Reactions in Solutions

What do you mean by concentration in chemistry?

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 

Describe the fundamental of volumetric analysis.

A mixture of carbon monoxide and carbon dioxide is found to have a density of $1.7 \mathrm{g}/\mathrm{lit}$at S.T.P. The mole fraction of carbon monoxide is

During a titration, $240 \mathrm{ml} \mathrm{of} \mathrm{NaOH}$ reacted completely with $100 \mathrm{ml} \mathrm{of} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution. The weight of ${\mathrm{H}}_2{\mathrm{SO}}_4$ taken was $9.8 \mathrm{g}$.

How many grams of $\mathrm{NaOH}$ should be added to the original $\mathrm{NaOH}$ solution to make one litre of $0.5\mathrm{M}$  $\mathrm{NaOH}$ solution?

(Molecular mass of $\mathrm{NaOH}$is $40\mathrm{g}/\mathrm{mol}$ and molecular mass of ${\mathrm{H}}_2{\mathrm{SO}}_4 \mathrm{is} 98 \mathrm{g}/\mathrm{mol}$.)

During a titration, $240 \mathrm{ml} \mathrm{of} \mathrm{NaOH}$ reacted completely with $100 \mathrm{ml} \mathrm{of} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution. The weight of ${\mathrm{H}}_2{\mathrm{SO}}_4$ taken was $9.8 \mathrm{g}$.

 Calculate the amount of $\mathrm{NaOH}$dissolved in solution.

During a titration, $240 \mathrm{ml} \mathrm{of} \mathrm{NaOH}$ reacted completely with $100 \mathrm{ml} \mathrm{of} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution. The weight of ${\mathrm{H}}_2{\mathrm{SO}}_4$ taken was $9.8 \mathrm{g}$.

What is the molarity of the $\mathrm{NaOH}$used?

Molar concentration of a solution of water is:

A liquid has density $1.5 \mathrm{g}/\mathrm{cc}.$ $50 \mathrm{cc}$ of it is mixed with $30 \mathrm{cc}$ of water. What will be the density of mixture solution ?

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.

$200 \mathrm{mL}$ 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.

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

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)

$7.45 \mathrm{g}$ of potassium chloride ($\mathrm{KCl}$) was dissolved in $100 \mathrm{g}$ of water. Calculate the molality of the solution.

A tank contains $5$ moles of oxygen, $2$ moles of nitrogen and $20 \mathrm{g}$ of hydrogen gases at room temperature. Find the mole fraction of hydrogen.