Methods of Expressing Concentration of Solutions

A 5 molar solution of  ${\text{H}}_2\text{S}{\text{O}}_4$ is diluted from 1 litre to a volume of 10 litres, the normality of the resulting solution will be :

What is mole percentage?

Which of the following remains unaffected by the temperature change?

Which of the following way cannot be used to express the percent strength of the solution?

The $\%\left(\frac{\mathrm{w}}{\mathrm{v}}\right)$ of ${\mathrm{H}}_2{\mathrm{O}}_2$ in $1.5 \mathrm{N}$ solution is

If the mole fraction of ethanol in a solution of ethanol in water is $0.050,$ then find the molarity of the given solution.

What amount of conc ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution should be used to prepare $500 \mathrm{ml}$ of $0.5{\mathrm{MH}}_2{\mathrm{SO}}_4 ?$(The concentration of ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution being used is $90\%$ and molecular mass of ${\mathrm{H}}_2{\mathrm{SO}}_4=98.079 \mathrm{g}. {\mathrm{mol}}^{-1})$

If the density of a $5\mathrm{M}$ solution of $\mathrm{KCl}$ is $1.26 {\mathrm{gml}}^{-1},$ then find the molality of the solution. (Molecular mass of $\mathrm{KCl}=74.55 \mathrm{g}{ \mathrm{mol}}^{-1}$)

Density of $3\mathrm{M}$ solution of $\mathrm{NaCl}$ is $1.25 \mathrm{g}/\mathrm{mL}.$ Calculate the volume of water required to make $1000 \mathrm{mL}$ of this $\mathrm{NaCl}$ solution. [Consider the density of water as $1\mathrm{g}/\mathrm{mL}].$

A solution is prepared by mixing $25.0 \mathrm{g}$ of water and $25.0 \mathrm{g}$ of ethanol. Determine the mole percentage of ethanol.

Calculate the mole percentage of carbon tetrachloride in a solution containing $70\%$ by mass of benzene.

Calculate the mole percentage of benzene in a solution containing $30\%$ by mass of carbon tetrachloride.

$0.100 \mathrm{mol}$ of sodium chloride is dissolved in $100 \mathrm{g}$ of pure water. What is the mole percentage of sodium chloride?

Define mole percentage.

Which of the following concentration terms is temperature independent?

The molarity of a solution obtained by mixing $750 \mathrm{mL}$ of $0.5\left(\mathrm{M}\right) \mathrm{HCl}$ with $250 \mathrm{mL}$ of $2\left(\mathrm{M}\right) \mathrm{HCl}$ will be

In what mass of water must $25 \mathrm{g}$ of ${\mathrm{CuSO}}_4.5{\mathrm{H}}_2\mathrm{O}$ be dissolved to obtain an $8\%$ solution of ${\mathrm{CuSO}}_4$? $\left(\mathrm{At}. \mathrm{wt}. \mathrm{of} \mathrm{Cu} = 63.5\right)$

Round off answer to the nearest integer value.

Calculate mole fraction of solute in an aqueous $4 \mathrm{m}$ solution assuming the density of the solution as $1.0 \frac{\mathrm{g}}{\mathrm{mL}}$.

Give your answer up to three decimal places. Give your answer as an nearest integer after multiplying with 1000.

A sugar syrup of weight $214.2 \mathrm{g}$ contains $34.2 \mathrm{g}$ of sugar $\left({\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\right).$ Mole fraction of sugar in the syrup is $\mathrm{y}\times {10}^{-4}$.

Calculate the value of $\mathrm{y}$?

A sugar syrup of weight $214.2 \mathrm{g}$ contains $34.2 \mathrm{g}$ of sugar has a molal concentration of A,

Give your answer by multiplying the value of A in to 100 and rounding off the value to two significant figure.