1. When 0.014 mol of a weak acid HA is dissolved in enough water to make 1.0 L o
ID: 1077410 • Letter: 1
Question
1. When 0.014 mol of a weak acid HA is dissolved in enough water to make 1.0 L of solution, [H+] is 1.8x10-3 M. Calculate the freezing point of this solution. Assume that the molarity concentration is equal to the molality concentration, and assume ideal behavior. Kf (H2O) is 1.86°C kg/mol.
A) -0.058°C B) -0.029°C C) -0.026°C D) +0.029°C E) +0.026°C
ANS: B
2. You use 2.0 g of solid MX to prepare a saturated solution in 250. g of water. You find the freezing point to be –0.028°C. Calculate Ksp for the solid. A) 2.2x 10–4 B) 5.6x 10–5 C) 1.4x10–5 D) 3.5x10–6 E) none of these
ANS: D
3.Which of the following statements is(are) true?
A) The rate of dissolution of a solid in a liquid always increases with increasing temperature.
B) The solubility of a solid in a liquid always increases with increasing temperature.
C) According to Henry's law, the amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the liquid.
D) Two of these statements are true.
E) All of these statements are true.
P.sI Ask Q1 and Q2 on Chegg before, but the answers are wrong. Thank you for your help.
Explanation / Answer
1. When 0.014 mol of a weak acid HA is dissolved in enough water to make 1.0 L o
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