$1.00 \ g$ of a non-electrolyte solute (molar mass $250 \ g \ mol^{-1}$) was dissolved in $51.2 \ g$ of benzene. If the freezing point depression constant,$K_f$ of benzene is $5.12 \ K \ kg \ mol^{-1},$ the freezing point of benzene will be lowered by .......... $K$.
- A$0.2$
- B$0.4$
- C$0.3$
- D$0.5$
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If $6 \ g$ of solute dissolved in $100 \ g$ of water lowers the freezing point by $0.93 \ K$. What is the molar mass of the solute? $(K_{f} = 1.86 \ K \ kg \ mol^{-1})$
Column-$I$ (Various solutions) Column-$II$ (Freezing point) $a$. $0.1 \, M \ BaCl_2$ solution $p$. $271 \, K$ $b$. $0.1 \, M \ NaCl$ solution $q$. $270 \, K$ $c$. $0.1 \, M \ K_3[Fe(CN)_6]$ solution $r$. $268 \, K$ $d$. $0.1 \, M \ Al_2(SO_4)_3$ solution $s$. $269 \, K$
Given: Freezing point of $0.1 \, M$ sucrose solution $= 272 \, K$ and freezing point of water $= 273 \, K$.
Which of the following options shows the correct matches?
| Column-$I$ (Various solutions) | Column-$II$ (Freezing point) |
|---|---|
| $a$. $0.1 \, M \ BaCl_2$ solution | $p$. $271 \, K$ |
| $b$. $0.1 \, M \ NaCl$ solution | $q$. $270 \, K$ |
| $c$. $0.1 \, M \ K_3[Fe(CN)_6]$ solution | $r$. $268 \, K$ |
| $d$. $0.1 \, M \ Al_2(SO_4)_3$ solution | $s$. $269 \, K$ |
Given: Freezing point of $0.1 \, M$ sucrose solution $= 272 \, K$ and freezing point of water $= 273 \, K$.
Which of the following options shows the correct matches?
Medium
View SolutionCalculate $\Delta T_{f}$ of aqueous $0.01 \ m$ formic acid if the van't Hoff factor is $1.1$. $[K_{f} = 1.86 \ K \ kg \ mol^{-1}]$ (in $K$)
Under identical conditions,which aqueous solutions have the same freezing point? (Molecular mass of urea $= 60 \ u$ and glucose $= 180 \ u$)
What is the value of $K_{f}$ if $30 \ g$ urea (molar mass $60$) dissolved in $0.5 \ dm^{3}$ of water decreases the freezing point by $0.15^{\circ}C$?
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