The pH of 0.01 M solution of acetic acid is 5.0 . What are the values of [ H +] and Ka respectively?

Question

The pH of 0.01 M solution of acetic acid is 5.0 . What are the values of [ H +] and Ka respectively? (A) 1 × 10-5 M , 1 × 10-8 (B) 1 × 10-5 M , 1 × 10-9 (C) 1 × 10-4 M , 1 × 10-8 (D) 1 × 10-3 M , 1 × 10-8

Tardigrade Admin · Accepted Answer

Given, pH of 0.01 M CH 3 COOH solution =5.0 Concentration, C of the solution =0.01 M [ H +] =1 × 10- pH =1 × 10-5 mol / L =1 × 10-5 M Since, acetic acid is a weak acid and for weak acid, [ H +] =√Ka ⋅ C [ H +]2 =Ka ⋅ C or Ka =([ H +]2/C) =((1 × 10-5)2/0.01) =1 × 10-8

Q. The $p H$ of $0.01 M$ solution of acetic acid is $5.0.$ What are the values of $[H^{+}]$ and $K_{a}$ respectively?

$1 \times 1 0^{- 5} M, 1 \times 1 0^{- 8}$

$1 \times 1 0^{- 5} M, 1 \times 1 0^{- 9}$

$1 \times 1 0^{- 4} M, 1 \times 1 0^{- 8}$

$1 \times 1 0^{- 3} M, 1 \times 1 0^{- 8}$

Q. The pH of 0.01M solution of acetic acid is 5.0. What are the values of [H+] and Ka​ respectively?

1×10−5M,1×10−8

1×10−5M,1×10−9

1×10−4M,1×10−8

1×10−3M,1×10−8

Given, pH of 0.01MCH3​COOH solution =5.0 Concentration, C of the solution =0.01M [H+]=1×10−pH =1×10−5mol/L=1×10−5M Since, acetic acid is a weak acid and for weak acid, [H+]=Ka​⋅C​ [H+]2=Ka​⋅C or Ka​=C[H+]2​ =0.01(1×10−5)2​ =1×10−8

Q. The $p H$ of $0.01 M$ solution of acetic acid is $5.0.$ What are the values of $[H^{+}]$ and $K_{a}$ respectively?

$1 \times 1 0^{- 5} M, 1 \times 1 0^{- 8}$

$1 \times 1 0^{- 5} M, 1 \times 1 0^{- 9}$

$1 \times 1 0^{- 4} M, 1 \times 1 0^{- 8}$

$1 \times 1 0^{- 3} M, 1 \times 1 0^{- 8}$