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 :

An aqueous solution of ${\mathrm{FeCl}}_3$ obtained, when an etched copper circuit board was washed, required $40 \mathrm{mL}$ of $0.1\mathrm{M}$ hydrazine hydrochloride for its reduction to ${\mathrm{Fe}}^{2+}$. During this process hydrazine gets converted to ${\mathrm{N}}_2$. How many $\mathrm{mL}$ of $\frac{2}{3}\mathrm{M}$ nitric acid is required for the re-oxidation of ${\mathrm{Fe}}^{2+}$ to ${\mathrm{Fe}}^{3+}$ ?

[Given: Nitric acid gets reduced to $\mathrm{NO}$ during this process]

Maltose is converted to $\mathrm{A}$ by Maltase. The mole fraction of $\mathrm{A}$ in $10\% (\mathrm{w}/\mathrm{w})$ aq. solution is approximately:

Given liquid solution contains two components $\mathrm{A}$ and $\mathrm{B}$. Component $\mathrm{A}$ follows Henry's law for the mole fraction range $0\le X_A\le 0.1$ at constant temperature (and low pressure, where, it can be taken $\left[\frac{{\mathrm{x}}_{\mathrm{A}}\mathrm{d}\left({\mathrm{lnP}}_{\mathrm{A}}\right)}{{\mathrm{dx}}_{\mathrm{A}}}\right]+\left(1-{\mathrm{x}}_{\mathrm{A}}\right)\left[\frac{\mathrm{d}\left({\mathrm{lnP}}_{\mathrm{B}}\right)}{{\mathrm{dx}}_{\mathrm{A}}}\right]=0$) . Then component $\mathrm{B}$ must follow Raoult's law for the molefraction range $\mathrm{b}\le {\mathrm{X}}_{\mathrm{B}}\le 1$. What is the value of $\mathrm{b}$?

Explain the effect of temperature on mole fraction.

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.

Calculate the molality of pure water.

Calculate the molality of a $10\%$ solution of hydrochloric acid.

Calculate the molality of a solution prepared by dissolving $149.2 \mathrm{g}$ of $\mathrm{KCl}$ in $800 \mathrm{g}$ of water. 

(Atomic mass of $\mathrm{K}=39.1 \mathrm{u}$ and $\mathrm{Cl}=35.5 \mathrm{u}$)

Define molality.

$0.100 \mathrm{mol}$ 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?

Why mole fraction is independent of temperature?

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.