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Standard XII

Chemistry

Depression in Freezing Point

If 25 mL of a...

Question

If 25 mL of a $H_{2} S O_{4}$ solution reacts completely with 1.06 g of pure $N a_{2} C O_{3}$ , what is the normality of this acid solution?

1 N

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0.5 N

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1.8 N

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0.8 N

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Solution

The correct option is A $0.8 N$
$N o r m a l i t y = \frac{g r . e q u i v a l e n t . w t}{m l o f s o l u t i o n} \times 1000$
$G r . e q . w t = \frac{w t}{e q . w t} G r . e q . w t = \frac{1.06}{53} g r . e q . w t = 0.02 g m$
$S o N o r m a l i t y = \frac{0.02}{25} \times 1000 N o r m a l i t y = 0.8 N$
So answer is D.

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Similar questions

0.106

g of

N a_{2} C O_{3}

completely neutralises

40.0

mL of

H_{2} S O_{4}

. Hence, normality of

H_{2} S O_{4}

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0.06

6

in the answer) :

Q. 25 mLof 2N HCL 50mL of 4N

H N O_{3}

and x mL of 2M

H_{2} S O_{4}

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Q. A definite amount of

B a C l_{2}

was dissolved in

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20

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for complete neutralization. Further

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0.1 N

N a_{2} C O_{3}

and the precipitate was filtered off. The filtrate reacted with

10.5

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using phenolphthalein as indicator. The strength of

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mL of a solution of

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32.9

mL of a solution of

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0.84 N H_{2} S O_{4}

that will be completely neutralized by

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{N a}_{2} C O_{3}

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Q. An aqueous solution containing

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If 25 mL of a H2SO4 solution reacts completely with 1.06 g of pure Na2CO3, what is the normality of this acid solution?

The correct option is A 0.8NNormality=gr.equivalent.wtmlofsolution×1000Gr.eq.wt=wteq.wtGr.eq.wt=1.0653gr.eq.wt=0.02gmSoNormality=0.0225×1000Normality=0.8NSo answer is D.

If 25 mL of a $H_{2} S O_{4}$ solution reacts completely with 1.06 g of pure $N a_{2} C O_{3}$ , what is the normality of this acid solution?