1.00 liter solution contains 0.31 M acetic acid and 0.40 M sodium acetate. If 0.100 moles of calcium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of calcium hydroxide.) A. The number of moles of CH3COOH will decrease.
B. The number of moles of CH3COO- will decrease.
C. The equilibrium concentration of H3O will decrease.
D. The pH will decrease.
E. The ratio of [CH3COOH] / [CH3COO-] will remain the same.

The answer is the explanation.

Explanation:

The acetic acid, CH3COOH, reacts with calcium hydroxide, Ca(OH)2, producing acetate ion, CH3COO- and water as follows:

2CH3COOH + Ca(OH)2 → 2CH3COO- + 2H2O + Ca²⁺

That means the moles of acetic acid decrease whereas the moles of  acetate ion are increased. The ratio of [CH3COOH] / [CH3COO-] is different.

As a base is added, the concentration of H3O+ decreases increasing the pH.

That means:

TRUE A. The number of moles of CH3COOH will decrease.

FALSE B. The number of moles of CH3COO- will decrease.

TRUE C. The equilibrium concentration of H3O will decrease.

FALSE D. The pH will decrease.

FALSE E. The ratio of [CH3COOH] / [CH3COO-] will remain the same.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

i think its 5049.

i hope this !