Chapter 2

Concentrated nitric acid used in the laboratory work is \(68 \%\) nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of solution is \(1.504 \mathrm{~g} \mathrm{~mL}^{-1}\) ?

A solution of glucose in water is labelled as 10 per cent \(w / w\), what would be the molality and mole fraction of each component in the solution? If the density of the solution is \(1.2 \mathrm{~g} \mathrm{~mL}^{-1}\), then what shall be the molarity of the solution?

An antifreeze solution is prepared from \(222.6 \mathrm{~g}\) of ethylene glycol \(\left[\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{OH})_{2}\right]\) and \(200 \mathrm{~g}\) of water. Calculate the molality of the solution. If the density of the solution is \(1.072 \mathrm{~g} \mathrm{~mL}^{-1}\) then what shall be the molarity of the solution?

Calculate the amount of oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}\right)\) required to obtain \(250 \mathrm{~mL}\) of deci-molar solution.

\(4 \mathrm{~g}\) of \(\mathrm{NaOH}\) are present in \(0.1 \mathrm{dm}^{3}\) solution have specific gravity \(1.038 \mathrm{~g} / \mathrm{mL}\). Calculate : (a) mole fraction of \(\mathrm{NaOH}\); (b) molality of \(\mathrm{NaOH}\) solution; (c) molarity of \(\mathrm{NaOH}\) solution; (d) normality of \(\mathrm{NaOH}\) solution.

Suppose \(5 \mathrm{~g}\) of acetic acid are dissolved in one litre of ethanol. Assume no reaction in between them. Calculate molality of resulting solution if density of ethanol is \(0.789 \mathrm{~g} / \mathrm{mL}\).

What are the final concentrations of all the ions when following are mixed? \(50 \mathrm{~mL}\) of \(0.12 \mathrm{M} \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}, 100 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{FeCl}_{3}\) and \(100 \mathrm{~mL}\) of \(0.26 \mathrm{M} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\)

\(30 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{BaCl}_{2}\) is mixed with \(40 \mathrm{~mL}\) of \(0.2 \mathrm{M} \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\). What is the weight of \(\mathrm{BaSO}_{4}\) formed? $$ \mathrm{BaCl}_{2}+\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} \longrightarrow \mathrm{BaSO}_{4}+\mathrm{AlCl}_{3} $$

Calculate the volume of \(1.00 \mathrm{~mol} \mathrm{~L}^{-1}\) aqueous sodium hydroxide that is neutralized by \(200 \mathrm{~mL}\) of \(2.00 \mathrm{~mol} \mathrm{~L}^{-1}\) aqueous hydrochloric acid and the mass of sodium chloride produced. Neutralization reaction is; $$ \mathrm{NaOH} \text { (aq.) }+\mathrm{HCl} \text { (aq.) } \longrightarrow \mathrm{NaCl}(\mathrm{aq} .)+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) $$