A weak monobasic acid is half neutralized by a strong base. If the Ph of the solution is 5.4 its `pK_(a)` is

STATEMENT-1: Autoprotolysis constant of water increases with the increase in temperature. STATEMENT-2: When a solution of a weak monobasic acid is titrated wita a strong base, at half neutralization point pH=pK_(a)+1. STATEMENT-3: The pH of 10^(-8) m HCl is 8.

The pH of a weak mono acidic base, neutralized upto 80% with a strong acid in a dilute solution, is 7.40. The ionization constant of the base is

Assertion : In a titration of weak monoprotic acid with strong base, the pH at the half equivalence point is pK_(a) . Reason : At half equivalence point, it will form acidic buffer at its maximum capacity where [acid] = [salt].

Assertion : In a titration of weak monoprotic acid with strong base, the pH at the half equivalent point is pK_(a) . Reason : At half equivalence point, it will form acidic buffer at its maximum capacity where [acid] = [salt].

Assertion : In a titration of weak monoprotic acid with strong base, the pH at the half equivalent point is pK_(a) . Reason : At half equivalence point, it will form acidic buffer at its maximum capacity where [acid] = [salt].

pH of a salt of a strong base with weak acid

pH of a salt of a strong base with weak acid