JEE Questions for Chemistry Equilibrium Quiz 6 - MCQExams.com

For a concentrated solution of a weak electrolyte AxBy of concentration C, the degree of dissociation ' α ' is given as

  • Chemistry-Equilibrium-3558.png
  • 2)
    Chemistry-Equilibrium-3559.png

  • Chemistry-Equilibrium-3560.png

  • Chemistry-Equilibrium-3561.png

  • Chemistry-Equilibrium-3562.png
Conjugate acid of HF2- is
  • H+
  • HF
  • F2-
  • H2F2
The first and second dissociation constants of an acid H2 A are 1. 0 × 10-5 and 5. 0 × 10-10, respectively. The overall dissociation constant of the acid will be
  • 5.0 × 10-5
  • 5.0 × 1015
  • 5.0 × 10-15
  • 0.2 × 105
Conjugate base of H2PO4- is
  • H3PO4
  • P2O5
  • PO43-
  • HPO42-
According to Bronsted and Lowry , the strength of an acid depends upon
  • the tendency to gain electrons
  • the tendency to loss protons
  • the tendency to accept protons
  • the tendency to loss electrons
The ionisation of strong electrolytes in acetic acid, compared to water, is
  • weak, low
  • strong, more
  • medium, the same
  • no ionisation, 100%
An acid solution of 0.005 M has a pH of 5. The degree of ionization of acid is
  • 0.1 × 10-2
  • 0.2 × 10-2
  • 0.5 × 10-4
  • 0.6 × 10-6
CH3COOH is weaker acid than H2SO4. It is due to
  • more ionisation
  • less ionisation
  • covalent bond
  • electrovalent bond
A monoprotic acid in 1.00 M solution is 0.01% ionised. The dissociation constant of this acid is
  • 1 × 10-8
  • 1 × 10-4
  • 1 × 10-6
  • 1 × 10-5
What is the conjugate base of OH-
  • O2-
  • O-
  • H2O
  • O2
pH value of which one of the following is not equal to one ?
  • 0.1 M HNO3
  • 0.05 M H2SO4
  • 0.1M CH3 COOH
  • 50 cm3 of 0.4 M HCl + 50 cm3 of 0.2 M NaOH
When 200 mL of aqueous solution of HC1 (pH =is mixed with 300 mL of an aqueous solution of NaOH (pH =the pH of the resulting mixture is
  • 10
  • 2.7
  • 4.0
  • 11.3
  • 2
Which of the following solutions will have pH = 9 at 298 K ?
  • 1 × 10-9 M HCl solution
  • 1 × 10-5 M NaOH solution
  • 1 × 10-9 M KOH solution
  • Both (and (2)
Hydroxyl ion concentration of 10-2 M HCl is
  • 1× 101 mol dm-3
  • 1× 10-12 mol dm-3
  • 1× 10-1 mol dm-3
  • 1× 10-14 mol dm-3
Hydrogen ion concentration in mol/L in a solution of pH= 5.4 will be
  • 3.98 × 10-6
  • 3.68 × 10-6
  • 3.88 × 106
  • 3.98 × 108
If the ionic product of Ni (OH)2 is 1.9 x 10-15, then the molar solubility of Ni (OH)2 in 1.0 M NaOH is
  • 1.9 × 10-18 M
  • 1.9 × 10-13 M
  • 1.9 × 10-15 M
  • 1.9 × 10-14 M
The KSP of Ag2CrO4 is 1.1 × 10-12 at 298 K. The solubility (in mol/L) of Ag2CrO4 in a 0.1 M AgNO3 solution is
  • 1.1 × 10-11
  • 1.1 × 10-10
  • 1.1 × 10-12
  • 1.1 × 10-9
If the solubility of PbBr2 in water is s mol/L, then what is its KSP considering 80% ionisation?
  • 2.048 S2
  • 2.048 S3
  • 1.042 S3
  • 3.042 S2
Passing H2S gas into a mixture of Mn2+, Ni2+, Cu2+ and Hg2+ ions in an acidified aqueous solution precipitates
  • CuS and HgS
  • MnS and CuS
  • MnS and NiS
  • Nis and HgS
In 1L saturated solution of AgCl [KSP(AgCl) = 1.6 × 10-10], 0.1 mole of CuCl [KSP (CuCl) = 1.0 × 10-6] is added. The resultant concentration of Ag+ in the solution is 1.6 x 10-x. The value of x is
  • 3
  • 5
  • 7
  • 9
The KSP for Cr (OH)3 is 1.6 × 10-30. The molar solubility of this compound in water is

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  • 2)
    Chemistry-Equilibrium-3567.png

  • Chemistry-Equilibrium-3568.png

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Chemistry-Equilibrium-3570.png
  • AgCl and PbCrO4
  • AgI and Ag2 CO3
  • AgCl and Ag2CO3
  • Ag2CO3 and AgI
  • Ag2CO3 and PbCrO4
Solubility product of silver bromide is 5.0 ×10-13. The quantity of potassium bromide (molar mass taken as 120 g mol-1) to be added to 1 L of 0.05 M solution of silver nitrate to start the precipitation of AgBr is
  • 1.2 × 10-10 g
  • 1.2 × 10-9 g
  • 6.2 × 10-5 g
  • 5.0 × 10-8 g
At 25oC, the solubility product of Mg (OH)2 is 1.0 × 10-11. At which pH, will Mg2+ ions start precipitating in the form of Mg (OH)2 from a solution of 0. 001M Mg2+ ions ?
  • 9
  • 10
  • 11
  • 8
The solubility of AgCl in 0. 2M NaCl solution is
(KSP of AgCl = 1.20 × 10-10)
  • 6.0 × 10-10 M
  • 0.2 M
  • 1.2 × 10-10 M
  • 0.2 × 10-10 M
Solid Ba (NO3)2 is gradually dissolved in a 1.0 × 10-4 M Na2CO3 solution. At what concentration of Ba2+ will a precipitate begin to form?
(KSP for BaCO3 = 5.1 × 10-9)
  • 4.1 × 10-5 M
  • 5.1 × 10-5 M
  • 8.1 × 10-8 M
  • 8.1 × 10-7 M
In qualitative analysis, in III group NH4 Cl is added before NH4OH because
  • to increase the concentration of NH4+ ions
  • to increase the concentration of Cl- ions
  • to reduce the concentration of OH- ions
  • to increase the concentration of OH- ions
If KP of Ag 2S is 10-17, then the solubility of Ag2S in 0.1 M solution of Na2S will be
  • 10-8
  • 5 × 10-9
  • 10-15
  • 10-16
Solubility product constant [Ksp ] of salts of types MX, MX2 and M3X at temperature T are 4.0 × 10-8, 3.2 × 10-14 and 2.7 × 10 respectively. Solubilities (mol, dm-3) of the salts at temperature T are in the order
  • MX > MX2 > M3X
  • M3X > MX2 > MX
  • MX2 > M3X > MX
  • MX > M3X > MX2
Solubility product of a salt AB is 1 x 10-8 M2 in a solution in which the concentration of A+ ions is 10-3 M. The salt will precipitate when the concentration of B- ions is kept
  • Between 10-8 to 10-7 M
  • between 10-7 M to 10-8 M
  • > 10-5 M
  • < 10-8 M
In a saturated solution of the sparingly soluble strong electrolyte AgIO3 (molecular mass =the equilibrium which sets in is
AgIO3 (s) ⇌ Ag+ (aq) IO3- (aq)
If, the solubility product constant Ksp of AgIO3 at a given temperature is 1.0 × 10-8, then what is the mass of AgIO3 contained in 100 mL of its saturated solution ?
  • 2.83 × 10-2 g
  • 2.83 × 10-3 g
  • 1.0 × 10-7 g
  • 1.0 × 10-4 g
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 × 10-15
  • 4 × 10-10
  • 1 × 10-15
  • 1 × 10-10
The solubility product of BaCl2 is 4 × 10-9. Its solubility (in mol/L) is
  • 4 × 10-3
  • 4 × 10-9
  • 1 × 10-3
  • 1 × 10-9
For which of the following sparingly soluble salt, the solubility (s)and solubility product (Ksp) are related by the expressions = (Ksp/4)1/3 ?
  • BaSO4
  • Ca3 (PO4)2
  • Hg2 Cl2
  • Ag3 PO4
  • CuS
The solubility of CaF2 is pure water is 2.3 × 10-6 mol dm-3. Its solubility product will be
  • 4.8 × 10-18
  • 48.66 × 10-18
  • 4.9 × 10-11
  • 48.66 × 10-15
The value of the ionic product of water depends
  • on volume of water
  • on temperature
  • changes by adding acid or alkali
  • always remain constant
Some chemists at ISRO wished to prepare a saturated solution of a silver compound and they wanted it to have the highest concentration of silver ion possible. Which of the following compounds, would they use?
KSP(AgCl) = 1.8 × 10-10
KSP (AgBr) = 5.0 × 10-13
KSP (Ag2CrO4) = 2.4 × 10-12
  • AgCl
  • AgBr
  • Ag2CrO4
  • None of these
The solubility product of a salt having general formula MX2, in water is 4 × 10-2 . The concentration of M 2+ ions in the aqueous solution of the salt is
  • 4.0 × 10-10 M
  • 1.6 × 10-10 M
  • 1.0 × 10-10 M
  • 2.0 × 10-3 M
At 90°C, pure water has H3O+ ion concentration of 10-6 mol /L-1. The Kw at 90°C is
  • 10-6
  • 10-14
  • 10-12
  • 10-8
Calculate the pH at the equivalence point during the titration of 0.1 M, 25 mL CH3 COOH with 0.05 M NaOH solution. [Ka (CH3 COOH) = 1.8 × 10-5]
  • 9.63
  • 8.63
  • 10.63
  • 11.63
One mole of ammonia was completely absorbed in 1L solution each of
I. M HCl
II. 1 M CH3COOH and
III. 1 M H2SO4 at 298 K
The decreasing order for the pH of the resulting solution is (given, Kb (NH3 ) = 4.
  • II > III > I
  • I > II > III
  • II > I > III
  • III > II > I
pH of an acid buffer is given by

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  • 2)
    Chemistry-Equilibrium-3578.png

  • Chemistry-Equilibrium-3579.png
  • None of these
The pKa of a certain weak acid is 4.0. What should be the [salt] to [acid] ratio if we have to prepare a buffer with pH = 5 using the acid, and one of the salts ?
  • 10 : 1
  • 1 : 10
  • 4 : 5
  • 5 : 4
An acidic buffer solution could be prepared by mixing the solutions of the following
  • sodium acetate and acetic acid
  • ammonium sulphate and sulphuric acid
  • ammonium chloride and ammonium hydroxide
  • sodium chloride and hydrochloric acid
20 mL 0.1 N acetic acid is mixed with 10 mL 0.1 N solution of NaOH. The pH of the resulting solution is (pKa of acetic acid is 4.
  • 3.74
  • 4.74
  • 5.74
  • 6.74
A 100 mL of 0.1 M solution of ammonium acetate is diluted by adding 100 mL of water. The pH of the resulting solution will be (pKa of acetic acid is nearly equal to pKb of NH4OH)
  • 4.9
  • 5.0
  • 7.0
  • 10.0
A buffer solution is prepared by mixing equal concentration of a weak base with its salt of strong acid. Kb for the base is 10-9 . pH of this buffer solution will be
  • 9
  • 4
  • 5
  • 13
A buffer solution contains 0.1 mole of sodium acetate dissolved in 1000 cm3 of 0.1M acetic acid. To the above buffer solution, 0.1 mole of sodium acetate is further added and dissolved. The pH of the resulting buffer is
  • pKa
  • pKa + 2
  • pKa - log 2
  • pKa + log 2
The pH of an aqueous solution of CH3 COONa of concentration C (M) is given by
  • 7 - 1/2pKa - 1/2 log C
  • 1/2pKw + 1/2 pKb + 1/2 log C
  • 1/2pKw - 1/2pKb - 1/2 log C
  • 1/2pKw + 1/2 pKa + log C
Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is
Chemistry-Equilibrium-3580.png
  • 1
  • 2
  • 3
  • 4
0:0:1


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