25.0 mL of 0.100 M acetic acid (K_a = 1.8x 10^-5, pK_a = 4.74) is titrated with 0.100 M NaOH. Which statements are correct?

After 12.5 mL of NaOH the pH is 4.74.

At 25.0 mL of NaOH the pH is 8.72.

After 37.5 mL of NaOH the pH is 12.30.

After 12.5 mL of NaOH the pH is 4.74.

At 25.0 mL of NaOH the pH is exactly 7.00.

At 25.0 mL of NaOH the pH is 8.72.

After 37.5 mL of NaOH the pH is 12.30.

JEE Main levelOne or more correct optionsDifficulty 2 of 3ia139

$25.0 mL$ of $0.100 M$ acetic acid ( $K_{a} = 1.8 \times 1 0^{- 5}$ , $p K_{a} = 4.74$ ) is titrated with $0.100 M$ NaOH. Which statements are correct?

Half-way:

pH = p K_{a} = 4.74

. Equivalence (0.0500 M acetate):

pH = 8.72

, not 7. At

37.5 mL

excess NaOH

= 1.25 mmol

62.5 mL

[OH X^{-}] = 0.0200 M

pH = 12.30