Question

For the coagulation of 500 ml of a sulphide sol, 5 ml of 0.2 M CaCl2 solution is required. The flocculation value of CaCl2 is Options=2,5,20,120

Answer 1

Given:

For the coagulation of 500 ml of a sulphide sol, 5 ml of 0.2 M CaCl2 solution is required

To find:

The flocculation value of CaCl2

Solution:

We know that,

1 Molar solution contains 1 Mole in 1 Litre

So, here we have

0.2 M of Cacl₂ contains 0.2 mol/L

Therefore, we can also say

1000 ml of CaCl₂ contains 0.2 moles of CaCl₂

∴ 5 ml of CaCl₂ contains,

= $\frac{0.2}{1000} \times 5$

= $2\times 10^-^4 \times 5$

= $1 \times 10^-^3 \:moles$

= $1\:mmoles$

Now,

$\boxed{\bold{Flocculation\:Value}}$ : The concentration or the number of millimoles of an electrolyte solution that is required to cause the coagulation of one litre of a colloidal solution is called the flocculation value of the colloidal solution.

According to the question, we have

If 500 ml of sol requires 1 mmoles for coagulation

Then 1 L or 1000 ml sol will require = $\frac{1}{500}\times 1000 = \bold{2 \:mmoles\:for\:coagulation}$ ← option:- (1)

Thus, the flocculation value of CaCl₂ is 2 mmoles.

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