We have three aqueous solutions of NaCl labelled as ‘A’, ‘B’ and 'C' with concentrations 0.1 M, 0.01 M and 0.001 M, respectively. The value of van’t Hoff factor for these solutions will be in the order.

Question

We have three aqueous solutions of NaCl labelled as ‘A’, ‘B’ and 'C' with concentrations 0.1 M, 0.01 M and 0.001 M, respectively. The value of van’t Hoff factor for these solutions will be in the order. (A) iA < iB < iC (B) iA > iB > iC (C) iA = iB = iC (D) iA < iB > iC

Tardigrade Admin · Accepted Answer

As NaCl is a strong electrolyte, it undergoes dissociation completely. Thus, varit Hoff factor will be same for all these solutions, iA = iB = iC.

Q. We have three aqueous solutions of $N a Cl$ labelled as ‘ $A$ ’, ‘ $B$ ’ and ' $C$ ' with concentrations $0.1 M$ , $0.01 M$ and $0.001 M$ , respectively. The value of van’t Hoff factor for these solutions will be in the order.

$i_{A} < i_{B} < i_{C}$

$i_{A} > i_{B} > i_{C}$

$i_{A} = i_{B} = i_{C}$

$i_{A} < i_{B} > i_{C}$

As $N a Cl$ is a strong electrolyte, it undergoes dissociation completely. Thus, varit Hoff factor will be same for all these solutions, $i_{A} = i_{B} = i_{C}$ .

Q. We have three aqueous solutions of NaCl labelled as ‘A’, ‘B’ and 'C' with concentrations 0.1M, 0.01M and 0.001M, respectively. The value of van’t Hoff factor for these solutions will be in the order.

iA​<iB​<iC​

iA​>iB​>iC​

iA​=iB​=iC​

iA​<iB​>iC​