40. The total mass of a solution is 184.8 g. The solvent mass is 125.2 g. What is the mass percent of
the solute?
(A) 32.3 %
(B) Not enough information is given.
(C) 43.3 %
(D) 21.6 %
(E) 67.7 %

41. You have 25.00 mL of a 0.1000 M sugar solution. How much water must be added to make a0.01809M solution?(A) 138.2 mL (B) 4.52 mL (C) 20.5 mL (D) 113.2 mL (E) 45.2 mL

42. How many grams of NaCl are contained in 350. mL of a 0.238 M solution of sodium chloride?(A) 83.3 g (B) 4.87 g (C) 13.9 g (D) 1.43 g (E) none of these

43. What volume of 18.0 M sulfuric acid is required to prepare 26.2 L of 0.126 M H2SO4? (A) 5.45 mL. (B) 0.183 L. (C) 472 mL. (D) 3.30 L. (E) 208 mL.

44. Choose the case that is not a Bronsted conjugate acid-base pair. (A) CH3NH3+, CH3NH2 (B) HCN, CN- (C) HClO2, ClO2- (D) HCO2H, HCO2- (E) H3BO3, H2BO3-

45. A solution has [OH-] = 3.0x10-7 M. The [H+] in this solution is (A) 1.0 M (B) 3.0 x 10-7 M (C) 1.0 x 10-7 M (D) 3.3 x 10-8 M (E) none of these

46. What is the pH of a 2.1 M solution of HNO3?(A) –0.32 (B) 0.32 (C) 14.32 (D) 13.68 (E) none of these

47. Given the reaction \( A(g) + B(g) \rightleftharpoons C(g) + D(g) \). You have the gases A, B, C, and D at equilibrium. Upon adding gas A, the value of K (A) increases because when A is added, more products are made, increasing the product-to-reactant ratio (B) decreases because A is a reactant, so the product-to-reactant ratio decreases (C) does not change because A does not figure into the product-to-reactant ratio (D) does not change as long as the temperature is constant (E) depends on whether the reaction is endothermic or exothermic

48. Given the equation A(g) $\rightleftharpoons$ B(g) + 2C(g). At a particular temperature, $K = 1.3 \times 10^5$. If you mixed 1.4 mol B, 0.050 mol C, and 0.0050 mol A in a 1-liter container, in which direction would the reaction initially proceed? (A) The reaction will proceed to the right. (B) The reaction will proceed to the left. (C) The mixture is at equilibrium. (D) More information is needed to answer the question.

49. The solubility of Mg(OH)2(s) in water at a certain temperature is 1.1x10-4 mol/L. Calculate the value of Ksp for Mg(OH)2(s) at this temperature. (A) 1.1 x 10-4 (B) 1.3 x 10-12 (C) 1.2 x 10-8 (D) 5.3 x 10-12 (E) none of these

50. The oxidation state of phosphorus in Mg3(PO4)2 is (A) 0 (B) +2 (C) +4 (D) +5 (E) +6

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