JEE Questions for Chemistry Equilibrium Quiz 7 - MCQExams.com

Which buffer solution comprising of the following has its pH value greater than 7 ?
  • CH3COOH + CH3COONa
  • HCOOH + HCOOK
  • CH3COONH4
  • NH4 OH + NH4 Cl
The dissociation constant of a substituted benzoic acid at 25°C is 1.0 × 10-4. The pH of 0.01 M solution of its sodium salt is
  • 3
  • 7
  • 8
  • 6
The buffering action of an acidic buffer is maximum when its pH is equal to
  • 5
  • 7
  • 1
  • pKa
Which of the following is not a buffer solution ?
  • 100 mL 0.1 M CH3COOH + 50 mL 0.1 M CH3COONa
  • 100 mL 0.1M CH3COOH + 50 mL 0.1M NaOH
  • 50 mL 0.1 M CH3COOH + 100 mL 0.1 M NaOH
  • 100 mL 0.1 M NH4OH + 50 mL 0.1 M HCl
The pKa of a weak acid, H A, is 4.80. The pKb of a weak base, BOH is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be
  • 9.58
  • 4.79
  • 7.01
  • 9.22
A buffer solution is prepared by mixing equal concentration of acid (ionisation constant Ka) and a salt. The pH of buffer is
  • pKa + 7
  • 14 - pKa
  • pKa
  • pKa + 1
A buffer solution is prepared by mixing 0.1, M ammonia and 1.0 M ammonium chloride. At 298 K, the pKb of NH4OH is 5.0. The pH of the buffer is
  • 10.0
  • 9.0
  • 6.0
  • 8.0
Assertion (A) The aqueous solution of CH3COONa is alkaline in nature.
Reason (R) Acetate ion undergoes anionic hydrolysis.
  • Both A and R are correct and R is the correct explanation of A
  • Both A and R are correct but R is not the correct explanation of A
  • A is correct but R is not correct
  • A is not correct but R is correct
The pKa of a weak acid H A is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid ionised is
  • 4.5
  • 2.5
  • 9.5
  • 7.0
The rapid change of pH near the stoichiometric point of an acid base titration is the basis of indicator detection. pH of the solution is related to the ratio of the concentrations of the conjugate acid (HIn) and base (In- ) forms of the indicator given by the expression

  • Chemistry-Equilibrium-3581.png
  • 2)
    Chemistry-Equilibrium-3582.png

  • Chemistry-Equilibrium-3583.png

  • Chemistry-Equilibrium-3584.png
The hydrolysis of sodium carbonate involves the reaction between
  • sodium ion and water
  • Na+ and OH-
  • CO32- and water
  • CO32- and H+
Which one of the following salts on being dissolved in water gives pH > 7 at 25°C ?
  • KCN
  • KNO3
  • NH4 Cl
  • NH4 CN
Degree of hydrolysis (h ) of a salt of weak acid and a strong base is given by

  • Chemistry-Equilibrium-3586.png
  • 2)
    Chemistry-Equilibrium-3587.png

  • Chemistry-Equilibrium-3588.png
  • None of these
What volume of M/10 NaOH added in 50 mL, M/10 acetic acid solution to get a buffer solution having highest buffer capacity ?
  • 50 mL
  • 25 mL
  • 10 mL
  • 40 mL
Which one of the following salts give an acidic solution in water ?
  • CH3COONa
  • NH4Cl
  • NaCl
  • CH3COONH4
The pH of a buffer solution containing equal molal concentration of a weak base and its chloride (Kb for weak base = 2 × 10-5) is
  • 5
  • 9
  • 4.7
  • 9.3
Which of the following salt does not get hydrolysed in water ?
  • KClO4
  • NH4Cl
  • CH3COONa
  • None of these
In a mixture of acetic acid and sodium acetate the ratio of concentration of the salt to the acid is increased ten times. Then, the pH of the solution
  • increases by one
  • decreases by one
  • decreases ten fold
  • increased ten fold
Consider the following solutions of equal concentrations
A = NH4Cl
B = CH3COONa
C = NH4OH
D = CH3COOH
A buffer solution can be obtained by mixing equal volumes of
  • C and D
  • A and B
  • A and C
  • C and D
A white substance having alkaline nature in solution is
  • NaNO3
  • NH4Cl
  • Na2CO3
  • Fe2O3
A solution FeCl3 in water acts as acidic solution due to
  • hydrolysis of Fe3+
  • acidic impurities
  • dissociation
  • ionisation
0.1 mole of CH3NH2 (Kb = 5 × 10-4) is mixed with 0.08 mole of HCl and diluted to 1L. What will be the H+ concentration in the solution ?
  • 8 × 10-2 M
  • 8 × 10-11 M
  • 1.6 × 10-11 M
  • 8 × 10-5 M
A buffer solution has equal volumes of 0.2 M NH4 OH and 0.02 M NH4Cl. The pKb of the base is 5. The pH is equal to
  • 10
  • 9
  • 4
  • 7
Assertion (A) The pH of a buffer solution containing equal moles of acetic acid and sodium acetate is 4.8 (pKa of acetic acid is 4.8).
Reason (R) The ionic product of water at 25°C is 10-4 mo12 L-2. The correct answer is
  • Both A and R are true and R is the correct explanation of A.
  • Both A and R are true and R is not the correct explanation of As.
  • A is true but R is not true.
  • A is not true but R is true.
The compound whose 0.1 M solutions is basic, is
  • ammonium acetate
  • ammonium chloride
  • ammonium sulphate
  • sodium acetate
Which of the following reactions will be favoured at low pressure?

  • Chemistry-Equilibrium-3590.png
  • 2)
    Chemistry-Equilibrium-3591.png

  • Chemistry-Equilibrium-3592.png

  • Chemistry-Equilibrium-3593.png
For the manufacture of ammonia by Haber’s process, i.e.
Chemistry-Equilibrium-3594.png
  • High temperature, high pressure
  • Low temperature, low pressure
  • High temperature, low pressure
  • Low temperature, high pressure
The equilibrium constant in a reversible chemical reaction at a given temperature
  • depends on the initial concentration of the reactants
  • depends on the concentration of one of the products at equilibrium
  • does not depend on the initial concentrations of reactants
  • is not characteristic of the reaction
Which of the following substances on dissolving in water will give a basic solution?
  • Na2CO3
  • Al2(SO4)3
  • NH4Cl
  • KNO3
A mixture of a weak acid (say acetic acid) and its salt with a strong base (say sodium acetate) is a buffer solution. Which other pair of substances from the following may have a similar property?
  • HCl and NaCl
  • NaOH and NaNO3
  • KOH and KCl
  • NH4OH and NH4Cl
Silver nitrate solution is gradually added to an aqueous solution containing 0.01 M each of chloride, bromide and iodide ions. The correct sequence in which the halides will be precipitated is
  • Br–, Cl–, I–
  • I–, Cl–, Br–
  • I–, Br–, Cl–
  • Br–, I–, Cl–
Which one of the following is NOT a buffer solution?
  • 0.8 MH2S + 0.8 M KHS
  • 2)
    Chemistry-Equilibrium-3596.png
  • 3 M H2CO3 + 3 M KHCO3
  • 0.05 MKClO4 + 0.05 MHClO4
A certain buffer solution contains equal concentrations of X− and HX. Kb for X− is 10-10. The pH of the buffer solution is
  • 4
  • 10
  • 7
  • 14
The solubility product of a sparingly soluble salt AB at room temperature is 1.21 × 10–6 M2. Its molar solubility is
  • 1.21 × 10–6
  • 1.1 × 10–4
  • 1.1 × 10–3
  • None of these
The solubility in water of a sparingly soluble salt, AB2 is 1.0 × 10–5 mol L–1. Its solubility product number will be
  • 4 × 10–10
  • 1 × 10–15
  • 1 × 10–10
  • 4 × 10–15
A certain weak acid has a dissociation constant of 1.0 × 10–4. The equilibrium constant for its reaction with a strong base is
  • 1.0 × 10–4
  • 1.0 × 10–10
  • 1.0 × 1010
  • 1.0 × 1014
If Ka1 and Ka2 acid are 1 × 10-2 and 1 × 10-6 respectively, then concentration of sulphate ions in 0.01 MH2SO4 solution will be
  • 1 × 10-2
  • 0.01 × 10-8
  • 1 × 10-6
  • 0.01 × 10-10
For the solution of a weak electrolyte AB2, the degree of dissociation is given by

  • Chemistry-Equilibrium-3602.png
  • 2)
    Chemistry-Equilibrium-3603.png

  • Chemistry-Equilibrium-3604.png

  • Chemistry-Equilibrium-3605.png

Chemistry-Equilibrium-3607.png

  • Chemistry-Equilibrium-3608.png
  • 2)
    Chemistry-Equilibrium-3609.png

  • Chemistry-Equilibrium-3610.png

  • Chemistry-Equilibrium-3611.png

Chemistry-Equilibrium-3613.png

  • Chemistry-Equilibrium-3614.png
  • 2)
    Chemistry-Equilibrium-3615.png

  • Chemistry-Equilibrium-3616.png
  • difficult to compute

Chemistry-Equilibrium-3617.png
  • 1 ∶ 36
  • 1 ∶ 1
  • 1 ∶ 3
  • 1 ∶ 9
The PKa of a weak acid HA is 4.80 The pKb of a weak base BOH is 4.78 The PH of an aqueous solution of the corrosponding salt BA will be
  • 9.58
  • 4.79
  • 7.01
  • 9.22
A vessel contains CO2 at 1000k temperature with a pressure 0.5 atm.some of CO2 is converted in to CO on addition of graphite. If total pressure at equilibrium is 0.8 atm the value of KP is:
  • 3 atm
  • 0.3 atm
  • 0.18 atm
  • 1.8 atm
Water is a
  • Protophobic solvent
  • Protophilic solvent
  • Amphiprotic solvent
  • Aprotic acid
Ammonium ion is
  • Conjugate acid
  • Conjugate base
  • Neither an acidnor a base
  • both an acid and a base.
Species acting both as bronsted acid and a base is

  • Chemistry-Equilibrium-3622.png
  • Na2CO3
  • NH3
  • OH-
What is the conjugate base of OH- ?
  • O2
  • H2O
  • O-
  • O2-
An example for lewis acid is
  • Ammonia
  • Aluminium chloride
  • Pyridine
  • Amines
In a given system, water and ice are in equilibrium. If pressure is applied to the above system, then,
  • More ice is formed
  • Amount of ice and water will remain same
  • More ice is melted
  • Either (or (3)
In 2HI ⇌ H2 + I2 ΔH > 0 the forward reaction is affected by change in
  • Catalyst
  • Pressure
  • Volume
  • Temp
0:0:1


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