List of top Chemistry Questions on Types of Solutions

Why saline water is mixed with medicine before injected into the blood of a patient?
200 cm3 of an aqueous solution of a protein contains 1.26 g of the protein. The osmotic pressure of this solution at 300 K is found to be 2.57 × 10^-3 bar. Calculate the molar mass of the protein.

Given: R = 0.083 L bar mol^-1 K^-1
Which of the following gases is most soluble in water?
What is the molarity of a solution that contains 0.5 mol of NaCl in 250 mL of solution?
Which among the following purification methods is based on the principle of “Solubility” in two different solvents?
Fehling’s solution ‘A’ is
Match List I with List II
LIST ILIST II
ACobalt catalyst1(H2​+Cl2​) production
BSyngas2Water gas production
CNickel catalyst3Coal gasification
DBrine solution4Methanol production
Choose the correct answer from the options given below:
Match List I with List II
LIST ILIST II
A Cobalt catalystI \((H_2​+Cl_2​)\) production
B SyngasIIWater gas production
C Nickel catalystIII  Coal gasification
DBrine solutionIV  Methanol production
Choose the correct answer from the options given below:

A solution of Fe2(SO4)3 is electrolyzed for ‘x’ min with a current of 1.5 A to deposit 0.3482 g of Fe. The value of x is _______. [nearest integer]

Given : 1 F = 96500 C mol–1. 

Atomic mass of Fe = 56 g mol–1

Raoult’s law becomes a special case of Henry’s law when
The normality of 26% (wt/vol) solution of ammonia (density =0.855) is approximately:
1.25 g of a sample of Na₂CO₃ and Na₂SO₄ is dissolved in 250mL solution. 25mL of this solution neutralizes 20mL of 0.1NH₂SO₄. The percentage of Na₂CO₃ in the sample is:

Chloroform, CHCl₃, boils at 61.7°C. If Kb for chloroform is 3.63°C/molal, what is the boiling point of a solution of 15.0 g of CHCl₃ and 0.616 kg of acenaphthalene (C₁₂H₁₀)?

The pH of a 0.1M monobasic acid is found to be 2. Hence, its osmotic pressure at a given temperature T is:
Raoult’s law becomes a special case of Henry’s law when
A 1.25g sample of a mixture of Na₂CO₃ and Na₂SO₄ is dissolved in 250mL solution. 25mL of this solution neutralises 20mL of 0.1NH₂SO₄. The % of Na₂CO₃ in the sample is:
The normality of 26% (w/v) solution of ammonia (density =0.855) is approximately:
Volume of 3%solution of sodium carbonate necessary to neutralise a litre of 0.1 N sulphuric acid is
Volume of 3%solution of sodium carbonate necessary to neutralise a litre of 0.1 N sulphuric acid is
Equal weights of NaCl and KCl are dissolved separately in equal volumes of solutions. Molarity of the two solutions will be:
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0 M \( \text{HNO}_3 \)? The concentrated acid is 70% \( \text{HNO}_3 \).
0.45 g of acid molecular weight 90 is neutralized by 20 mL of 0.5N caustic potash. The basicity of the acid is:
The van’t Hoff factor i for an electrolyte which undergoes dissociation and association in solvents are respectively:
If the elevation in boiling point of a solution of 10 g of solute (mol. wt. = 100) in 100 g of water is \( \Delta T_b \), the ebullioscopic constant of water is:
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 Kf of benzene is 5.12 K kg mol^-1, the freezing point of benzene will be lowered by: