Tamil Nadu Board Samacheer Kalvi solutions for Class 11th Chemistry Volume 1 and 2 Answers Guide chapter 9 - Solutions [Latest edition]

The molality of a solution containing 1.8 g of glucose dissolved in 250 g of water is

Which of the following concentration terms is/are independent of temperature

Stomach acid, a dilute solution of HCl can be neutralized by reaction with aluminium hydroxide \[\ce{Al(OH)3 + 3HCl (aq) -> AlCl3 + 3H2O}\]

How many milliliters of 0.1 M Al(OH)₃ solution is needed to neutralize 21 ml of 0.1 M HCl?

The partial pressure of nitrogen in air is 0.76 atm and its Henry’s law constant is 7.6 × 10⁴ atm at 300 K. What is the mole fraction of nitrogen gas in the solution obtained when air is bubbled through water at 300 K?

Henry’s law constant for the solubility of Nitrogen gas in water at 350 K is 8 × 10⁴ atm. The mole fraction of nitrogen in air is 0.5. The number of moles of Nitrogen from air dissolved in 10 moles of water at 350 K and 4 atm pressure is

Which one of the following is incorrect for an ideal solution?

Which one of the following gases has the lowest value of Henry’s law constant?

P₁ and P₂ are the vapour pressures of pure liquid components, 1 and 2 respectively of an ideal binary solution If x₁ represents the mole fraction of component 1, the total pressure of the solution formed by 1 and 2 will be

Osomotic pressure (π) of a solution is given by the relation

Which one of the following binary liquid mixtures exhibits positive deviation from Raoults law?

The Henry’s law constants for two gases A and B are x and y respectively. The ratio of mole fractions of A to B 0.2. The ratio of mole fraction of B and A dissolved in water will be

At 100°C the vapour pressure of a solution containing 6.5 g a solute in 100 g water is 732 mm. If K_b = 0.52, the boiling point of this solution will be:

According to Raoults law, the relative lowering of vapour pressure for a solution is equal to ______.

At same temperature, which pair of the following solutions are isotonic?

The empirical formula of a nonelectrolyte(X) is CH2 O. A solution containing six gram of X exerts the same osmotic pressure as that of 0.025M glucose solution at the same temperature. The molecular formula of X is

The K_H for the solution of oxygen dissolved in water is 4 × 10⁴ atm at a given temperature. If the partial pressure of oxygen in air is 0.4 atm, the mole fraction of oxygen in solution is ______.

Normality of 1.25M sulphuric acid is ______.

Two liquids X and Y on mixing gives a warm solution. The solution is ______.

The relative lowering of vapour pressure of a sugar solution in water is 2.5 × 10^-3. The mole fraction of water in that solution is ______.

The mass of a non – volatile solute (molar mass 80 g mol^-1) should be dissolved in 92g of toluene to reduce its vapour pressure to 90% ______.

For a solution, the plot of osmotic pressure (π) versus the concentration (c in mol L^-1) gives a straight line with slope 310 R where ‘R’ is the gas constant. The temperature at which osmotic pressure measured is ______.

200 ml of an aqueous solution of a protein contains 1.26 g of protein. At 300 K, the osmotic pressure of this solution is found to be 2.52 × 10^-3 bar. The molar mass of protein will be (R = 0.083 L bar mol^-1 K^-1)

The Van't Hoff factor (i) for a dilute aqueous solution of the strong elecrolyte barium hydroxide is (NEET) ______.

Which is the molality of a 10% w/w aqueous sodium hydroxide solution?

The correct equation for the degree of an associating solute, ‘n’ molecules of which undergoes association in solution, is

Which of the following aqueous solutions has the highest boiling point?

The freezing point depression constant for water is 1.86° K Kg mol^-1. If 5 g Na₂SO₄ is dissolved in 45 g water, the depression in freezing point is 3.64°C. The Vant Hoff factor for Na₂SO₄ is ______.

Equimolal aqueous solutions of NaCl and KCl are prepared, If the freezing point of NaCl is -2°C, the freezing point of KCl solution is expected to be ______.

Phenol dimerizes in benzene having van’t Hoff factor 0.54. What is the degree of association?

Assertion: An ideal solution obeys Raoults Law.

Reason: In an ideal solution, solvent – solvent as well as solute – solute interactions are similar to solute-solvent interactions.

Define molality.

Define Normality.

What is a vapour pressure of liquid?

What is a relative lowering of vapour pressure?

State and explain Henry’s law.

State Raoult law and obtain the expression for lowering of vapour pressure when the nonvolatile solute is dissolved Insolvent.

What is molal depression constant? Does it depend on nature of the solute?

What is osmosis?

Define isotonic solutions

You are provided with a solid ‘A’ and three solutions of A dissolved in water – one saturated, one unsaturated, and one super saturated. How would you determine each solution?

Explain the effect of pressure on solubility.

A sample of 12 M Concentrated hydrochloric acid has a density 1.2 M gL^-1 calculate the molality.

A 0.25 M glucose solution, at 370.28 K has approximately the pressure as blood does what is the osmotic pressure of blood?

Calculate the molality of a solution containing 7.5 g glycine(NH₂-CH₂-COOH) dissolved in 500g of water.

Which solution has the lower freezing point? 10 g of methanol (CH₃OH) in 100g g of water (or) 20 g of ethanol (C₂H₅OH) in 200 g of water.

How many moles of solute particles are present in one liter of 10^-4 M potassium sulphate?

Henry’s law constant for solubility of methane in benzene is 4.2 × 10^-5 mm Hg at a particular constant temperature. At this temperature calculate the solubility of methane at

1. 750 mm Hg
2. 840 mm Hg.

The observed depression in the freezing point of water for a particular solution is 0.093°C calculate the concentration of the solution in molality. Given that molal depression constant for water is 1.86 K Kg mol^-1.

The vapour pressure of pure benzene (C₆H₆) at a given temperature is 640 mm Hg. 2.2 g of non – volatile solute is added to 40 g of benzene. The vapour pressure of the solution is 600 mm Hg. Calculate the molar mass of the solute?