Chapter 2

Find the weight of \(\mathrm{NaOH}\) in its 60 milli-equivalents.

Find the normality of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) having 50 milli- equivalents in 3 litre.

What volume of water is required to make \(0.20 \mathrm{~N}\) solution from \(1600 \mathrm{~mL}\) of \(0.2050 \mathrm{~N}\) solution?

How would you prepare exactly \(3.0\) litre of \(1.0 \mathrm{M} \mathrm{NaOH}\) by mixing proportions of stock solutions of \(2.50 \mathrm{M} \mathrm{NaOH}\) and \(0.40 \mathrm{M} \mathrm{NaOH}\). No water is to be used.

Calculate normality of \(\mathrm{NH}_{4} \mathrm{OH}\) when \(2 \mathrm{~g}\) is present in \(800 \mathrm{~mL}\) solution. Also calculate its molarity.

Calculate the concentration of a solution obtained by mixing \(300 \mathrm{~g}\) \(25 \%\) by weight solution of \(\mathrm{NH}_{4} \mathrm{Cl}\) and \(150 \mathrm{~g}\) of \(40 \%\) by weight solution of \(\mathrm{NH}_{4} \mathrm{Cl}\)

A sample of \(\mathrm{NaOH}\) weighing \(0.38 \mathrm{~g}\) is dissolved in water and the solution is made to \(50.0 \mathrm{~mL}\) in a volumetric flask. What is the molarity of the resulting solution?

How many moles of \(\mathrm{NaOH}\) are contained in \(27 \mathrm{~mL}\) of \(0.15 \mathrm{M} \mathrm{NaOH}\) ?

In a reaction vessel \(0.184 \mathrm{~g}\) of \(\mathrm{NaOH}\) is required to be added for completing the reaction. How many millilitre of \(0.150 \mathrm{M} \mathrm{NaOH}\) solution should be added for this requirement.

Commercially available concentrated hydrochloric acid contains \(38 \%\) \(\mathrm{HCl}\) by mass. (a) What is the molarity of this solution? The density is \(1.19 \mathrm{~g} \mathrm{~mL}^{-1}\). (b) What volume of concentrated \(\mathrm{HCl}\) is required to make \(1.00\) litre of \(0.10 \mathrm{M} \mathrm{HCl} ?\)