1. Write the equilibrium-constant expressions and obtain numerical values for each constant in (a) the basic dissociation of aniline, C6H5NH2 . (b) the acidic dissociation of hypochlorous acid, HClO. (c) the acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl. (d) the basic dissociation of NaNO2 . (e) the dissociation of H3AsO3 to H3O + and AsO33- 2. The chemicals A and B react as follows to produce C and D: A + B ↔ C + D Ke = [C] [D] [A] [B] The equilibrium constant Ke has a value of 0.30. Assume 0.20 mol of A and 0.50 mol of B are dissolved in 1.00 L, and the reaction proceeds. Calculate the concentrations of reactants [A], [B] and products [C], [D] at equilibrium. Using step-by-step process
1. Write the equilibrium-constant expressions and obtain numerical values for each constant in
(a) the basic dissociation of aniline, C6H5NH2 .
(b) the acidic dissociation of hypochlorous acid, HClO.
(c) the acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl.
(d) the basic dissociation of NaNO2 .
(e) the dissociation of H3AsO3 to H3O + and AsO33-
2. The chemicals A and B react as follows to produce C and D:
A + B ↔ C + D
Ke = [C] [D]
[A] [B]
The equilibrium constant Ke has a value of 0.30. Assume 0.20 mol of A and 0.50 mol of B are dissolved in 1.00 L, and the reaction proceeds. Calculate the concentrations of reactants [A], [B] and products [C], [D] at equilibrium.
Using step-by-step process
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