What should be the molarity of aqueous solution of K 2 SO 4 so that it is isotonic with aqueous 1 M glucose at same temperature, assuming complete dissociation?

Question

What should be the molarity of aqueous solution of K 2 ​ SO 4 ​ so that it is isotonic with aqueous 1 M glucose at same temperature, assuming complete dissociation?

TestHub · Accepted Answer

For isotonic solutions, the osmotic pressures are equal.

$π_{1} = π_{2}$

$i_{1} C_{1} RT = i_{2} C_{2} RT$

For glucose, $i_{1} = 1$ and $C_{1} = 1 M$ .

For $K_{2} SO_{4}$ , assuming complete dissociation, it yields $2 K^{+}$ and $SO_{4}^{2 -}$ , so $i_{2} = 3$ . Let its molarity be $C_{2}$ .

$1 \times 1 = 3 \times C_{2}$

$C_{2} = \frac{1}{3} M = 0.333 M$

Answer: $0.333 M$

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