1) Two gases, A and B, are placed in an empty, 2.43-liter container at 500 °C. W

Question

1) Two gases, A and B, are placed in an empty, 2.43-liter container at 500 °C. When equilibrium is established, 2.05 mol A, 2.83 mol B, and 0.74 mol C are present. Evaluate Kc for the following reaction at 500 °C.

2) It is desired to buffer a solution at pH = 4.30. What molar ratio of CH3COOH to NaCH3COO should be used? The Ka for CH3COOH is 1.8 x 10-5.

3) How much NH4Cl must be added to 2.00 liters of 0.2 M aqueous ammonia to give a solution with pH = 8.55? Assume no volume change due to the addition of NH4Cl. TheKb of ammonia is 1.8 x 10-5, and the molar mass of ammonium chloride is 53.491 g/mol

4) Calculate the freezing point of a solution that contains 30.8 g of urea, CH4N2O (MW = 60.06 g/mol), in 196 g of water. Urea is a nonvolatile nonelectrolyte. Kf for H2O = 1.86

Explanation / Answer

chegg;s policy prohibits asking multiple question of a single post, so I am going to solve one of the questions for you.

2) let the molar ration of CH3COOH to NaCH3COO be x.so,

pH=pKa+log(salt/acid)

or 4.3=4.76 + log(1/x)

or x=2.88

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