Ncert Solutions Chemistry Class 11th
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7.85. Does a catalyst influence the values of the equilibrium constant?
7.85. Does a catalyst influence the values of the equilibrium constant?
A catalyst does not affect the equilibrium composition of a reaction mixture. Catalysts influence the rate of both forward and backward reactions equally.
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Questions and Answers:
7.84. Why is the equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the reaction in the forwarding direction?
Questions and Answers:
7.84. Why is the equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the reaction in the forwarding direction?
Equilibrium constant depends upon the way in which the reaction is written.
Upvote MCQs:
7.79 Choose the incorrect statement.
(a) If Brönsted acid is a strong acid then its conjugate base is a weak base and vice versa.
(b) Acids are proton donors and bases are proton acceptors.
(c) higher order ionization constants (Ka2, Ka3) are higher than the lower order ionization constant (Ka1) of a polyprotic acid.
(d) All are correct.
MCQs:
7.79 Choose the incorrect statement.
(a) If Brönsted acid is a strong acid then its conjugate base is a weak base and vice versa.
(b) Acids are proton donors and bases are proton acceptors.
(c) higher order ionization constants (Ka2, Ka3) are higher than the lower order ionization constant (Ka1) of a polyprotic acid.
(d) All are correct.
5.10. 34.05 mL of phosphorus vapour weighs 0.0625 g at 546°C and 1.0 bar pressure. What is the molar mass of phosphorus?
5.10. 34.05 mL of phosphorus vapour weighs 0.0625 g at 546°C and 1.0 bar pressure. What is the molar mass of phosphorus?
7.78. Assertion: Salt does not dissolve in non-polar solvent.
Reason: For non-polar solvent, solvation enthalpy is small and not sufficient to overcome lattice enthalpy of the salt.
7.78. Assertion: Salt does not dissolve in non-polar solvent.
Reason: For non-polar solvent, solvation enthalpy is small and not sufficient to overcome lattice enthalpy of the salt.
(a) In case of a non-polar (covalent) solvent, solvation enthalpy is small and hence, not sufficient to overcome lattice enthalpy of the salt. Consequently, the salt does not dissolve in non-polar solvent. As a general rule, for a salt to be able to dissolve in a particular solvent its solvation en
Upvote 7.77. Assertion: Higher order ionization constants (Ka2, Ka3) are higher than the lower order ionization constant (Ka1) of a polyprotic acid.
Reason: It is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces.
7.77. Assertion: Higher order ionization constants (Ka2, Ka3) are higher than the lower order ionization constant (Ka1) of a polyprotic acid.
Reason: It is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces.
(d) Higher order ionization constants (Ka2, Ka3) are smaller than the lower order ionization constant (Ka1) of a polyprotic acid. The reason for this is that it is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces. This can be seen in the case of r
Upvote 7.76. Assertion: The pH of NH4Cl solution in water is less than 7.
Reason: Ammonium hydroxide is a weak acid and remains almost unionised in solution.
7.76. Assertion: The pH of NH4Cl solution in water is less than 7.
Reason: Ammonium hydroxide is a weak acid and remains almost unionised in solution.
(c) Ammonium hydroxide is a weak base (Kb = 1.77 * 10–5) and not a weak acid. Therefore, it remains almost unionised in solution. This results in increased of H+ ion concentration in solution making the solution acidic. Thus, the pH ofNH4Cl solution in water is less than 7.
Upvote 7.75. Assertion: The solutions of salts formed from strong acids and bases are neutral.
Reason: The cations (e.g., Na+, K+, Ca2+, Ba2+, etc.) of strong bases and anions (e.g., Cl–, Br–, NO3–, ClO4– etc.) of strong acids simply get hydrated but do not hydrolyse.
7.75. Assertion: The solutions of salts formed from strong acids and bases are neutral.
Reason: The cations (e.g., Na+, K+, Ca2+, Ba2+, etc.) of strong bases and anions (e.g., Cl–, Br–, NO3–, ClO4– etc.) of strong acids simply get hydrated but do not hydrolyse.
(a) The cations (e.g., Na+, K+, Ca2+, Ba2+, etc.) of strong bases and anions (e.g., Cl–, Br–, NO3–, ClO4– etc.) of strong acids simply get hydrated but do not hydrolyse, and therefore the solutions of salts formed from strong acids and bases are neutral i.e., their pH is 7. However, the other categ
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