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An aqueous ethanol solution 400 ml was diluted to 400

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56. An aqueous ethanol solution (400 mL) was diluted to 4.00 L, giving a concentration of 0.0400 M. The concentration of the original solution was __________ M. a. 0.400 b. 0.200 c. 2.00 d. 1.60 e. 4.00 57. What is the concentration (M) of an aqueous methanol produced when 0.200 L of a 2.00 M solution was diluted to 0.800 L? 58. A 0.100 M solution of __________ will contain the highest concentration of potassium ions. 59. What is the molarity of an aqueous solution containing 22.5 g of sucrose (C 12 H 22 O 11 ) in 35.5 mL of solution?
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60. What is the molarity of an aqueous solution containing 22.5 g of glucose (C 6 H 12 O 6 ) in 35.5 mL of solution? a. 3.52 b. 0.634 c. 0.197 d. 0.125 e. 1.85 61. What mass (g) of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride? 62. What is the concentration of iodide ions in a 0.193 M solution of barium iodide? 63. When 0.500 mol of HC 2 H 3 O 2 is combined with enough water to make a 300 mL solution, the concentration of HC 2 H 3 O 2 is ______ M. 64. In a titration of 35.00 mL of 0.737 M H 2 SO 4 , __________ mL of a 0.827 M KOH solution is required for neutralization. a. 35.0 b. 1.12 c. 25.8 d. 62.4 e. 39.3 65. Calculate the concentration (M) of arsenic acid (H 3 AsO 4 ) in a solution if 25.00 mL of that solution required 35.21 mL of 0.1894 M KOH for neutralization. 66. Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H 2 C 2 O 4 ) in a solid given that a 0.7984 g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization. 67. How many moles of BaCl 2 are formed in the neutralization of 393 mL of 0.171 M Ba(OH) 2 with aqueous HCl?
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68. What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO 3 is treated with an excess of aqueous hydrobromic acid? a. 1.44 b. 1.23 c. 53.6 d. 34.5 e. 188 69. A 17.5 mL sample of an acetic acid (CH 3 CO 2 H) solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of aceticacid was __________ M. 70. What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl? 71. The point in a titration at which the indicator changes is called the __________. 72. Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization? a. 10.0 mL of 0.0500 M phosphoric acid b. 20.0 mL of 0.0500 M nitric acid c. 5.0 mL of 0.0100 M sulfuric acid d. 15.0 mL of 0.0500 M hydrobromic acid e. 10.0 mL of 0.0500 M perchloric acid
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