JEE Questions for Chemistry Equilibrium Quiz 3 - MCQExams.com

The pH value of 0.001M aqueous solution of NaCl is
  • 7
  • 4
  • 11
  • unpredicatble
A solution contains 10 mL of 0.1 N NaOH and 10 mL of 0.05 N H2 SO4 , pH of this solution is
  • less than 7
  • 7
  • zero
  • greater than 7

Chemistry-Equilibrium-3502.png
  • 8
  • 2
  • 1
  • 3
10-6M NaOH is diluted 100 times. The pH of the diluted base is
  • between 7 and 8
  • between 5 and 6
  • between 6 and 7
  • between 10 and 11
An aqueous solution whose pH is zero will be called as
  • acidic
  • basic
  • neutral
  • amphoteric
The pH values of 0.1 M solution of HCl , CH3 COOH , NH4Cl and CH3 COONa will have the order
  • HCl < CH3COOH < NH4Cl < CH3 COONa
  • CH3COONa < NH4Cl < CH3COOH < HCl
  • NH4Cl < CH3COONa < CH3COOH < HCl
  • All will have same of pH value
A weak acid HX has dissociation constant 10-5. The pH of 0.1 M solution of this acid will be
  • 2
  • 3
  • 4
  • 5
Which of the following acids will have lowest value of pKa ?
  • CH3 CH2 COOH
  • 2)
    Chemistry-Equilibrium-3503.png

  • Chemistry-Equilibrium-3504.png
  • FCH2 CH2 COOH
50mL of H2O is added to 50 mL of 1 × 10-3 M barium hydroxide solution. What is the pH of the resulting solution?
  • 3.0
  • 3.3
  • 11.0
  • 11.7
The pH of a 0.1 M solution of NH4OH
(having Kb = 1.0 × 10-5) is equal to
  • 10
  • 6
  • 11
  • 12
The pH of a solution obtained by mixing 50 mL of 1 N HCl and 30 mL of 1 N NaOH is (log 2.5 = 0.3979)
  • 3.979
  • 0.6021
  • 12.042
  • 1.2042
  • 0.3979
pH of a 0.0001 M HCl solution is
  • 4.0
  • 2.0
  • 6.0
  • 7.0
pH of an aqueous solution containing 10-8 mol /L of HCl is
  • 8
  • 10
  • 6.96
  • 12
100 mL of 0.015 M HCl solution is mixed with 100 mL of 0.005 M HCl. What is the pH of the resultant solution?
  • 2.5
  • 1.5
  • 2
  • 1
The pH of 10-8 M HCl solution is
  • 8
  • more than 8
  • between 6 and 7
  • slightly more than 7
Calculate the pH of a solution in which hydrogen ion concentration is 0.005 g-equi /L.
  • 2.3
  • 2.8
  • 2.9
  • 2.6
The approximately pH of 0.005 molar sulphuric acid is
  • 0.005
  • 2
  • 1
  • 0.001
Which solution has pH equal to 10 ?
  • 10-4 M KOH
  • 10-10 M KOH
  • 10-10 M HCl
  • 10-4 M HCl
A 0.01 M ammonia solution is 5% ionised, its pH will be
  • 11.80
  • 10.69
  • 7.22
  • 12.24
100 mL of 0.01 M solution of NaOH is diluted to 1 dm3.What is the pH of the diluted solution ?
  • 12
  • 11
  • 2
  • 3
Calculate pOH of 0.001 M NH4OH, when it is 1% dissociated in the solution.
  • 5
  • 2.96
  • 9.04
  • 11.4
What will be the pH value of 0.05 M Ba (OH)2 solution?
  • 12
  • 13
  • 1
  • 12.96
The pH value of 1/1000 N KOH solution is
  • 3
  • 10-11
  • 2
  • 11
The concentration of oxalic acid is x mol L-1.40 mL of this solution reacts with 16 mL of 0.05 M acidified KMnO4. What is the pH of x M oxalic acid solution? (assume that oxalic acid dissociates completely)
  • 1.3
  • 1.699
  • 1
  • 2
20 mL of 0.5 N HCl and 35 mL of 0.1 N NaOH are mixed. The resulting solution will
  • be neutral
  • be basic
  • turn phenolphthalein solution pink
  • turn methyl orange red
The pH of an aqueous solution having hydroxide ion concentration as 1 x 10-5 is
  • 5
  • 9
  • 4.5
  • 11
An aqueous solution of 1 M NaCl and 1 M HCl is
  • not a buffer but pH < 7
  • not a buffer but pH > 7
  • a buffer with pH < 7
  • a buffer with pH > 7
The solubility product of Ag2 Cr O4 is 32 x 10-2. What is the concentration of CrO4- ions in that solution?
  • 2 × 10-4 M
  • 16 × 10-4 M
  • 8 × 10-4 M
  • 8 × 10-8 M
What will be solubility product of Ca(OH)2 if its solubility is √3 ?
  • 3
  • 3√3
  • 12√3
  • 27
Which of the following salts has the greatest molar solubility in pure water?
  • CaCO3 (KSP = 8.7 x 10-9 )
  • CuS (KSP = 8.5 x 10-45)
  • Ag2CO3 (KSP = 6.2 x 10-12 )
  • Pb9IO3 (KSP = 2.6 x 10-13 )
Given the KSP expression. KSP = [A3+]2 [B2-]3
  • A2B3 (s) ⟺ 3A3+ (aq) + 2B2- (aq)
  • A2B3 (s) ⟺ 3A3+ (aq) + 3B2- (aq)
  • A3B2 (s) ⟺ 3A3+ (aq) + 2B2- (aq)
  • A3B2 (s) ⟺ 2A3+ (aq) + 3B2- (aq)
The solubility product of a binary weak electrolyte is 4 × 10-10 at 298 K. Its solubility (in mol dm-3) at the same temperature is
  • 4 × 10-5
  • 2 × 10-5
  • 8 × 10-10
  • 16 × 10-20
The solubility of CaF2 is s mol/L. Then, solubility product is
  • S2
  • 4S3
  • 4S2
  • S3
H2S is passed into 1 dm3 of a solution containing 0.1 mole of Zn2+ and 0.01 mole of Cu2+ till the sulphide ion concentration reaches 8.1 × 10-19 mole. Which one of the following statement is correct ?
(KSP of ZnS and CuS are 3 × 10-22 and 8 × 10-36, respectively)
  • Only ZnS precipitates
  • Both CuS and ZnS precipitate
  • Only CuS precipitates
  • No precipitation occurs
The solubility of Ca3(PO4 )2 in water is y mole / L. Its solubility product is
  • 6 y4
  • 36 y4
  • 64 y5
  • 108 y5
The expression for the solubility product of Ag2CO3 will be
  • Ksp = s2
  • Ksp = 4s3
  • Ksp = 27s4
  • Ksp = s
1 dm3 solution containing 10-5 moles each of Cl- ions and CrO42- ions is treated with 10-4 moles of silver nitrate. Which one of the following observations is made ?
(Ksp Ag2 CrO4 = 4 × 10-12) (KspAgCl = 1 × 10-10)
  • Precipitation does not occur
  • Silver chromate gets precipitated first
  • Silver chloride gets precipitated first
  • Both silver chromate and silver chloride start precipitating simultaneously
The solubility product of Hg2I2 is equal to
  • [Hg22+] [I-]
  • [Hg2+][I-]
  • [Hg22+][I-]2
  • [Hg2+][I-]2
Approximate relationship between dissociation constant of water (K) and ionic product of water (Kw) is
  • Kw = K
  • Kw = 55.6 × K
  • Kw = 18 × K
  • Kw = 14 × K
Which of the following has the highest value of solubility product?
  • CuS
  • Bi2S3
  • CdS
  • ZnS
The solubility product of iron (III) hydroxide is 1.6 × 10-39. If X is the solubility of iron (III) hydroxide, then which one of the following expressions can be used to calculate X ?
  • Ksp = X4
  • Ksp = 9X4
  • Ksp = 27X3
  • Ksp = 27X4
Solubility of Ca(OH)2 is a s mol L-1. The solubility product (Ksp ) under the same condition is
  • 4s3
  • 3s4
  • 4s2
  • s3
Addition of sodium acetate to 0.1 M acetic acid will cause
  • increase in pH
  • decrease in pH
  • no change in pH
  • change in pH that cannot be predicted
Solubility product of Mg(OH)2 at ordinary temperature is
1.96 × 10-11. pH of a saturated solution, of Mg(OH)2 will be
  • 10.53
  • 8.47
  • 6.94
  • 3.47
An aqueous solution contains Ni2+ , Co2+ and Pb2+ ions at equal concentrations. The solubility product of NiS, PbS and CoS in water at 25oC are 1.4 × 10-24, 3.4 × 10-28 and 3 × 10-26, respectively. Indicate which of these ions will be precipitated first and last when sulphide concentration is progressively increased from zero?
  • NiS and PbS
  • NiS and CoS
  • CoS and NiS
  • PbS and NiS
The solubility of AgC1 in 0.2 M NaCl is
(Ksp of AgCl = 1.8 × 10-10)
  • 1.8 × 10-11 M
  • 9 × 10-10 M
  • 6.5 × 10-12 M
  • 5.6 × 10-11
The solubility of AgCl is l × 10-5 mol/L. Its solubility in 0.1 molar sodium chloride solution is
  • 1 × 10-10
  • 1 × 10-5
  • 1 × 10-9
  • 1 × 10-4
The solubility product of a sparingly soluble salt AX2 is 3.2 × 10-11. Its solubility (in mol/L) is
  • 5.6 × 10-6
  • 3.1 × 10-4
  • 2 × 10-4
  • 4 × 10-4
When ammonium chloride is added to ammonia solution, the pH of the resulting solution will be
  • increased
  • seven
  • decreased
  • unchanged
Solubility of AgCl at 20°C is 1.435 × 10-3 g/ L. The solubility product of AgCl is
  • 1 × 10-5
  • 1 × 10-10
  • 1.435 × 10-5
  • 108 × 10-3
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