The specific gravity of sulphuric acid 1.8. What volume of this sample of concentrated H $_{2}$ SO $_{4}$ is required to prepare 500 ml 0.9 M H $_{2}$ SO $_{4}$ solution?

23.5 ml

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24.5 ml

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25.5 ml

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26.5 ml

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Solution

The correct option is B 24.5 ml
1000 mL will weigh 1800g
mass of $H_{2} S O_{4}$ present = 1800 gm
number of mole of $H_{2} S O_{4}$ = actual $m a s s / m o l a r m a s s$ = 1800 ÷ 98 = 18.36
thus molarity of a stock solution is 18.36 M
To prepare 500 mL of 0. 9 M solution, $M_{1} V_{1} = M_{2} V_{2}$
18.36 x A = 0.9 x 500 mL
$\frac{450}{18.36}$
= 24.5 ml

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The specific gravity of sulphuric acid 1.8. What volume of this sample of concentrated H2SO4 is required to prepare 500 ml 0.9 M H2SO4 solution?

The correct option is B 24.5 ml1000 mL will weigh 1800gmass of H2SO4 present = 1800 gmnumber of mole of H2SO4 = actual mass/molarmass= 1800 ÷ 98 = 18.36thus molarity of a stock solution is 18.36 MTo prepare 500 mL of 0. 9 M solution, M1V1=M2V218.36 x A = 0.9 x 500 mL45018.36= 24.5 ml

The specific gravity of sulphuric acid 1.8. What volume of this sample of concentrated H $_{2}$ SO $_{4}$ is required to prepare 500 ml 0.9 M H $_{2}$ SO $_{4}$ solution?