A 1 liter solution contains 0.384 M acetic acid and 0.512 M sodium acetate. Addition of 0.422 moles of calcium hydroxide will:

- Exceed the buffer capacity

- Raise the pH by several units

Explanation:

Will:

(Assume that the volume does not change upon the addition of hydrobromic acid.)

Raise the pH slightly

Lower the pH slightly

Raise the pH by several units

Lower the pH by several units

Not change the pH

Exceed the buffer capacity

1L of a buffer of 0.384M acetic acid and 0.512M of sodium acetate contains 0.384 moles of the acid and 0.512 moles of the salt.

A base as Ca(OH)2 reacts with the acid, CH3COOH as follows:

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

For the reaction of the 0.422 moles of calcium hydroxide are required:

0.422 moles Ca(OH)2 * (2 moles CH3COOH / 1 mole Ca(OH)2) = 0.844 moles of CH3COOH

As there are just 0.384 moles of acetic acid:

Exceed the buffer capacity

And:

Raise the pH by several units

-Because the solution becomes more basic-

where's the diagram?

the increase of protons   hope this