Equilibrium
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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.
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
Upvote Assertion and Reason:
Directions:
(a) Assertion and reason both are correct statements and reason is correct explanation for assertion.
(b) Assertion and reason both are correct statements but reason is not correct explanation for assertion.
(c) Assertion is correct statement but reason is wrong statement.
(d) Assertion is wrong statement but reason is correct statement.
7.74. Assertion: OH– is called the conjugate base of an acid H2O.
Reason: NH4+ is called conjugate acid of the base NH3.
Assertion and Reason:
Directions:
(a) Assertion and reason both are correct statements and reason is correct explanation for assertion.
(b) Assertion and reason both are correct statements but reason is not correct explanation for assertion.
(c) Assertion is correct statement but reason is wrong statement.
(d) Assertion is wrong statement but reason is correct statement.
7.74. Assertion: OH– is called the conjugate base of an acid H2O.
Reason: NH4+ is called conjugate acid of the base NH3.
(b) Both are correct statements but R is not the reason for A. The acid-base pair that differs only by one proton is called a conjugate acid-base pair. Therefore, OH– is called the conjugate base of an acid H2O and NH4+ is called conjugate acid of the base NH3. If Brönsted acid is a strong acid the
Upvote 7.73 The concentration of sulphide ion in 0.1M HCl solution saturated with hydrogen sulphide is 1.0 × 10–19 M. If 10 mL of this is added to 5 mL of 0.04 M solution of the following: FeSO4, MnCl2, ZnCl2 and CdCl2. in which of these solutions precipitation will take place?
7.73 The concentration of sulphide ion in 0.1M HCl solution saturated with hydrogen sulphide is 1.0 × 10–19 M. If 10 mL of this is added to 5 mL of 0.04 M solution of the following: FeSO4, MnCl2, ZnCl2 and CdCl2. in which of these solutions precipitation will take place?
For precipitation to take place, it is required that the calculated ionic product exceeds the Ksp value. So, following data on Ksp values should have been provided to answer the question.
KspforFeS=6.3×10−18,
MnS=2.5×10−13,
ZnS=1.6×10−24
CdS=8.0×10−27
Before mixing:
[S2−]=1.0×10−19M and [M2+]=0.04M&nbs
Upvote 7.72 What is the minimum volume of water required to dissolve 1g of calcium sulphate at 298 K? (For calcium sulphate, Ksp is 9.1 x 10−6).
7.72 What is the minimum volume of water required to dissolve 1g of calcium sulphate at 298 K? (For calcium sulphate, Ksp is 9.1 x 10−6).
CaSO4 (s)↔Ca2+ (aq)+SO2−4 (aq)
Ksp= [Ca2+] [ SO2−4]
Let the solubility of CaSO4 be s.
[Ca2+] = [ SO2−4] = s
Then, Ksp=s2
9.1×10−6=s2
s =3.02×10−3mol/L
Molecular mass of CaSO4=136g/mol
Solubility of CaSO4 in gram/L= 3.02×10−3×136=0.41g/L
This means that we need 1L of water to dissolve 0.41g of CaSO4.
Therefor
Upvote 7.71. What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide?
(For iron sulphide, Ksp=6.3 x 10−18)
7.71. What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide?
(For iron sulphide, Ksp=6.3 x 10−18)
Let the maximum concentration of each solution be x mol/L. After mixing, the volume of the concentrations of each solution will be reduced to half i.e., x/2.
∴ [FeSO4]= [Na2S]=x / 2
Then, [Fe2+]= [FeSO4]=x/ 2
Also, [S2−]= [Na2S]=x/2
FeS (x)↔Fe2+ (aq)+S2− (aq)
Ksp= [Fe2+] [S2−]
= >6.3×10−18= (x/2) (x/2)
x2/
Upvote