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Van't Hoff Factor

The observed ...

Question

The observed osmotic pressure for a $0.10 M$ solution of $F e {({N H}_{4})}_{2} {({S O}_{4})}_{2}$ at $25^{o} C$ is $10.8$ atm. The expected and experimental (observed) values of Van't Hoff factor (i) will be respectively:
$(R = 0.082 L a t m k^{-} {m o l}^{- 1})$

5

and

4.42

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4

and

4.00

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5

and

3.42

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3

and

5.42

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Solution

The correct option is A $5$ and $4.42$
$π = i C R T$
$10.8 = i \times 0.1 \times 0.082 \times 298$ (Experimental value)
$∴ i = \frac{10.8}{0.1 \times 0.082 \times 298}$
$∴ i = 4.42 \to$ Experimental value
Expected value $= 5$

Suggest Corrections

Similar questions

F e (N H_{4})_{2} (S O_{4})_{2}

25^{o} C

[R = 0.082 L a t m K^{- 1} m o l^{- 1}]

0.10 M

F e (N H_{4}) 2 (S O_{4})_{2}

25 ° C

10.8 atm

[R = 0.082 L {atm K}^{- 1} {mol}^{- 1}]

The osmotic pressure of a 0.010 M MgSO₄ solution at 500 K is 0.82 atm. Calculate , the van't Hoff factor, for this MgSO₄ solution.

5 %

25^{o} C

= 180

R = 0.0821

K^{- 1} m o l^{- 1}

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i = 2.47

2.5 L

300 K

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C a C l_{2}

111 g . m o l^{- 1}

R = 0.082 L . a t m . K^{- 1} m o l^{- 1}

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