1. When 0.014 mol of a weak acid HA is dissolved in enough water to make 1.0 L o

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

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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