Van't Hoff Factor

Determine $\mathrm{i}$(vant-Hoff factor) for a tribasic acid ${\mathrm{H}}_3\mathrm{A}.$ Assuming first dissociation to be $100\%,$ second dissociation $50\%,$ third dissociation $20\%,$ (Round off your answer to nearest integer).

Which of the following has the lowest freezing point and the highest boiling point?

Determination of the molar mass of acetic acid in benzene solvent, using freezing point depression is affected by: 

${\mathrm{MX}}_2$ dissociates into ${\mathrm{M}}^{2+}$ and ${\mathrm{X}}^{-}$ ions in an  aqueous solution, with a' degree of dissociation $\left(\mathrm{\alpha }\right)$ of $0.5.$  The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is 

If relative decrease in vapour pressure is $0.4$ for a solution containing $1 \mathrm{mol}$ $\mathrm{NaCl}$ in $3 \mathrm{mol} {\mathrm{H}}_2\mathrm{O}, \mathrm{NaCl}$ is _____ $\%$  ionised.

Complete the following table.

The freezing point of the benzene decreases by $0.45° \mathrm{C}$ when $0.2 \mathrm{g}$of acetic acid is added to $20 \mathrm{g}$ of benzene. If acetic acid associates to form a dimer in benzene, the percentage association of acetic acid will be ( ${\mathrm{K}}_{\mathrm{f}}$ for benzene $=5.12 \mathrm{K} \mathrm{Kg} {\mathrm{mol}}^{-1}$)

In aqueous solution of $1\times {10}^{-3}$ molal ${\mathrm{K}}_x\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]$ depression in freezing point is $7.2\times {10}^{-3} \mathrm{K}$. Determine the sum of primary and secondary valency of complex $\left({\mathrm{K}}_{\mathit{f}}\right.$ of $\left.{\mathrm{H}}_2\mathrm{O}=1.8 \mathrm{K} \mathrm{Kg}/\mathrm{mole}\right)$. (Assume that $\%$ ionisation of complex is $100\%$)

Available are $1 \mathrm{L}$ of $0.1 \mathrm{M} \mathrm{NaCl}$ and $2 \mathrm{L} \mathrm{of} 0.2 \mathrm{M} {\mathrm{CaCl}}_2$ solutions. Using only these two solutions, what maximum volume of a solution can be prepared having $[{\mathrm{Cl}}^{–} ]=0.34 \mathrm{M}$ exactly. Both electrolytes are strong.

Assuming each salt to be $90\%$ dissociated which of the following will have highest osmotic pressure?

  What will be the molecular weight of $\mathrm{NaCl}$ determined experimentally from elevation in the boiling point or depression in freezing point method?

Consider separate solution of $0.500 \mathrm{M} {\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}\left(\mathrm{aq}\right), 0.100 \mathrm{M} {\mathrm{Mg}}_3\left({\mathrm{PO}}_4{)}_2\right(\mathrm{aq}), 0.250 \mathrm{M} \mathrm{KBr}(\mathrm{aq})$ and $0.125 \mathrm{M} {\mathrm{Na}}_3{\mathrm{PO}}_4\left(\mathrm{aq}\right)$ at $25°\mathrm{C}$. Which statement is true about these solution, assuming all salts to be strong electrolytes ?

If $\mathrm{\alpha }$ is the degree of dissociation of ${\mathrm{Na}}_2{\mathrm{SO}}_4$, the Van't Hoff factor $\left(\mathrm{i}\right)$ used for calculating the molecular mass is

In which of the following pairs of solutions will the values of the Vant Hoff factor be the same?

A solute $\mathrm{S}$ undergoes a reversible trimerization, when dissolved in a certain solvent. The boiling point elevation of its $0.1 \mathrm{molal}$ solution was found to be identical to the boiling point elevation in case of a $0.08 \mathrm{molal}$ solution of a solute which neither undergoes association nor dissociation. To what percent had the solute $‘\mathrm{S}’$ undergone trimerization?

A $0.01$ molal solution of ammonia freezes at $-0.02°\mathrm{C}$. Calculate the Van’t Hoff factor, $\mathrm{i}$, and the percentage dissociation of ammonia in water.$\left( {\mathrm{K}}_{\mathrm{f}\left({\mathrm{H}}_2\mathrm{O}\right)}=1.86 \mathrm{K} {\mathrm{molal}}^{–1} \right)$

Calculate the percentage of the degree of dissociation of an electrolyte ${\mathrm{XY}}_2$ (Normal molar mass$=164$) in water if the observed molar mass by measuring the elevation in boiling point is $65.6$.

The degree of dissociation of an electrolyte is a and its van’t Hoff factor is i. The number of ions obtained by complete dissociation of 1 molecule of the electrolyte is :

The Van't Hoff factor for $0.1 \mathrm{M} \mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2$ solution is $2.74.$ The degree of dissociation is

In the following aqueous solutions
A. $1\mathrm{}\mathrm{m}$ sucrose
B. $1\mathrm{}\mathrm{m}$ potassium ferricyanide and
C. $1\mathrm{}\mathrm{m}$ potassium sulphate,
maximum value of vapour pressure of solution is that of