Chapter 10

\(100 \mathrm{~g}\) of \(\mathrm{NaCl}\) is stirred in \(100 \mathrm{~mL}\) of water at \(20^{\circ} \mathrm{C}\) till the equilibrium is attained : (a) How much \(\mathrm{NaCl}\) goes into the solution and how much of it is left undissolved at equilibrium? The solubility of \(\mathrm{NaCl}\) at \(20^{\circ} \mathrm{C}\) is \(6.15\) mol/litre. (b) What will be the amount of \(\mathrm{NaCl}\) left undissolved if the solution is diluted to \(200 \mathrm{~mL} ?\)

Calculate the concentration of \(\mathrm{CO}_{2}\) in a soft drink that is bottled with a partial pressure of \(\mathrm{CO}_{2}\) of \(4.0 \mathrm{~atm}\) over the liquid at \(25^{\circ} \mathrm{C}\). The Henry's law constant for \(\mathrm{CO}_{2}\) in water is \(3.1 \times 10^{-2} \mathrm{~mol} /\) litre-atm at this temperature.

Calculate the concentration of \(\mathrm{CO}_{2}\) in a soft drink bottle after the bottle is opened and sits at \(25^{\circ} \mathrm{C}\) under a \(\mathrm{CO}_{2}\) partial pressure of \(3.0 \times 10^{-4} \mathrm{~atm}\). Henry's law constant for \(\mathrm{CO}_{2}\) in water is \(3.1 \times 10^{-2}\) mol/litre-atm at this temperature.