Advertisements
Advertisements
Question
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
Solution
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
RELATED QUESTIONS
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 four colligative properties is most often used for molecular mass determination? Why?
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?
Calculate van't Hoff-factor for 0.2 m aqueous solution of KCl which freezes at - 0.680°C. (Kf = 1.86 K kg mol-1).
If the van't Hoff-factor for 0.1 M Ba(NO3)2 solution is 2.74, the degree of dissociation is ______.
Osmotic pressure of a urea solution at 10°C is 500 mm Hg. Osmotic pressure of the solution become 105.3 mm Hg, when it is diluted and temperature is raised to 25°C. The extent of dilution is ____________.
0.6 g of a solute is dissolved in 0.1 L of a solvent which develops an osmotic pressure of 1.23 atm at 27°C. The molecular mass of the solute is ______.
Relationship between van't Hoff's factor (i) and degree of dissociation (α) is ______.
The osmotic pressure of a solution containing 10 g of cane sugar dissolved in 100 mL of water at 70°C is ____________.
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 the following equations is NOT correct for van't Hoff factor?
Which of following 0.1 m aqueous solution exhibits highest osmotic pressure at 25°C?
Solution of 'A' containing 1.73 g of it in 100 cm3 of water is found to be isotonic with a 3.42% (w/v) solution of sucrose. The molecular weight of A is ______. (At. mass C = 12, H = 1, 0 = 16)
Van't Hoff factor (i) for centimolal solution of \[\ce{K3[Fe(CN)6]}\] is 3.333. What is its percentage dissociation?
The equation that represent general van't Hoff equation is ______.
For which among the following equimolar aqueous solutions Van't Hoff factor has the lowest value?
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 ______.
