Concentration Terms

A solution of sugar is obtained by mixing $200 \mathrm{g}$ of its $25\%$ solution and $500 \mathrm{g}$of its $40\%$solution (both by mass). The mass percentage of the resulting sugar solution is _______ (Nearest integer)

A solution is prepared by adding $2 \mathrm{g}$ of $\text{'}\text{'}\mathrm{X}\text{'}\text{'}$ to $1$ mole of water. Mass percent of $\text{'}\text{'}\mathrm{X}\text{'}\text{'}$in solution is 

Calculate the mole fraction  of $\mathrm{NaCl}$ in the system containing $0.5 \mathrm{mol} \mathrm{NaCl}$ and $10 \mathrm{mol} {\mathrm{H}}_2\mathrm{O}$

Round off the answer up to three significant figures.

$100 {\mathrm{cm}}^3$of a given sample of ${\mathrm{H}}_2{\mathrm{O}}_2$ gives $1000 {\mathrm{cm}}^3$ of ${\mathrm{O}}_2$ at S.T.P. The given sample is

$200 \mathrm{mL}$ of $\frac{\mathrm{M}}{4}\mathrm{HCl}$ solution was diluted to make it $\frac{\mathrm{M}}{10}\mathrm{HCl}$ solution. The volume of water needed for the dilution is:

How much $\mathrm{NaCl}$ is to be dissolved in 60 g water to form a solution of 20% by mass?

$2.0$ molar solution is obtained when $0.5$ mole solute is dissolved in:

$3\mathrm{M}$ and $30 \mathrm{mL}$ of calcium hydroxide reacted with $6\mathrm{M}$ and $50\mathrm{mL} {\mathrm{H}}_2{\mathrm{SO}}_4$, Then find the molarity of resulting solution.

Find the amount of dibasic acid with molecular weight 200, required to produce 100ml of 0.1 N aqueous solutions

400 gram 20% weight/weight solution on cooling gives 30 gram precipitate then find out percentage weight/weight of remaining solution.

The volume of water to be added to 400 ml of N/8 HCI to make it exactly N/12 is

A $100 \mathrm{g}$ mixture of alcohol and water contains $54 \mathrm{g}$ water. Calculate the mole fraction of alcohol and water in this solution.

(Alcohol = ethanol)

$100 \mathrm{ml}$ of $0.2 \mathrm{N} \mathrm{HCl}$ solution is added to $100 \mathrm{ml}$ of $0.2 \mathrm{N} {\mathrm{AgNO}}_3$ solution. The molarity of nitrate ions in the resulting mixture will be

Density of a solution of $\mathrm{NaCl}$ in a polar solvent is $1.2 \mathrm{gm}/\mathrm{cc}$. If $\%$ by weight ($\mathrm{W}/\mathrm{W}$) of $\mathrm{NaCl}$ in solution is $5.85$, then formality and $\%$ by volume ($\mathrm{W}/\mathrm{V}$) of $\mathrm{NaCl}$ are-

The number of millimoles of ${\mathrm{H}}_2{\mathrm{SO}}_4$present in 5 litres of $0.2 \mathrm{N} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution is

A sample of an ethanol–water solution has a volume of $55.0 {\mathrm{cm}}^3$ and a mass of $50.0 \mathrm{g}$. What is the percentage of ethanol (by mass) in the solution? Assume that there is no change in volume when the pure compounds are mixed. The density of ethanol is $0.80 \mathrm{g}/{\mathrm{cm}}^3$ and that of water is $1.00 \mathrm{g}/{\mathrm{cm}}^3$.

Round off your answer to the nearest integer.

The density of $3 \mathrm{M}$ solution of NaCl is $1.2 \mathrm{gm}/\mathrm{ml}$. Calculate the molality of the solution.

Round off your answer to the nearest integer.

Commercially available concentrated hydrofluoric acid contains $38\% \mathrm{HF}$ by volume$\left(\raisebox{1ex}{$\mathrm{v}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{V}$}\right.\%\right)$. The density of $\mathrm{HF}$ is $1.19 \mathrm{g} {\mathrm{ml}}^{-1}$ and density of solution is $1.39 \mathrm{g} {\mathrm{ml}}^{-1}$. What is the molality of this solution?