(D) Initial moles of $HNO_3$ = $Molarity \times Volume(L) = 0.5 \times 0.8 = 0.4 \ mol$.Moles of $HNO_3$ evaporated = $\frac{Mass}{Molar \ mass} = \fr

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(D) Initial moles of $HNO_3$ = $Molarity \times Volume(L) = 0.5 \times 0.8 = 0.4 \ mol$.Moles of $HNO_3$ evaporated = $\frac{Mass}{Molar \ mass} = \frac{11.5 \ g}{63 \ g \ mol^{-1}} \approx 0.1825 \ mol$.Moles of $HNO_3$ remaining = $0.4 - 0.1825 = 0.2175 \ mol$.New volume of solution = $\frac{800 \ mL}{2} = 400 \ mL = 0.4 \ L$.New molarity = $\frac{Moles \ remaining}{Volume(L)} = \frac{0.2175}{0.4} = 0.54375 \ M$.Expressing in $x \times 10^{-2} \ M$,we get $54.375 \times 10^{-2} \ M$.Rounding to the nearest integer,$x = 54$.

Class 11 Chemistry Some Basic Concepts of Chemistry Mix Examples of Some Basic Concept of Chemistry

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When $800 \ mL$ of $0.5 \ M$ nitric acid is heated in a beaker,its volume is reduced to half and $11.5 \ g$ of nitric acid is evaporated. The molarity of the remaining nitric acid solution is $x \times 10^{-2} \ M$. (Nearest Integer) (Molar mass of nitric acid is $63 \ g \ mol^{-1}$)

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A
$51$
B
$52$
C
$53$
D
$54$

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Some Basic Concepts of Chemistry

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Mix Examples of Some Basic Concept of Chemistry

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When $800 \ mL$ of $0.5 \ M$ nitric acid is heated in a beaker,its volume is reduced to half and $11.5 \ g$ of nitric acid is evaporated. The molarity of the remaining nitric acid solution is $x \times 10^{-2} \ M$. (Nearest Integer) (Molar mass of nitric acid is $63 \ g \ mol^{-1}$)

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$10 \ g$ $NaHCO_{3(s)}$ sample is heated in open to constant weight,the residue is titrated against $0.1 \ M \ HCl$ in presence of phenolphthalein as an indicator,$500 \ mL$ of acid was required to reach end point hence $PERCENT$ purity of sample is $............... \%$.

Calculate the number of moles of $NaOH$ required to completely neutralize $100 \ g$ of $118\%$ oleum.

What volume of $NH_3$ gas at $STP$ would be needed to prepare $100 \ mL$ of $2.5$ molal $(2.5 \ m)$ ammonium hydroxide solution? (Assume the density of the solution is $1 \ g/mL$)

When $40 \, mL$ of $0.1 \, N \, HCl$ and $20 \, mL$ of $0.1 \, M \, H_2SO_4$ are mixed together,the normality of the mixture will be

Iron sulphide is heated in air to form $A$, an oxide of sulphur. $A$ is dissolved in water to give an acid. The basicity of this acid is:

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