Henry`s law is not applicable for the aqueous solution of.......

(A) O2 

(B) N2

(C) SO3

(D) He

Answer (C) 

Explanation: Henry`s law is not applicable for the aqueous solution of those gas which undergoes  chemical reactions with solvent (water).

Here SO3 react with water to form sulphuric acid.

Henry`s law constant of CO2 in water at 298K is 5/3 k bar. If pressure of CO2 is 0.01 bar, then find its mole fraction.

Van’t Hoff Factor

In 1886, Van’t Hoff introduced a factor 'i' called Van’t Hoff factor to express the extent of association

or dissociation of solute in solution.

Related Questions;

(1) calculate weight of urea which must be dissolved in 400 gm of water so that final has V.P. 2% than V.P. of pure water?

(2) 10 gm of a solute is dissolved in 80 gm of acetone V.P. of solution is 271 mm Hg. If V.P. of pure acetone is 283 mm of Hg. calculate molar mass of solute.

(3) Vapour pressure of a solution containing 6 gm of non volatile solute in 180 gm of water is 20 torr/mmHg. If 1 mole of water is further added in to the V.P. increases by 0.02 torr. calculate the V.P. of pure water and molecular wt of the non volatile solute.

(4) An aqueous solution has 5% urea and 10% glucose by weight. what will be the freezing point of this solution ? ( Kf = 1.86 K Kg per mole)

(5) Acetic acid dimerised to an extent of 30% in benzene . The observed molecular mass (in gm) is...

(6) How much ice will separate if a solution containing 25 g of ethylene glycol [C2H4(OH) 2] in 100g of water is cooled to 10°C? Kf(H2O) = 1.86 (25.05 g)

(7) The dielectric con stant of H2O is 80. The electrostatic force of attraction between Na+ and Cl–will be.

(8) The van't Hoff's factor for 0.1 M Ba(NO3)2 solution is 2.74. the degree of dissociation is.

(9) An aqueous solution has 5% urea and 10% glucose by weight. what will be the freezing point of this solution ? ( Kf = 1.86 K Kg per mole)

(10) Acetic acid dimerised to an extent of 30% in benzene . The observed molecular mass (in gm) is...

(11) How much ice will separate if a solution containing 25 g of ethylene glycol [C2H4(OH) 2] in 100g of water is cooled to 10°C? Kf(H2O) = 1.86 (25.05 g)

(12) The dielectric con stant of H2O is 80. The electrostatic force of attraction between Na+ and Cl–will be.

(13) The van't Hoff's factor for 0.1 M Ba(NO3)2 solution is 2.74. the degree of dissociation is.

(14) How can derivatives relation between relative lovering of vapour pressure and molality?

(15) A saturared solution of XCl3 has a vapour pressure 17.20 mm Hg at 20°C, while pure water vapour pressure is 17.25 mm Hg. Solubility product (Ksp) of XCl3 at 20°C is

(16) Calculate the percentage degree of dissociation of an electrolyte XY2 ( normal molar mass=165) in water if the observed molar mass by measuring elevation in boiling point is 65.5.

(17) Which of the following pair of solution (aq.) contain isotonic solution at same temperature? (Assume 100 % ionisation of electrolytes) 

(1) 0.1 M NaCI and 0.2 M CaCI2

(2) 0.1 M NaCI and 0.3 M AICI3 

(3) 0.3 M NaCI and 0.1 M AICI3 

(4) 0.3 M NaCI and 0.2 CaCI2

(18) Freezing point of pure liquid A is T K. If some amount of non-electrolyte non-volatile impurity is added in A, an ideal solution is formed. On cooling at 200 K, only 30% (by mass) liquid A is present and at 201 K, 60 % (by mass) liquid A is present. The value of T is .

(19) Liquid A and B form ideal solution at temperature T. Mole fraction of A in liquid and vapour phase are 0.4 and 4/13 respectively, when total pressure is 130 torr. The vapour pressure (in torr) of A and B in pure state at temperature T are respectively.

(20) 2 millimolar solution of sodium ferrocyanide is 60% dissociated at 27°C. osmotic pressure of the slotution is .

(21) Decimolar solution of K4[Fe(CN)6] dissociate by 60% at 27°C. Determine osmotlc pressure in Nature/M2.

(22) A complex is represented as CoCl3.xNH3.Freezing point of its 0.1 molar solution is - 0.558° C (Kf = 18.6) Assuming 100 % dissociation and coordination number of Co(iii) is six , the what is the complex formula ?

(23) A complex is wrltten as M(en)y.xBr. lts 0.05 molar solution shows 2.46 atm osmotlc pressure at 27°C. Assuming 100 % ionisaton and coordination number of metal (iii) is six, complex may be:

(24) Find the freezing point of a solution when 5 moI of Kl is mixed with 1 moI of HgCI2 in 3500 g of H20. Kf of H20 1.86 K/m. (KI + HgCI2 --> K2Hgl4 + KCI)

(25) A mixture of weighing 228 g contain CaCl2 and NaCl . If this mixture is dissolved in 10 kg of water and form ideal solution that boil at 100.364 ℃ The mol % of NaCl in mixture is [ kb of water = 0.52 K per mol Kg]

(26) What is the Raoult's law and it's application ?

(27) What is Vapour pressure of liquid ?

(28) The van't Hoff's factor for 0.1 M Ba(NO3)2 solution is 2.74. the degree of dissociation is.

(29) Aqueous solution of 0.004 M Na2SO4 and 0.01 M glucose are iosotonic .The degree of dissociation of Na2SO4 is ..

(30) A saturared solution of XCl3 has a vapour pressure 17.20 mm Hg at 20°C, while pure water vapour pressure is 17.25 mm Hg. Solubility product (Ksp) of XCl3 at 20°C is.

Colligative Properties

These are the properties that depend on the concentration of solute molecule or ions in solution but not on the chemical identity of the solute. 

For example, addition of ethylene glycol to water lowers the freezing point of water below 0°C. 

The magnitude of freezing point lowering is directly proportional to the number of solute molecules added to a particular quantity of solvent. 

(1) If 0.01 mole of ethylene glycol is added to 1 kg of water, the freezing point is lowered to - 0.019°C while

(2)  On adding 0.020 mole of ethylene glycol to 1 kg of water, the freezing point is lowered to -0.038°C. 

The various colligative properties are 

(1) Relative lowering of vapour pressure 

(2) Osmotic pressure 

(3) Elevation of boiling point 

(4) Depression of freezing point 

Henry's law constant for CO2​ in water is 1.67×10^8 Pa at 298K. Calculate the quantity of CO2​ in 500 ml of soda water when packed under 2.5 atm CO2​ pressure at 298K.

If N2 gas is bubbled through water at 293 K, how many millimoles of N2 gas would dissolve in 1 litre of water. Assume that N­2 exerts a partial pressure of 0.987 bar. Given that Henry’s law constant for N2 at 293 K is 76.84 kbar.

The solubility of gas is related to its mole fraction in the aqueous solution. The mole fraction of the gas in the solution is calculated by applying Henry’s law. Thus,

As 1litre water contains 55.5 mol of it, therefore, if n represents number of moles of N₂ in solution,

Related Questions:

(1) The vapour pressure of ethanol and methanol are 44.5 mm and 88.7 mm Hg respectively. An ideal solution is formed at the same temperature by mixing 60 g of ethanol with 40g of methanol. Calculate total vapour pressure of the solution.

(2) What is the composition of the vapour which is in equilibrium at 30°C with a benzene-toluene solution with a mole fraction of benzene of 0.400?

Liquid A and B forms an ideal solution and initial vapour pressure of A and B are P°A= 0.4 atm and P°A= 0.6 atm respectively. In a cylinder piston arrangement, 2 mole vapour of A and 3 mole vapour of B is collected at 0.42 atm.

(1) predict wheather the vapour will condense or not ?

(2) If the vapours are  compared slowly and isothermally at what  pressure F drop of liquid will form?

(3) If initial volume of vapour was 10 litre , at what volume first drop of liquid is form?

(4) What is the composition of first drop of liquid formed?

(5) If vapour pressure are further compressed. At what  pressure  almost complete condensation of vapour will occure?

(6) Determine the composition of last traces of vapours remains?

(7) What is the composition of system at 0.55 atm pressure?

(8) Determine the composition of liquid and vapour formed  at 0.51 atm also  calculate the moles of liquid of A and B in liquid and vapour formed ?

(9) At what pressure half of the total amount of vapour will condense?

Related Questions;

(1) calculate weight of urea which must be dissolved in 400 gm of water so that final has V.P. 2% than V.P. of pure water?

(2) 10 gm of a solute is dissolved in 80 

gm of acetone V.P. of solution is 271 mm Hg. If V.P. of pure acetone is 283 mm of Hg. calculate molar mass of solute.

(3) Vapour pressure of a solution containing 6 gm of non volatile solute in 180 gm of water is 20 torr/mmHg. If 1 mole of water is further added in to the V.P. increases by 0.02 torr. calculate the V.P. of pure water and molecular wt of the non volatile solute.

(4) An aqueous solution has 5% urea and 10% glucose by weight. what will be the freezing point of this solution ? ( Kf = 1.86 K Kg per mole)

(5) Acetic acid dimerised to an extent of 30% in benzene . The observed molecular mass (in gm) is...

(6) How much ice will separate if a solution containing 25 g of ethylene glycol [C2H4(OH) 2] in 100g of water is cooled to 10°C? Kf(H2O) = 1.86 (25.05 g)

(7) The dielectric con stant of H2O is 80. The electrostatic force of attraction between Na+ and Cl–will be.

(8) The van't Hoff's factor for 0.1 M Ba(NO3)2 solution is 2.74. the degree of dissociation is.

Vapour pressure of a solution containing 6 gm of non volatile solute in 180 gm of water is 20 torr/mmHg. If 1 mole of water is further added in to the V.P. increases by 0.02 torr. calculate the V.P. of pure water and molecular wt of the non volatile solute.

10 gm of a solute is dissolved in 80 gm of acetone V.P. of solution is 271 mm Hg. If V.P. of pure acetone is 283 mm of Hg. calculate molar mass of solute.

calculate weight of urea which must be dissolved in 400 gm of water so that final has V.P. 2% than V.P. of pure water?

What is relation between relative lowering of vapour pressure and molality of solution?

ILLUSTRATION

(1) calculate weight of urea which must be dissolved in 400 gm of water so that final has V.P. 2% than V.P. of pure water?

(2) 10 gm of a solute is dissolved in 80 

gm of acetone V.P. of solution is 271 mm Hg. If V.P. of pure acetone is 283 mm of Hg. calculate molar mass of solute.

(3) Vapour pressure of a solution containing 6 gm of non volatile solute in 180 gm of water is 20 torr/mmHg. If 1 mole of water is further added in to the V.P. increases by 0.02 torr. calculate the V.P. of pure water and molecular wt of the non volatile solute.

Related Questions;

(1) An aqueous solution has 5% urea and 10% glucose by weight. what will be the freezing point of this solution ? ( Kf = 1.86 K Kg per mole)

(2) Acetic acid dimerised to an extent of 30% in benzene . The observed molecular mass (in gm) is...

(3) How much ice will separate if a solution containing 25 g of ethylene glycol [C2H4(OH) 2] in 100g of water is cooled to 10°C? Kf(H2O) = 1.86 (25.05 g)

(4) The dielectric con stant of H2O is 80. The electrostatic force of attraction between Na+ and Cl–will be.

(5) The van't Hoff's factor for 0.1 M Ba(NO3)2 solution is 2.74. the degree of dissociation is.

200 ml of 0.2M urea solution is mixed with 200 ml of glucose solution at 300 K. Calculate osmotic pressure of resulting solution.

Related Questions;

(1) An aqueous solution has 5% urea and 10% glucose by weight. what will be the freezing point of this solution ? ( Kf = 1.86 K Kg per mole)

(2) Acetic acid dimerised to an extent of 30% in benzene . The observed molecular mass (in gm) is...

(3) How much ice will separate if a solution containing 25 g of ethylene glycol [C2H4(OH) 2] in 100g of water is cooled to 10°C? Kf(H2O) = 1.86 (25.05 g)

(4) The dielectric con stant of H2O is 80. The electrostatic force of attraction between Na+ and Cl–will be.

(5) The van't Hoff's factor for 0.1 M Ba(NO3)2 solution is 2.74. the degree of dissociation is.

(6) Aqueous solution of 0.004 M Na2SO4 and 0.01 M glucose are iosotonic .The degree of dissociation of Na2SO4 is ..

(7) How can derivatives relation between relative lovering of vapour pressure and molality?

(8) A saturared solution of XCl3 has a vapour pressure 17.20 mm Hg at 20°C, while pure water vapour pressure is 17.25 mm Hg. Solubility product (Ksp) of XCl3 at 20°C is

(9) Calculate the percentage degree of dissociation of an electrolyte XY2 ( normal molar mass=165) in water if the observed molar mass by measuring elevation in boiling point is 65.5.

(10) Which of the following pair of solution (aq.) contain isotonic solution at same temperature? (Assume 100 % ionisation of electrolytes) (1) 0.1 M NaCI and 0.2 M CaCI2(2) 0.1 M NaCI and 0.3 M AICI3 (3) 0.3 M NaCI and 0.1 M AICI3 (4) 0.3 M NaCI and 0.2 CaCI2

How to determine total vapour pressure of solution in liquid phase as well as gas phase ?

According to Raoult's Law: The partial pressure of any volatile component of a solution at any temperature is equal to the vapour pressure of the pure component multiplied by the mole fraction of that component in the solution.

      Where X_A­ and X_B is the mole fraction of the component A and B in liquid phase respectively

According to Dalton's Law:

The vapour behaves like an ideal gas, then according to Dalton's law of partial pressures, the total pressure P_Tis given by:

 Partial pressure of the gas = Total pressure x Mole fraction

                                        P_A = P_T Y_A and P_B =P_T Y_B

Where Y_A­ and Y_B is the mole fraction of the component A and B in gas phase respectively

Combination of Raoult's and Dalton's Law:

(3) Thus, in case of ideal solution the vapour phase is phase is richer with more volatile component i.e., the one having relatively greater vapour pressure

Graph Between 1/YA Vs 1/XA:

According to Dalton's law of partial pressures, the total pressure P_T is given by:

 Partial pressure of the gas = Total pressure x Mole fraction

Where Y_A­ and Y_B is the mole fraction of the component A and B in gas phase respectively

According to Raoult's law:

On rearrangement of this equation we get a straight line equation:

Illustrative Examples:

Liquid A and B form ideal solution at temperature T. Mole fraction of A in liquid and vapour phase are 0.4 and 4/13 respectively, when total pressure is 130 torr. The vapour pressure (in torr) of A and B in pure state at temperature T are respectively.

Solubility of gases and Henry's Law:

When a solution containing w of urea in 1kg of water is cooled to 272K, 200g of ice is separated. If for water is 1.86Kkgmol−1,w is:

Related Questions;

(1) An aqueous solution has 5% urea and 10% glucose by weight. what will be the freezing point of this solution ? ( Kf = 1.86 K Kg per mole)

(2) Acetic acid dimerised to an extent of 30% in benzene . The observed molecular mass (in gm) is...

(3) How much ice will separate if a solution containing 25 g of ethylene glycol [C2H4(OH) 2] in 100g of water is cooled to 10°C? Kf(H2O) = 1.86 (25.05 g)

(4) The dielectric con stant of H2O is 80. The electrostatic force of attraction between Na+ and Cl–will be.

(5) The van't Hoff's factor for 0.1 M Ba(NO3)2 solution is 2.74. the degree of dissociation is.

(6) Aqueous solution of 0.004 M Na2SO4 and 0.01 M glucose are iosotonic .The degree of dissociation of Na2SO4 is ..

(7) How can derivatives relation between relative lovering of vapour pressure and molality?

(8) A saturared solution of XCl3 has a vapour pressure 17.20 mm Hg at 20°C, while pure water vapour pressure is 17.25 mm Hg. Solubility product (Ksp) of XCl3 at 20°C is

(9) Calculate the percentage degree of dissociation of an electrolyte XY2 ( normal molar mass=165) in water if the observed molar mass by measuring elevation in boiling point is 65.5.

(10) Which of the following pair of solution (aq.) contain isotonic solution at same temperature? (Assume 100 % ionisation of electrolytes) (1) 0.1 M NaCI and 0.2 M CaCI2(2) 0.1 M NaCI and 0.3 M AICI3 (3) 0.3 M NaCI and 0.1 M AICI3 (4) 0.3 M NaCI and 0.2 CaCI2

What is Azeotropic mixture or solution?

A solution which boils like a pure liquid and has same composition in liquid as well as vapour phase is called Azeotropic solution or mixture.

Features of Azeotropic mixture:

# For Azeotropic solution XA =YA

# An ideal solution can not form Azeotropic mixture.

# only non ideal solution form Azeotropic mixture.

# composition of Azeotrope alter on changing external pressure.

# Azeotropic solution can't separated by fractional distillation.

Type of Azeotropic solution or mixture:

(1) Minimum boiling Azeotropic solution. 

It is formed by solution which show positive (+) deviation from ideal behaviour. Such solution has boiling point smaller than boiling point of both of components liquids.

For example, mixture of 95% ethanol by weight and 4% of water. 

Water boils at 373 K, and ethanol boils at about 351.5K, while azeotropes mixture of both boil at around 351.15 K, suggesting a boiling point lower than its constituents.

(2) Maximum boiling Azeotropic solution.

It is formed by solution which show negative (-) deviation from ideal behaviour. Such solution has boiling point larger than boiling point of both of components liquids.

For example,  mixture of approximately 20% by weight hydrochloric acid and 79 % of water.

Water boils at 373 K and hydrochloric acid boil at about 188 K,  while azeotropes  of both boil at around 383 K which is a boiling point greater than its constituents.

Related Questions;

(1) An aqueous solution has 5% urea and 10% glucose by weight. what will be the freezing point of this solution ? ( Kf = 1.86 K Kg per mole)

(2) Acetic acid dimerised to an extent of 30% in benzene . The observed molecular mass (in gm) is...

(3) How much ice will separate if a solution containing 25 g of ethylene glycol [C2H4(OH) 2] in 100g of water is cooled to 10°C? Kf(H2O) = 1.86 (25.05 g)

(4) The dielectric con stant of H2O is 80. The electrostatic force of attraction between Na+ and Cl–will be.

(5) The van't Hoff's factor for 0.1 M Ba(NO3)2 solution is 2.74. the degree of dissociation is.

(6) Aqueous solution of 0.004 M Na2SO4 and 0.01 M glucose are iosotonic .The degree of dissociation of Na2SO4 is ..

(7) How can derivatives relation between relative lovering of vapour pressure and molality?

(8) A saturared solution of XCl3 has a vapour pressure 17.20 mm Hg at 20°C, while pure water vapour pressure is 17.25 mm Hg. Solubility product (Ksp) of XCl3 at 20°C is

(9) Calculate the percentage degree of dissociation of an electrolyte XY2 ( normal molar mass=165) in water if the observed molar mass by measuring elevation in boiling point is 65.5.

(10) Which of the following pair of solution (aq.) contain isotonic solution at same temperature? (Assume 100 % ionisation of electrolytes) (1) 0.1 M NaCI and 0.2 M CaCI2(2) 0.1 M NaCI and 0.3 M AICI3 (3) 0.3 M NaCI and 0.1 M AICI3 (4) 0.3 M NaCI and 0.2 CaCI2

(11) Freezing point of pure liquid A is T K. If some amount of non-electrolyte non-volatile impurity is added in A, an ideal solution is formed. On cooling at 200 K, only 30% (by mass) liquid A is present and at 201 K, 60 % (by mass) liquid A is present. The value of T is .

(12) Liquid A and B form ideal solution at temperature T. Mole fraction of A in liquid and vapour phase are 0.4 and 4/13 respectively, when total pressure is 130 torr. The vapour pressure (in torr) of A and B in pure state at temperature T are respectively.

(13) 2 millimolar solution of sodium ferrocyanide is 60% dissociated at 27°C. osmotic pressure of the slotution is .

(14) Decimolar solution of K4[Fe(CN)6] dissociate by 60% at 27°C. Determine osmotlc pressure in Nature/M2.

(15) A complex is represented as CoCl3.xNH3.Freezing point of its 0.1 molar solution is - 0.558° C (Kf = 18.6) Assuming 100 % dissociation and coordination number of Co(iii) is six , the what is the complex formula ?

(16) A complex is wrltten as M(en)y.xBr. lts 0.05 molar solution shows 2.46 atm osmotlc pressure at 27°C. Assuming 100 % ionisaton and coordination number of metal (iii) is six, complex may be:

(17) Find the freezing point of a solution when 5 moI of Kl is mixed with 1 moI of HgCI2 in 3500 g of H20. Kf of H20 1.86 K/m. (KI + HgCI2 --> K2Hgl4 + KCI)

(18) A mixture of weighing 228 g contain CaCl2 and NaCl . If this mixture is dissolved in 10 kg of water and form ideal solution that boil at 100.364 ℃ The mol % of NaCl in mixture is [ kb of water = 0.52 K per mol Kg]

(19) What is the Raoult's law and it's application ?

(20) What is Vapour pressure of liquid ?

What is " Clasius Claperon" equation ?

The dependence of vapour pressure and temperature is given by CLASIUS CLAPERON equation.

Vapour pressure of a particular liquid system is only the function of temperature only. It is independent from all other 

What is "Anoxia" conditions ?

At high altitudes the partial pressure of oxygen is less than that at the ground level. This leads to low concentrations of oxygen in the blood and tissues of people living at high altitudes or climbers. Low blood oxygen causes climbers to become weak and unable to think clearly, symptoms of a condition known as anoxia.

What is bends condition and what is relation of bends with Scuba divers ?

Scuba divers must cope with high concentrations of dissolved gases while breathing air at high pressure underwater. Increased pressure increases the solubility of atmospheric gases in blood. When the divers come towards surface, the pressure gradually decreases. This releases the dissolved gases and leads to the formation of bubbles of nitrogen in the blood. This blocks capillaries and creates a medical condition known as bends, which are painful and dangerous to life.

 To avoid bends, as well as, the toxic effects of high concentrations of nitrogen in the blood, the tanks used by scuba divers are filled with air diluted with helium (11.7% helium, 56.2% nitrogen and 32.1% oxygen).

What is effect of temperature on vapour pressure ? Explain with CLASIUS CLAPERON equation.

Factors affecting vapour pressure:

(A) Temperature:.

(1) The temperature at which the vapour pressure of the liquid becomes equal to the atmospheric pressure is called its boiling point.

(2) Vapour pressure is directly proportional to theTemperature so that on increasing temperature the rate of evaporation increases and rate of condensation decreases and hence vapour pressure increases.

(3) The dependence of vapour pressure and temperature is given by CLASIUS CLAPERON equation.

(4) Vapour pressure of a particular liquid system is only the function of temperature only. It is independent from all other