1. Calculate the pH of 0.200 M barium acetate solution. 2. Is the following reac

Question

1. Calculate the pH of 0.200 M barium acetate solution.

2.

Is the following reaction product-favored or reactant-favored?

F^- (aq) + H2O (l) >><< HF (aq) + OH^- (aq)

Explain.

3. For the reaction below decide whether the equilibrium lies predominantly to the right or to the left.

HCL(aq) + CO3^2- (aq) >>><<< Cl^- (aq) + HCO3^- (aq)

Why?

4. Which is the strongest base? Which is the weakest base?

CH3CO2

2.

Is the following reaction product-favored or reactant-favored?

F^- (aq) + H2O (l) >><< HF (aq) + OH^- (aq)

Explanation / Answer

1)

[CH3COO-] = 2 x 0.2 = 0.4

CH3COO- + H2O <----> CH3COOH + OH-

Ka = 10^-4.75 = 1.78 x 10^-5

the constant of this reaction is Kw/Ka = 5.62 x 10^-10

5.62 x 10^-10 = x^2 / 0.4-x

x = [OH-] = 1.499 x 10-5 M

pOH = 4.82

pH = 14 - 4.82 = 9.17

2)   the reaction is

F^- (aq) + H2O (l) >><< HF (aq) + OH^- (aq)

it is mostly reactant favored because

HF is a strong acid than H20 , so HF donates the proton and OH- accepts to form   H20  

3)   the reaction is

     HCL(aq) + CO3^2- (aq) >>><<< Cl^- (aq) + HCO3^- (aq)

the reaction predominantly favors the right side because   the strong acid HCl   donates its proton which is accepted

by the weak acid HC03-

4)    C032-

       HS- and CH3C02-   are conjugate bases of weak acids H2S and CH3C00H . so they are strong bases .

     NH3 is a strong base .

    so   Co32-   is the weak base

5)     K2C03 ------> Basic

        NH4Br ------->   Acidic

      FeCl3 -----> acidic

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