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 :

Liquid benzene  $\left({\mathrm{C}}_6{\mathrm{H}}_6\right)$ burns in oxygen according to the equation

$2{\mathrm{C}}_6{\mathrm{H}}_6\left(\mathrm{l}\right)+15{\mathrm{O}}_2\left(\mathrm{g}\right)\to 12{\mathrm{CO}}_2\left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

How many litres of  ${\mathrm{O}}_2$ at STP are needed to complete the combustion of $39 \mathrm{g}$ of liquid benzene?  $(\mathrm{Molecular}\mathrm{weight}\mathrm{of}{\mathrm{O}}_2=32,{\mathrm{C}}_6{\mathrm{H}}_6=78)$

Calculate mole fraction of $\mathrm{KI}$ if the density of $20\%$ (mass/mass) aqueous $\mathrm{KI}$ is $1.202 \mathrm{g} {\mathrm{mL}}^{-1}$.

Calculate molarity of $\mathrm{KI}$ if the density of $20\%$ (mass/mass) aqueous $\mathrm{KI}$ is $1.202 \mathrm{g} {\mathrm{mL}}^{-1}$.

Calculate molality of $\mathrm{KI}$ if the density of $20\%$ (mass/mass) aqueous $\mathrm{KI}$ is $1.202 \mathrm{g} {\mathrm{mL}}^{-1}$.

Calculate the molality and mole fraction of the solute in aqueous solution containing $3.0 \mathrm{g}$ of urea (molar mass= $60 \mathrm{g} {\mathrm{mol}}^{-1}$) per $250 \mathrm{g}$ of water?

The weight of ${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4.2{\mathrm{H}}_2\mathrm{O}$ required to prepare $500\mathrm{ml}$ of $0.2 \mathrm{N}$ solution is?

Calculate the molality of $2$ molar solution of urea having density $1.1 \mathrm{g}/\mathrm{ml}$?

Calculate the mass percent of a solution obtained by mixing $100 \mathrm{g}$of $10\%$ urea solution with $150 \mathrm{g}$ of $15\%$ urea solution.

What is the molarity of $1\mathrm{N} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution

$4.9 \mathrm{gm}$ of ${\mathrm{H}}_2{\mathrm{SO}}_4$ is present in $500 {\mathrm{cm}}^3$ of the solution has molarity

$300 \mathrm{ml}$ of $4.6\%$(by volume) of ethyl alcohol solution  is present in a container. If $100 \mathrm{ml}$ of this solution is taken and diluted with water such that final volume become $2$ litre. The molarity of diluted solution is (Density of pure ethyl alchohol is $2 \mathrm{g}/\mathrm{ml}$) 

$10 \mathrm{g}$ of glucose are dissolved in $150 \mathrm{g}$ of water. The mass $\%$ of glucose is

$1 \mathrm{g}$ mole of oxalic acid is dissolved in $2$ litre of solution. The concentration of solution is

$0.01$ mole of a non-electrolyte is dissolved in $10 \mathrm{g}$ of water. The molality of the solution is

In the given reaction, ${\mathrm{FeC}}_2{\mathrm{O}}_4+{\mathrm{KMnO}}_4\stackrel{{\mathrm{H}}^{+}}{\to }{\mathrm{Fe}}^{+3}+{\mathrm{CO}}_2+{\mathrm{Mn}}^{+2}$

If the equivalents of ${\mathrm{Fe}}^{+3}$ are $\text{'}\mathrm{a}\text{'}$, then the equivalents of ${\mathrm{FeC}}_2{\mathrm{O}}_4$ will be

One mole of ${\mathrm{H}}_2{\mathrm{SO}}_4$ is dissolved in $1000 \mathrm{mL}$ solution. Find Normality ?

$25\mathrm{ml}$ of aqueous solution of Hydrochloric acid containing $7.3 \mathrm{gms}$ of the acid per litre neutralised $30 \mathrm{ml}$ of aqueous solution of caustic soda. What is the normality of the alkali solution?

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R.

Assertion A: $3.1500 g$of hydrated oxalic acid dissolved in water to make $250.0 mL$ solution will result in $0.1 M$ oxalic acid solution.

Reason R: Molar mass of hydrated oxalic acid is $126 g mo{l}^{–1}$ .

In the light of the above statements, choose the correct answer from the options given below: 

$9 \mathrm{gms}$ of oxalic acid in $1 \mathrm{lt}$ solution, Find the molarity.