The ratio of the value of any colligative property for $KCl$ solution to that for sugar solution is nearly

In comparison to a $0.01 \ M$ solution of glucose,the depression in freezing point of a $0.01 \ M \ MgCl_2$ solution is (Molecular weight of $MgCl_2 = 95$,molecular weight of glucose $= 180$).

The experimental molecular weight of an electrolyte will always be less than its calculated value because the value of Van't Hoff factor $i$ is

Considering acetic acid dissociates in water,its dissociation constant is $6.25 \times 10^{-5}$. If $5 \ mL$ of acetic acid is dissolved in $1 \ L$ water,the solution will freeze at $-x \times 10^{-2} \ {}^{\circ}C$,provided pure water freezes at $0 \ {}^{\circ}C$.
$x = . . . . . . . . .$ (Nearest integer)
Given: $(K_{f})_{\text{water}} = 1.86 \ K \ kg \ mol^{-1}$.
Density of acetic acid is $1.2 \ g \ mL^{-1}$.
Molar mass of water $= 18 \ g \ mol^{-1}$.
Molar mass of acetic acid $= 60 \ g \ mol^{-1}$.
Density of water $= 1 \ g \ cm^{-3}$.
Acetic acid dissociates as:
$CH_3COOH \rightleftharpoons CH_3COO^{-} + H^{+}$

Of the following four aqueous solutions,the total number of those solutions whose freezing point is lower than that of $0.10 \, M \, C_{2}H_{5}OH$ is (Integer answer).
$(i)$ $0.10 \, M \, Ba_{3}(PO_{4})_{2}$
$(ii)$ $0.10 \, M \, Na_{2}SO_{4}$
$(iii)$ $0.10 \, M \, KCl$
$(iv)$ $0.10 \, M \, Li_{3}PO_{4}$

The freezing point of a $1.00 \ m$ aqueous solution of $HF$ is found to be $-1.91 \ ^oC$. The freezing point constant of water,$K_f$ is $1.86 \ K \ kg \ mol^{-1}$. The percentage dissociation of $HF$ at this concentration is ................ $\%$