(A) The theoretical weight is calculated based on $100\%$ purity of the substance. Since the sample is impure,its percentage purity is less than $100\

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More than the theoretical weight

(A) The theoretical weight is calculated based on $100\%$ purity of the substance. Since the sample is impure,its percentage purity is less than $100\%$. To obtain the required amount of the pure compound,we must take a larger quantity of the impure sample to compensate for the impurities present. Therefore,the weight of the impure substance required will be greater than the theoretical weight calculated for a pure substance.

Class 11 Chemistry Some Basic Concepts of Chemistry Chemical stoichiometry

Medium

For preparing a $0.1 \ N$ solution of a compound from its impure sample,where the percentage purity is known,the weight of the substance required will be:

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A
More than the theoretical weight
B
Less than the theoretical weight
C
Same as the theoretical weight
D
None of these

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Some Basic Concepts of Chemistry

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Chemical stoichiometry

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For preparing a $0.1 \ N$ solution of a compound from its impure sample,where the percentage purity is known,the weight of the substance required will be:

Similar Questions

What is the mass of oxygen in $g$ required to produce enough $CO$ for the complete reduction of $1.6 \ kg$ of $Fe_2O_3$ (molar mass $= 160 \ g/mol$)?

When ${CO_2}_{(g)}$ is passed over hot coke,it is reduced to ${CO}_{(g)}$. When $0.5 \, L$ of ${CO_2}_{(g)}$ is passed over hot coke,the total volume of the gas increases by $700 \, mL$ at $STP$. The composition of the resulting gaseous mixture is:

$A$ sample of nitric acid has a density of $1.41 \ g \ mL^{-1}$ and the mass percentage of nitric acid is $69 \%$. Calculate the concentration of nitric acid in the sample in moles per liter. (in $M$)

Which solution is required to completely neutralize $25 \ mL$ of $N/10$ $NaOH$ solution?

The normality of $0.04 \ M \ H_2SO_4$ is = ........ $N$

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