Ionic EquilibriumHard

Question

At 40o C, the density of heavy water is 1.02 g/ml and its ionic product is 5.1 × 10−15. Which of the following if the only incorrect information regarding heavy water at 40o C?

Options

A.The molar concentration of heavy water is 51 M.
B.The dissociation constant of heavy water is 10−16.
C.Its degree of dissociation is 10−8.
D.The molal concentration of heavy water is 50 m.

Solution

$(a)\left\lbrack D_{2}O \right\rbrack = \frac{d}{M} = \frac{1.02 \times 10^{3}\text{ g/L}}{20\text{ g/mol}} = 51\text{ M}$

$(b)K_{d} = K_{w}/\left\lbrack D_{2}O \right\rbrack = \frac{5.1 \times 10^{- 15}}{51} = 10^{- 15} $$${(c)\left\lbrack D^{+} \right\rbrack = \left\lbrack OD^{-} \right\rbrack = \sqrt{K_{w}} }{\therefore\alpha = \frac{\sqrt{K_{w}}}{C} = \frac{\sqrt{5.1 \times 10^{- 15}}}{51} = \frac{10^{- 8}}{\sqrt{51}} }{(d)\text{Molality = }\frac{1000}{20} = 50\text{ m}}$$

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