Questions in solutions

SelectQuestion
Assertion (A) : The freezing point is the temperature at which solid crystallizes from solution. Reason (R) : The freezing point depression is the difference between that temperature and freezing point of pure solvent
15 g of a substance dissolved in $150 g$ of water produces a depression of 1.2°C in the freezing point. The molecular mass of solid is (${{K}_{b}}$for water is $18.5\,K\,mo{{l}^{-1}}\,\,100\,g$)
The molal freezing point constant for water is 1.86°C. Therefore, the change in freezing point of 0.1 m of NaCl solution in water is expected to be
What is the molality of solution of a certain solute in a solvent, if there is a freezing point depression of 0.184°C and if the freezing point constant is 18.4
A 0.5 molal solution of ethylene glycol in water is used as coolant in a car. If the freezing point constant of water be 1.86°C per mole, the mixture shall freeze at
Given that $\Delta {{T}_{f}}$is the depression in freezing point of the solvent in a solution of a non-volatile solute of molality m the quantity $\underset{m\to 0}{\mathop{\text{lim}}}\,\left( \frac{\Delta {{T}_{f}}}{m} \right)$is equal to
8 g of HBr is added in 100 g of ${{H}_{2}}O$. The freezing point will be $({{K}_{f}}=1.86,\,H=1,\,Br=80)$
$PtC{{l}_{4}}.6{{H}_{2}}O$can exist as a hydrated complex 1 molal aq. solution has depression in freezing point of 3.72°. Assume 100% ionisation and ${{K}_{f}}({{H}_{2}}O)=1.86{}^\circ \,mo{{l}^{-1}}\,kg,$then complex is
Maximum freezing point will be for 1 molal solution of, assuming equal ionisation in each case :
Depression of freezing point of 0.01 molal aq. $C{{H}_{3}}COOH$solution is 0.02046°.1 molal urea solution freezes at – 1.86°C. Assuming molality equal to molarity, pH of $C{{H}_{3}}COOH$solution is

View Selected Questions (0)

Back to Categories

Back to Home