CaCl2 dissolved in 100. grams of H2O at 25 C. Compared to the boiling point and freezing point of 100. grams of H2O at standard pressure, the solution at standard pressure has 1) a higher boiling point and a lower freezing point 2) a higher boiling point and a higher freezing point 3) a lower boiling point and a higher freezing point 4) a lower boiling point and a lower freezing point

2 56) What occurs when NaCl(s) is added to water? 1) The boiling point of the solution decreases, and the freezing point of the solution decreases. 2) The boiling point of the solution decreases, and the freezing point of the solution increases. 3) The boiling point of the solution increases, and the freezing point of the solution increases. 4) The boiling point of the solution increases, and the freezing point of the solution decreases. 57) Based on Reference Table F, which of these saturated solutions has the lowest concentration of dissolved ions? 1) NiCl2(aq) 2) NaCl(aq) 3) AgCl(aq) 4) MgCl2(aq) 58) Which aqueous solution has the lowest freezing point? 1) 1.0 M CH3COOH 2) 1.0 M C6H12O6 3) 1.0 M C2H5OH 4) 1.0 M NaCl 59) According to Reference Table G, which solution is saturated at 30 C? 1) 30 grams of NaCl in 100 grams of water 2) 30 grams of NaCl in 200 grams of water 3) 12 grams of KClO3 in 200 grams of water 4) 12 grams of KClO3 in 100 grams of water 60) What is the molarity of a solution containing 20 grams of NaOH in 500 milliliters of solution? 1) 0.5 M 2) 1 M 3) 0.04 M 4) 2 M 61) Which compound decreases in solubility as the of the solution is increased from 10ºC to 50ºC? 62) Which of these contains only one substance? 1) saltwater 2) distilled water 3) sugar water 4) rainwater 63) The graph below represents four solubility curves. Which curve best represents the solubility of a gas in water? 1) A 2) B 3) C 4) D 64) What is the concentration of O2(g), in parts per million, in a solution that contains gram of O2(g) dissolved in grams of H2 O(l)? 1) 800 ppm 2) 80 ppm 3) 0.8 ppm 4) 8 ppm 65) When 5 grams of KCl are dissolved in 50. grams of water at 25 C, the resulting mixture can be described as 1) homogeneous and supersaturated 2) heterogeneous and supersaturated 3) heterogeneous and unsaturated 4) homogeneous and unsaturated 1) NH4Cl 2) NH3 3) NaNO3 4) NaCl

3 66) Base your answer to the following question on the diagram below which represents the solubility curve of salt X. The four points on the diagram represent four solutions of salt X. Which point represents the most concentrated solution of salt X? 1) A 2) B 3) C 4) D 67) The attraction between water molecules and an Na + ion or a Cl ion occurs because water molecules are 1) polar 2) symmetrical 3) linear 4) nonpolar 68) Two grams of potassium chloride are completely dissolved in a sample of water in a beaker. This solution is classified as 1) a compound 2) an element 3) a heterogeneous mixture 4) a homogeneous mixture 69) Solubility data for four different salts in water at 60 C are shown in the table below. 70) What is the mass of NH4Cl that must dissolve in 200. grams of water at 50. C to make a saturated solution? 1) 84 g 2) 104 g 3) 42 g 4) 26 g 71) According to Table F, which ions combine with chloride ions to form an insoluble compound? 1) Li + ions 2) Ag + ions 3) Ca 2+ ions 4) Fe 2+ ion 72) According to Reference Table G, which of these substances is most soluble at 60ºC? 1) KClO3 2) NH4Cl 3) KCl 4) NaCl 73) A solute is added to water and a portion of the solute remains undissolved. When equilibrium between the dissolved and undissolved solute is reached, the solution must be 1) supersaturated 2) dilute 3) saturated 4) unsaturated 74) After being thoroughly stirred at 10. C, which mixture is heterogenous? 1) 2) 3) 4) 75) Under which conditions of and pressure is a gas most soluble in water? 1) low and high pressure 2) high and high pressure 3) low and low pressure 4) high and low pressure 76) When 2.00 moles of sugar (C6H12O6) are dissolved in 1,000. grams of water, the boiling point of the resulting solution is closest to 1) 100. C 2) 99.0 C 3) 99.5 C 4) 101 C Which salt is most soluble at 60 C? 1) A 2) B 3) C 4) D

4 77) A sample is prepared by completely dissolving 10.0 grams of NaCl in 1.0 liter of H 2O. Which classification best describes this sample? 1) heterogeneous compound 2) heterogeneous mixture 3) homogeneous mixture 4) homogeneous compound 78) Which 1-molal aqueous solution has the lowest freezing point? 1) 2) 3) 4) 79) The solubility of KCl(s) in water depends on the 1) of the water 2) pressure on the solution 3) size of the KCl sample 4) rate of stirring 80) The solubility of KClO3(s) in water increases as the 1) of the solution increases 2) pressure on the solution increases 3) pressure on the solution decreases 4) of the solution decreases 81) Which barium salt is insoluble in water? 1) Ba(ClO4)2 2) BaCO3 3) Ba(NO3)2 4) BaCl2 82) Which solution has the lowest freezing point? 1) 10. g of KI dissolved in 100. g of water 2) 20. g of KI dissolved in 200. g of water 3) 30. g of KI dissolved in 100. g of water 4) 40. g of KI dissolved in 200. g of water 83) What is the total number of moles of NaCl(s) needed to make 3.0 liters of a 2.0 M NaCl solution? 1) 0.70 mol 2) 8.0 mol 3) 1.0 mol 4) 6.0 mol 84) A student adds solid KCl to water in a flask. The flask is sealed with a stopper and thoroughly shaken until no more solid KCl dissolves. Some solid KCl is still visible in the flask. The solution in the flask is 1) unsaturated and is at equilibrium with the solid KCl 2) saturated and is at equilibrium with the solid KCl 3) unsaturated and is not at equilibrium with the solid KCl 4) saturated and is not at equilibrium with the solid KCl 85) Which of the salts listed below is most soluble at 60ºC? 1) NaNO3 2) KCl 3) KNO3 4) NH4Cl 86) Which compound becomes less soluble in water as the of the solution is increased? 1) NaCl 2) NH4Cl 3) HCl 4) KCl 87) What is the total number of grams of NaI(s) needed to make 1.0 liter of a M solution? 1) ) ) 1.5 4) 15 88) At room, the solubility of which solute in water would be most affected by a change in pressure? 1) sodium nitrate 2) sugar 3) methanol 4) carbon dioxide 89) According to Reference Table G, how many grams of KNO3 would be needed to saturate 200 grams of water at 70ºC? 1) 268 g 2) 43 g 3) 134 g 4) 86 g

5 90) At which can water contain the most dissolved oxygen at a pressure of 1 atmosphere? 1) 10.ºC 2) 20.ºC 3) 30.ºC 4) 40.ºC 91) What is the molarity of 1.5 liters of an aqueous solution that contains 52 grams of lithium fluoride, LiF, (gram-formula mass = 26 grams/mole)? 1) 1.3 M 2) 2.0 M 3) 3.0 M 4) 0.75 M 92) Which compound is least soluble in 100 grams of water at 40 C? 1) KClO3 2) SO2 3) NH4Cl 4) NaCl

6 Answer Key SOLUTIONS 51) 1 52) 1 53) 3 54) 2 55) 1 56) 4 57) 3 58) 4 59) 4 60) 2 61) 2 62) 2 63) 2 64) 4 65) 4 66) 4 67) 1 68) 4 69) 4 70) 2 71) 2 72) 2 73) 3 74) 2 75) 1 76) 4 77) 3 78) 2 79) 1 80) 1 81) 2 82) 3 83) 4 84) 2 85) 1 86) 3 87) 3 88) 4 89) 1 90) 1 91) 1 92) 2