If the pH of an aqueous solution is 4.7, then its H +concentration will be

Question

If the pH of an aqueous solution is 4.7, then its H +concentration will be (A)  3× 10-6 (B)  3× 10-5 (C)  2× 10-5 (D)  5× 10-5

Tardigrade Admin · Accepted Answer

p H =- log [ H +] Here, pH =4.7 ∴ 4.7 =- log [ H +] 4.7 = log [ H +]-1 Antilog 4.700 =[ H +]-1 50120.0 =(1/[ H +]) [ H +] =(1/50120) [ H +] =0.00002 [ H +] =2 × 10-5

Q. If the $p H$ of an aqueous solution is $4.7$ , then its $H^{+}$ concentration will be

$3 \times 1 0^{- 6}$

$3 \times 1 0^{- 5}$

$2 \times 1 0^{- 5}$

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

$p H = - lo g [H^{+}]$
Here, $p H = 4.7$
$∴ 4.7 = - lo g [H^{+}]$
$4.7 = lo g [H^{+}]^{- 1}$
Antilog $4.700 = [H^{+}]^{- 1}$
$50120.0 = \frac{1}{[ H ^{+} ]}$
$[H^{+}] = \frac{1}{50120}$
$[H^{+}] = 0.00002$
$[H^{+}] = 2 \times 1 0^{- 5}$

Q. If the pH of an aqueous solution is 4.7, then its H+concentration will be

3×10−6

3×10−5

2×10−5

5×10−5