What volume of 0.10 M $H_{2} S O_{4}$ must be added to 50 mL of a 0.10 M NaOH solution to make a solution in which the molarity of the $H_{2} S O_{4}$ is 0.050 M?

400 mL

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50 mL

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100 mL

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150 mL

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Solution

The correct option is D 100 mL
Firstly, calculate how much volume of $H_{2} S O_{4}$ is required to completely neutralize $N a O H$ .

$0.1 M H_{2} S O_{4} = 0.2 N H_{2} S O_{4}$
$0.1 M N a O H = 0.1 N$

$V_{1} N_{1} = V_{2} N_{2}$

$V_{1} = \frac{50 \times 0.1}{0.2}$

$V_{1} = 25 m l$

Now, Let $x m l$ of $H_{2} S O_{4}$ is added more

$x \times 0.2 = (75 + x) \times (0.05 \times 2)$
$x = 75 m l$

Total volume $= 100 m l$

$∴$ option C is correct.

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What volume of 0.10 M H2SO4 must be added to 50 mL of a 0.10 M NaOH solution to make a solution in which the molarity of the H2SO4 is 0.050 M?

The correct option is D 100 mLFirstly, calculate how much volume of H2SO4 is required to completely neutralize NaOH.0.1MH2SO4=0.2NH2SO40.1MNaOH=0.1NV1N1=V2N2V1=50×0.10.2V1=25mlNow, Let x ml of H2SO4 is added morex×0.2=(75+x)×(0.05×2)x=75mlTotal volume =100ml∴ option C is correct.

What volume of 0.10 M $H_{2} S O_{4}$ must be added to 50 mL of a 0.10 M NaOH solution to make a solution in which the molarity of the $H_{2} S O_{4}$ is 0.050 M?