Ionization constant of acetic acid is 1.8 × 10-5. The concentration of H+ions in 0.1 M solution is ;

Question

Ionization constant of acetic acid is 1.8 × 10-5. The concentration of H+ions in 0.1 M solution is ; (A)  1.8× 10-3M  (B)  1.8× 10-5M  (C)  1.3× 10-3M  (D)  1.34× 10-3M

Tardigrade Admin · Accepted Answer

CH 3 COOH ionise as follows: <img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/42f3ab029cb46c251fc30155a12ee3df-.png" /> [ H 3 O +]= C α and α=√Ka / C (for any weak electrolyte) or [ H 3 O +]=√Ka ⋅ C =√1.8 × 10-5 × .1=1.34 × 10-3 M

Q. Ionization constant of acetic acid is $1.8 \times 1 0^{- 5}$ . The concentration of $H^{+}$ ions in $0.1 M$ solution is ;

$1.8 \times 1 0^{- 3} M$

$1.8 \times 1 0^{- 5} M$

$1.3 \times 1 0^{- 3} M$

$1.34 \times 1 0^{- 3} M$

$C H_{3} COO H$ ionise as follows :

$[H_{3} O^{+}] = C α$
and $α = K_{a} / C$ (for any weak electrolyte)
or $[H_{3} O^{+}] = K_{a} \cdot C$
$= 1.8 \times 1 0^{- 5} \times .1 = 1.34 \times 1 0^{- 3} M$

Q. Ionization constant of acetic acid is 1.8×10−5. The concentration of H+ions in 0.1M solution is ;

1.8×10−3M

1.8×10−5M

1.3×10−3M

1.34×10−3M