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Concentrated sulphuric acid has density ...

Concentrated sulphuric acid has density of 1.9 g/mL and 99% `H_(2)SO_(4)` by mass. Calculate the molarity of the acid.

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Let v mL of 95.6 mass % sulphuric acid of density `1.84 g ml^(-1)` be added to 1000mL of 40 mass % `H_(2)SO_(4)` so that total solution of 50 mass % `H_(2)SO_(4)` becomes (1000 + v)mL.
Volume of solution of 95.6% `H_(2)SO_(4) = (100)/(1.84)`
Amount of `H_(2)SO_(4)` in v mL of solution ` = 95.6 xx (1.84)/(100) xx v`
Volume of solution of 40 % `H_(2)SO_(4) = (100)/(1.31)`
Amount of `H_(2)SO_(4)` in 1000 mL of solution `=(40 xx 1.31)/(100) xx 1000`
Volume of solution of 50% `H_(2)SO_(4) = (100)/(1.40)`
Amount of `H_(2)SO_(4)` in (1000+ v) mL of solution .
`= 50 xx (1.40)/(100) xx (1000+v)`
Thus , `(95.6 xx 1.84 xx v)/(100) + (40 xx 1.31)/(100) xx 1000 = (50 xx 1.40)/(100) (1000+v)`
` 175.90v + 52400 = 70000+70v`
`105.90 v = 17600`
or ` v = 166.2 mL`
vol. of `H_(2)SO_(4)` of density 1.84 contaning 95.6 mass % of `H_(2)SO_(4)` to be added = 166.2 mL
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Knowledge Check

  • The concentrated sulphuric acid that is peddled commercially is 95% H_(2)SO_(4) by weight. If the density of this commerical acid is 1.834 g cm^(-3) , the molarity of this solution is

    A
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    B
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    C
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    D
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    B
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    C
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  • Conc. H SO_4 has density of 1.9 g mL^(-1) and is 99% by weight. Calculate the molarity of H_2SO_4 " (Mol wt of " H_2SO_4 = 98 g mol^(-1) ).

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