Question

What is the osmotic pressure of 12% solution of cane sugar (molecular weight 342) at 17°C.
12 g sugar is dissolved in 100 mL​

Answer 1

Explanation:

Moles sugar = 5g342g/mol=0.0146 mass solution = 100 g assuming d = 1 g/mL volume solution = 100 mL = 0.100 L

Answer 2

The osmotic pressure of 12% solution of cane sugar is 8.35 atm

Explanation:

Osmotic pressure is a colligative property which depends on the amount of solute added.

$\pi=iCRT$

$\pi$ = osmotic pressure

i= vant hoff factor = 1 ( for sucrose)

C= concentration in Molarity

R= solution constant = 0.0821 Latm/Kmol

T= temperature in Kelvin = $17^0C=(17+273)K=290K$

12 g of sugar in dissolved in 100 ml of solution

moles of sugar =$\frac{\text {given mass}}{\text {molar mass}}=\frac{12g}{342g/mol}=0.035moles$

Molarity=$\frac{0.035moles\times 1000}{100ml}=0.35mole/L$

$\pi=1\times 0.35\times 0.0821\times 290=8.35atm$

Thus the osmotic pressure of 12% solution of cane sugar is 8.35 atm

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