Reactions in Solutions

What do you mean by concentration in chemistry?

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 ?

$200 \mathrm{mL}$ 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:

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

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

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

The density of $2\mathrm{M}$ aqueous solution of $\mathrm{NaOH}$ is $1.28 \mathrm{g}/{\mathrm{cm}}^3$. The molality of the solution is :

What is the mass percentage of sodium in sodium carbonate?

Calculate mole fraction of solute and solvent of the following:

(i) $15 \mathrm{g}$ of urea$(\mathrm{Molar} \mathrm{mass}=60)$ dissolved in $40 \mathrm{g} \mathrm{of} {\mathrm{H}}_2\mathrm{O}$.

(ii) $30 \mathrm{g}$ of glucose$\left(\mathrm{Molar} \mathrm{mass}=180\right)$ dissolved in $270 \mathrm{g} \mathrm{of} {\mathrm{H}}_2\mathrm{O}$

$250 \mathrm{mL}$ of a calcium carbonate solution contains $2.5$ grams of ${\mathrm{CaCO}}_3$. If $10 \mathrm{mL}$ of this solution is diluted to one litre, what is the concentration of the resultant solution? 

 The molarity of urea solution containing $6.02\times {10}^{20}$ molecules of urea are present in $100\mathrm{ml}$ of its solution is

The amount of ${\mathrm{H}}_2{\mathrm{O}}_2$ present in $1 \mathrm{L}$ of $1.5 \mathrm{N} {\mathrm{H}}_2{\mathrm{O}}_2$ solution is

What mass of sodium carbonate is required to prepare its $0.05 \mathrm{M}$ aqueous solution in $250 \mathrm{mL}?$