The concentration of [ H +]and concentration of [ OH -]of a 0.1 M aqueous solution of 2 % ionised weak monobasic acid is [ionic product of water =1 × 10-14 ]

Question

The concentration of [ H +]and concentration of [ OH -]of a 0.1 M aqueous solution of 2 % ionised weak monobasic acid is [ionic product of water =1 × 10-14 ] (A)  0.02 × 10-3 M and 5 × 10-11 M (B)  1 × 10-3 M and 3 × 10-11 M (C)  2 × 10-3 M and 5 × 10-12 M (D)  3 × 10-2 M and 4 × 10-13 M

Tardigrade Admin · Accepted Answer

[ H +]in monobasic acid = molarity × degree of ionisation =0.1 × (2/100)=2 × 10-3 M ionisation constant of water Kw=(H+)(O H-) [O H-]=(1 × 10-14/2 × 10-3)=5 × 10-12 M

Q. The concentration of $[H^{+}]$ and concentration of $[O H^{-}]$ of a $0.1 M$ aqueous solution of $2%$ ionised weak monobasic acid is
[ionic product of water $= 1 \times 1 0^{- 14}$ ]

$0.02 \times 1 0^{- 3} M$ and $5 \times 1 0^{- 11} M$

$1 \times 1 0^{- 3} M$ and $3 \times 1 0^{- 11} M$

$2 \times 1 0^{- 3} M$ and $5 \times 1 0^{- 12} M$

$3 \times 1 0^{- 2} M$ and $4 \times 1 0^{- 13} M$

$[H^{+}]$ in monobasic acid
= molarity $\times$ degree of ionisation
$= 0.1 \times \frac{2}{100} = 2 \times 1 0^{- 3} M$
ionisation constant of water
$K_{w} = (H^{+}) (O H^{-})$
$[O H^{-}] = \frac{1 \times 1 0 ^{- 14}}{2 \times 1 0 ^{- 3}} = 5 \times 1 0^{- 12} M$

Q. The concentration of [H+]and concentration of [OH−]of a 0.1M aqueous solution of 2% ionised weak monobasic acid is [ionic product of water =1×10−14 ]

0.02×10−3M and 5×10−11M

1×10−3M and 3×10−11M

2×10−3M and 5×10−12M

3×10−2M and 4×10−13M