Concentration of Solutions of Solids in Liquids

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?

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.

$4.9 \mathrm{gm}$ 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

$25\mathrm{ml}$ 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.

$\mathrm{pH}$ of 1 litre of $\mathrm{HCl}$ solution is 1. How much water (in litres) is added to make $\mathrm{pH}=2$ ?

$2 \mathrm{g}$ of X is dissolved in $1$ mol of water. Find mass percentage of X in the solution?

Calculate the molarity of $\mathrm{NaOH}$ in the solution prepared by dissolving its $4 \mathrm{gm}$ in enough water to form $250 \mathrm{ml}$ of the solution.

The specific gravity of $98\% {\mathrm{H}}_2{\mathrm{SO}}_4$ is $1.8 \mathrm{g}/\mathrm{cc}$. $50 \mathrm{mL}$ of this solution is mixed with $1750 \mathrm{mL}$ of pure water. Molarity of resulting solution is : 

What is the total number of moles of ${\mathrm{H}}_2{\mathrm{SO}}_4$ needed to prepare $5.0 \mathrm{L}$ of a $2.0 \mathrm{M}$ solution of ${\mathrm{H}}_2{\mathrm{SO}}_4$ ?

$0.2$ mole of $\mathrm{HCl}$ and $0.1$ mole of ${\mathrm{CaCl}}_2$ were dissolved in water to have $500 \mathrm{mL}$ of solution, the molarity of ${\mathrm{Cl}}^{-}$ ions is :