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Question

Find the pH of resultant solution when 100ml of 0.005M H2SO4 at 25oC is diluted to 1000ml. What is the amount of NaOH required to be dissolved in 500ml to exactly neutralize the above solution?

A
4g
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B
4×102g
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C
40g
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D
0.4g
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Solution

The correct option is B 4×102g
Number of moles of H+ in 0.005 M H2SO4=0.005×2×0.1=0.001 moles

After dilution concentration of H+ ions= 0.0011=0.001 mole/l

pH=log [0.001]=3

Amount of NaOH required to neutralize the solution= 0.001 mole

Weight= mole × molecular weight =0.001×40=4×102g

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