A solution is prepared by adding 0.10 mol of potassium acetate, KCH3COO, to 1.00 L of water. Whichstatement about the solution is correct? A. The solution is basic. B. The solution is neutral. C. The solution is acidic. D. The concentrations of potassium ions and acetate ions will be identical. E. The concentration of acetate ions will be greater than the concentration of potassium ions.

Question

Laura Buck

Chemistry

24 July, 00:26

A solution is prepared by adding 0.10 mol of potassium acetate, KCH3COO, to 1.00 L of water. Whichstatement about the solution is correct? A. The solution is basic. B. The solution is neutral. C. The solution is acidic. D. The concentrations of potassium ions and acetate ions will be identical. E. The concentration of acetate ions will be greater than the concentration of potassium ions.

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Answers (1)

Know the Answer?

Mike Hartman · Answer 1

I believe there's something wrong with this question, or at least there are two correct answers

Both ions has the same concentration in solution.

The solution is basic.

Explanation:

This is an highly soluble salt, 268.6 g/100 mL at 25 °C. In addition, the stoichiometry between the ions is 1:1, so their concentrations has to be the same.

The acetate ion is the conjugated bas from acetic acid, and acetic acid is an weak acid, so its conjugated base is somewhat basic, because it shifts the hydrogen equilibrium in producing acetic acid (consuming hydronium) which makes a solution slightly basic.