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 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.
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 ____________.
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 ______.
The osmotic pressure of a solution containing 10 g of cane sugar dissolved in 100 mL of water at 70°C is ____________.
If van't Hoff factor of monofluoroacetic acid in water is 1.076. What is it's degree of dissociation?
Which of the following salts of same concentration will have same value of van't Hoff factor as that of K4[Fe(CN)6]?
Which of the following equation is correct to determine osmotic pressure using van't Hoff equation?
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?
0.01 m aqueous formic acid solution freezes at – 0.021°C. Calculate its degree of dissociation, Kf = 1.86 K kg mol–1.
The equation that represent general van't Hoff equation is ______.
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 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]
