Reference no: EM132554153

1. Write the algebraic expression and the balanced chemical equilibrium reaction for the equilibrium constant Kw

2. Write the expression for the equilibrium constant Ka for the HOCl equilibrium above.

3. In a strong acid solution, both of the following equilibria are present. Which reaction contributes most to the overall concentration of H3O+?

HCl(aq) + H2O(l) ? H3O+(aq) + Cl-(aq) Ka >> 1

H2O(l) + H2O(l) ? H3O+(aq) + OH-(aq) Kw = 1.0 x 10-14

Explain your reasoning.

4. In a weak acid solution, both of the following equlibria are present. Which reaction contributes most to the overall concentration of H3O+?

HOCl(aq) + H2O(l) ? H3O+(aq) + OCl-(aq) Ka = 3.5 x 10-8

H2O(l) + H2O(l) ? H3O+(aq) + OH-(aq) Kw = 1.0 x 10-14

Explain your reasoning.

5. Which solution has a lower pH, 1.0 M HCl or 1.0 M HOCl? Justify your answer without a calculation.

6. Calculate the pH of a 1.0 M HCl solution and the pH of a 1.0 M HOCl solution (using the Ka value provided above).

7. Are any hydroxide ions present in a 1.0 M HCl solution? If so, list their source and calculate the [OH-] of a 1.0 M HCl solution.

8. Can a solution have a negative pH? If so, list an acid that could produce such a solution, as well as its concentration.