Single Choice

A $$1.2$$% of solution of $$NaCl$$ is isotonic with $$7.2$$% of solution of glucose. Calculate the van't Hoff's factor of $$NaCl$$ solution.

A2.36
B1.5
C1.95
Correct Answer
D1

Solution

The molar masses of NaCl and glucose are 58.5 g/mol and 180 g/mol respectively.
The expression for the osmotic pressure is as follows:
$$\pi =iCRT$$
Since the two solutions are isotonic, they have equal osmotic pressure.

$$\pi (NaCl)=\pi (glucose)$$

$$i_{NaCl}\times \dfrac{1.2}{58.5}=1\times \dfrac{7.2}{180}$$

$$i_{NaCl}=1.95$$

SIMILAR QUESTIONS

Solutions

In which case van't Hoff factor is maximum (assuming no hydrolysis)?

Solutions

At same temperature which pair of the following solutions are isotonic?

Solutions

The value of van't Hoff factors for $$KCl, NaCl$$ and $${K}_{2}{SO}_{4}$$, respectively, are :

Solutions

If $$\alpha$$ is the degree of dissociation of $${Na}_{2}{SO}_{4}$$, the vant Hoff's factor ($$i$$) used for calculating the molecular mass is:

Solutions

Which of the following salt has the same value of Van't Hoff factor i as that of $$K_3 [Fe(CN)_6]$$?

Solutions

The Van't Hoff factor, i for a $$0.2$$ molal aqueous solutions of urea is:

Solutions

The Van't Hoff factor for sodium phosphate would be:

Solutions

The freezing point of a solution containing 5.85 g of $$NaCl$$ in 100g of water is $$-3.348^o$$C. Calculate van't Hoff factor 'i' for this solution. What will be the experimental molecular weight of NaCI? ($$K_f$$ for water = $$1.86 K kg mol^{-1}$$, at. wt. Na = 23, Cl = 35.5)

Contact Details