What is the ph of an aqueous solution of 1 m ch3cooh (pka=4)

pH = 2.

Explanation:

A weak acid is in equilibrium with its ions in a solution, so it must have an equilibrium constant (Ka). And, pKa = -logKa

Ka = 10⁻⁴

So, for CH₃COOH the equilibrium must be:

CH₃COOH(aq) ⇄ H⁺(aq) + CH₃COO⁻(aq)

1 M                           0                0                Initial

-x                              +x              +x               Reacted

1-x                             x                x                 Equilibrium

And the equilibrium constant:

Supposing x << 1:

10⁻⁴ = x²

x = √10⁻⁴

x = 10⁻² M, so the supposing is correct.

So,

pH = -log[H⁺]

pH = -log10⁻²

pH = 2

po-215 i got it right on the quiz

that's what i got you can count the number of atoms