Equal volumes of two solutions, one having pH 6 and the other having pH 4 are mixed. The pH of the resulting solution would be

Question

Equal volumes of two solutions, one having pH 6 and the other having pH 4 are mixed. The pH of the resulting solution would be (A) 5.7 (B) 4.3 (C) 5.0 (D) 5.5

Tardigrade Admin · Accepted Answer

[ H 3 O +] =(10-6+10-4/2)=5.05 × 10-5 pH =- log (5.05 × 10-5)=4.3

Q. Equal volumes of two solutions, one having $p H 6$ and the other having $p H 4$ are mixed. The $p H$ of the resulting solution would be

5.7

4.3

5.0

5.5

$[H_{3} O^{+}] = \frac{1 0 ^{- 6} + 1 0 ^{- 4}}{2} = 5.05 \times 1 0^{- 5}$

$p H = - lo g (5.05 \times 1 0^{- 5}) = 4.3$

Q. Equal volumes of two solutions, one having pH6 and the other having pH4 are mixed. The pH of the resulting solution would be

5.7

4.3

5.0

5.5

[H3​O+]=210−6+10−4​=5.05×10−5 pH=−log(5.05×10−5)=4.3

Q. Equal volumes of two solutions, one having $p H 6$ and the other having $p H 4$ are mixed. The $p H$ of the resulting solution would be

$[H_{3} O^{+}] = \frac{1 0 ^{- 6} + 1 0 ^{- 4}}{2} = 5.05 \times 1 0^{- 5}$

$p H = - lo g (5.05 \times 1 0^{- 5}) = 4.3$