An aqueous solution of sucrose, containing 34.2 gm of $C_{12} H_{22} O_{11}$ , has an osmotic pressure of $2.38$ atm at $17^{o} C$ . For an aqueous solution of glucose, $C_{6} H_{12} O_{6}$ to be isotonic with the solutions, it would have:

34.2 gm of glucose

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17.1 gm of glucose

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18.0 gm of glucose

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36.0 gm of glucose

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Solution

The correct option is C 18.0 gm of glucose
The expression for the osmotic pressure is $Π = C R T$ . Two solutions are isotonic when they have the same osmotic pressure.

Thus, $Π (s u c r o s e) = Π (g l u c o s e)$

$C (s u c r o s e) R T = C (g l u c o s e) R T$

This will be true when the number of moles of glucose is equal to the number of moles of sucrose.

Hence, the mass of glucose is $34.2 \times \frac{180}{342} = 18.0 g$ .

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An aqueous solution of sucrose, containing 34.2 gm of C12H22O11, has an osmotic pressure of 2.38 atm at 17oC. For an aqueous solution of glucose, C6H12O6 to be isotonic with the solutions, it would have:

An aqueous solution of sucrose, containing 34.2 gm of $C_{12} H_{22} O_{11}$ , has an osmotic pressure of $2.38$ atm at $17^{o} C$ . For an aqueous solution of glucose, $C_{6} H_{12} O_{6}$ to be isotonic with the solutions, it would have: