Advertisements
Advertisements
प्रश्न
A 0.1 m solution of K2SO4 in water has a freezing point of –4.3°C. What is the value of van’t Hoff factor if Kf for water is 1.86 K kg mol–1?
Advertisements
उत्तर
Given: Molality of K2SO4 solution = m = 0.1 m
Freezing point of solution = Tf = – 4.3 °C
Kf of water = 1.86 K kg mol–1
To find: van’t Hoff factor
Formula: ΔTf = i Kfm
Calculation:
ΔTf = `"T"_"f"^0` – Tf
= 0 °C – (–4.3 °C) = 4.3 °C = 4.3 K
Now, using the formula,
ΔTf = i Kf.m
∴ i = `(Δ"T"_"f")/("K"_"f"."m")`
`= (4.3 "K")/(1.86 "k kg mol"^-1 xx 0.1 "mol kg"^-1)`
= 23.11
The value of van’t Hoff factor is 23.11.
APPEARS IN
संबंधित प्रश्न
Answer the following in one or two sentences.
What is van’t Hoff factor?
Answer the following in one or two sentences.
How is van’t Hoff factor related to degree of ionization?
Answer the following in one or two sentences.
Which of the following solution will have higher freezing point depression and why?
i. 0.1 m NaCl
ii. 0.05 m Al2(SO4)3
Answer the following in one or two sentences.
Which of the four colligative properties is most often used for molecular mass determination? Why?
Derive the relationship between the degree of dissociation of an electrolyte and van’t Hoff factor.
At 25 °C, a 0.1 molal solution of CH3COOH is 1.35 % dissociated in an aqueous solution. Calculate the freezing point and osmotic pressure of the solution assuming molality and molarity to be identical.
A 0.15 m aqueous solution of KCl freezes at - 0.510 °C. Calculate i and osmotic pressure at 0 °C. Assume the volume of solution equal to that of water.
At T (K), the molar ionic conductivities of NH; and OH− at infinite dilution are 72 and 198 S cm2 mol−1 respectively. The molar conductivity of 0.01 M NH4OH solution at the same temperature is found to be 9 S cm2 mol−1. The percentage dissociation of NH4OH at this concentration is ____________.
It a centimolal aqueous solution of K3[Fe(CN)6] has degree of dissociation 0.78. What is the value of van't Hoff factor?
Relationship between van't Hoff's factor (i) and degree of dissociation (α) is ______.
If van't Hoff factor of monofluoroacetic acid in water is 1.076. What is it's degree of dissociation?
Van't Hoff factor for K3[Fe(CN)6] is 3.333. What is it's percentage dissociation in water?
Why is observed molar mass of acetic acid in benzene is greater than actual molar mass?
Which of following 0.1 m aqueous solution exhibits highest osmotic pressure at 25°C?
Van't Hoff factor (i) for centimolal solution of \[\ce{K3[Fe(CN)6]}\] is 3.333. What is its percentage dissociation?
0.01 m aqueous formic acid solution freezes at – 0.021°C. Calculate its degree of dissociation, Kf = 1.86 K kg mol–1.
For which among the following equimolar aqueous solutions Van't Hoff factor has the lowest value?
Write modification of expressions of colligative properties with the help of van't Hoff factor.
Calculate the van't Hoff factor assuming the complete dissociation of NaBr in its aqueous solution.
Calculate ΔTb and boiling point of 0.05 m aqueous solution of glucose. (Given: Kb = 0.52 K m−1).
The value of van't Hoff factor will be minimum for ______.
The depression in freezing point of 0.2 m aqueous solution of an electrolyte is 0.7 K. Calculate its percent degree of dissociation. [Kf for water = 1.86 K kg mol-1; n = 2]
