What will be the pH of 1 - 10-4M H2SO4 solution-

The correct option is B 03.70 Sulphuric acid is a dibasic acid and hence gives #160; two H^+ atoms in it's solution. Since, it is a strong acid it ...

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Standard IX

Chemistry

pH of a Solution

What will be ...

Question

What will be the pH of $1 \times 10^{- 4}$ M $H_{2} S O_{4}$ solution?

10.4

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03.70

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Solution

The correct option is B $03.70$
Sulphuric acid is a dibasic acid and hence gives two $H^{+}$ atoms in it's solution. Since, it is a strong acid it dissociates completely as:
$H_{2} S O_{4} ⇌ 2 H^{+} + S O_{4}^{2 -}$
$[H^{+}] = 2 * 0.0001 M$
$p H = - l o g (2 * 0.0001) = 3.70$

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What will be the pH of 1×10−4M H2SO4 solution?

The correct option is B 03.70Sulphuric acid is a dibasic acid and hence gives two H+ atoms in it's solution. Since, it is a strong acid it dissociates completely as:H2SO4⇌2H++SO2−4[H+]=2∗0.0001MpH=−log(2∗0.0001)=3.70

What will be the pH of $1 \times 10^{- 4}$ M $H_{2} S O_{4}$ solution?

The correct option is B $03.70$
Sulphuric acid is a dibasic acid and hence gives two $H^{+}$ atoms in it's solution. Since, it is a strong acid it dissociates completely as:
$H_{2} S O_{4} ⇌ 2 H^{+} + S O_{4}^{2 -}$
$[H^{+}] = 2 * 0.0001 M$
$p H = - l o g (2 * 0.0001) = 3.70$