What should be the molarity of aqueous solution of K_2SO_4 so that it is isotonic with aqueous 1\ M glucose at same temperature, assuming complete dissociation?

Question

Quantrex Academy · Accepted Answer

Correct answer: C. 0.333\ M

For isotonic solutions, the osmotic pressures are equal.

\pi_1 = \pi_2

i_1 C_1 RT = i_2 C_2 RT

For glucose,

i_1 = 1

and

C_1 = 1\ \text{M}

.

For

\text{K}_2\text{SO}_4

, assuming complete dissociation, it yields

2\text{K}^+

and

\text{SO}_4^{2-}

, so

i_2 = 3

. Let its molarity be

C_2

.

1 \times 1 = 3 \times C_2

C_2 = \dfrac{1}{3}\ \text{M} = 0.333\ \text{M}

Answer:

0.333\ \text{M}

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