A solution is 0.10 M in HA (K_a = 2.0x10^-4) and 0.10 M in HB (K_a = 5.0x10^-6). Using [H+] = sqrtK_AC_A + K_BC_B, select the correct statement(s).

[A-] = [B-] because both acids are monobasic

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3ia220

A solution is $0.10 M$ in $HA$ ( $K_{a} = 2.0 \times 1 0^{- 4}$ ) and $0.10 M$ in $HB$ ( $K_{a} = 5.0 \times 1 0^{- 6}$ ). Using $[H X^{+}] = K_{A} C_{A} + K_{B} C_{B}$ , select the correct statement(s).

[H X^{+}] = 2.0 \times 1 0^{- 5} + 5.0 \times 1 0^{- 7} = 4.53 \times 1 0^{- 3} M

, pH

2.34

[A X^{-}] = K_{A} C_{A} / [H X^{+}] = 4.42 \times 1 0^{- 3}

and

[B X^{-}] = K_{B} C_{B} / [H X^{+}] = 1.10 \times 1 0^{- 4} M

. They differ by the ratio of the

K_{a} C

products (

\approx 40

), so the last statement is false.