JEE Questions for Chemistry Equilibrium Quiz 12 - MCQExams.com

The pH of 10 M HCl aqueous solution is
  • less than 0
  • zero
  • 2
  • 1
When the pH of a solution is 2, the hydrogen ion concentration in moles per litre is
  • 1× 10–14
  • 1× 10–2
  • 1× 10–7
  • 1× 10–12
What is the OH− concentration of an aqueous solution of a substance whose pH= 3.2 ?
  • 10–3.8
  • 10–3.2
  • 10–10.8
  • 10–10.2
The number of H+ in 1 cc of a solution of pH = 13 is
  • 6.023 × 107
  • 1 × 10–13
  • 6.023 × 1013
  • 1 × 1016
In decimolar solution, CH3COOH is ionised to the extent of 1.3%. If log 1.3 = 0.11 , what is the pH of the solution ?
  • 3.89
  • 4.89
  • 2.89
  • unpredictable
The concentration of [H+] and concentration of [OH-] of a 0.1 aqueous solution of 2% ionised weak acid is [ ionic product of water = 1 × 10–4]
  • 0.02 × 10–3 M and 5 × 10–11 M
  • 1 × 10–3 M and 3 × 10–11 M
  • 2 × 10–3 M and 5 × 10–12 M
  • 3 × 10–2 M and 4 × 10–13 M
Which of the following solution will have pH close to 1.0 ?
  • 100 ml of M/10HCl+100 ml of M/10NaOH
  • 55 ml of M/10 HCl + 45 ml of M/10 NaOH
  • 10 ml of M/10 HCl + 90 ml M/10 NaOH
  • 75 ml of M/5 HCl + 25 ml of M/5 NaOH
The pH of 0.1 M solution of a weak acid is 3. What is the value of the ionisation constant for the acid?
  • 0.1
  • 10–3
  • 10–5
  • 10–7
A certain buffer solution contains equal concentration of X- and HX. The Ka for HX is10-8. The pH of the buffer is
  • 3
  • 8
  • 11
  • 14
The pKa of HCN is 9.30.The pH of a solution prepared by mixing 2.5 moles of KCN and 2.5 moles of HCN in water and making up the total volume of 500 ml is
  • 9.30
  • 7.30
  • 10.30
  • 8.30
Solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25. Then pKb of NH4OH is
  • 9.25
  • 4.75
  • 3.75
  • 8.25
If the solubility of PbCl2 at 250C is 6.3 × 10-3 mole/litre, its solubility product at that temperature is

  • Chemistry-Equilibrium-3973.png
  • 2)
    Chemistry-Equilibrium-3974.png

  • Chemistry-Equilibrium-3975.png

  • Chemistry-Equilibrium-3976.png
A saturated solution of Ag2SO4 has solubility 2.5 × 10-2 M The value of its solubility product is
  • 62.5 ×10–6
  • 6.25 ×10–4
  • 15.625 ×10–10
  • 3.125 ×10–6
If the maximum concentration of PbCl2 in water is 0.01 M at 250C, its maximum concentration in 0.1 M NaCl will be
  • 2 × 10–3 M
  • 1 × 10–4 M
  • 1.6 × 10–2 M
  • 4 × 10–4 M
The maximum amount of BaSO4 precipitated on mixing BaCl2 (0.5 M) with H2SO4(1M) will correspond to
  • 0.5 M
  • 1.0 M
  • 1.5 M
  • 2.0 M
The solubility of BaSO4 in water is 2.33 × 10–3 g L–1 . Its solubility product will be (molecular weight of BaSO4 =
  • 1 ×10–5
  • 1 ×10–10
  • 1 ×10–15
  • 1 ×10–20
The Ksp for M2SO4 at 298 K is 1.08 × 10–4. The maximum concentration of M+ that could be attained in a saturated solution of this solid at 298 K is
  • 3 × 10–2 M
  • 3 × 10–3 M
  • 2.89 × 10–4 M
  • 6 × 10–2 M
Solubility of an MX2 type electrolyte is 0.5 × 10–4 mole/lit , then ksp of the electrolyte is
  • 5 × 10–12
  • 25 × 10–10
  • 1 × 10–13
  • 5 × 10–13
The solubility product of AgI at 25ºC is 1.0 × 10–16 Mol2 L–2 The solubility of AgI in 10–14 N N solution of KI at 25ºC is approximately (in mol L–1)
  • 1.0 × 10–16
  • 1.0 × 10–12
  • 1.0 × 10–10
  • 1.0 × 10–8
How many ml of 1 M H2SO4 is required to neutralise 10 ml of 1 M NaOH solution?
  • 2.5
  • 5.0
  • 10.0
  • 20.0
At 25ºC, the dissociation constant of CH3COOH and NH4OH in aqueous solution are almost the same. The pH of a solution of 0.01 N CH3COOH is 4.0 at 25ºC The pH of 0.01N NH4OH solution at the same temperature would be
  • 3.0
  • 4.0
  • 10.0
  • 10.5
10 ml of a strong acid solution of pH 2.000 are mixed with 990 ml of a buffer solution of pH = 4.000. The pH of the resulting solution will be
  • 4.100
  • 4.000
  • 4.200
  • 3.800
The pH of 10—7 HCl aqueous solution of HCl at 25º C is
  • 7.0
  • less than 7
  • more than 7
  • None of the above(a - c)
Solutions A and B contain one and two moles of CH3COONH4 in one litre respectively. The hydrolysis will be
  • more in A
  • more in B
  • same in A and B
  • very little in A
Which of the following weakest ?

  • Chemistry-Equilibrium-4116.png
  • 2)
    Chemistry-Equilibrium-4117.png

  • Chemistry-Equilibrium-4118.png

  • Chemistry-Equilibrium-4119.png
The following reactions are known to occur in the body
Chemistry-Equilibrium-3986.png
  • pH will decrease
  • hydrogen ion concentration will diminish
  • H2CO3 concentration will be altered
  • The forward reaction will be promoted
When CO2 dissolves in water, the following equilibrium is established
Chemistry-Equilibrium-3987.png
  • 3.8 × 10−13
  • 3.8 × 10−1
  • 6.0
  • 13.4
A solution is a mixture of 0.05 M NaCl and 0.05 NaI. The concentration of iodide ion in the solution when AgCl just starts precipitating is equal to (Ksp(AgCl) = 1 × 10-10, Ksp(AgCI) = 4 × 10-16 )
  • 2 × 10-8 M
  • 3 × 10-6 M
  • 4 × 10-6 M
  • 2 × 10-7 M
The dissociation constants of mono basic acids A, B, C and D are 6 × 10-4, 5 × 10-3 and 7 × 10-10 respectively. The pH values of their 0.1 molar aqueous solutions are in the order
  • A < B < C < D
  • A > B > C > D
  • A = B = C = D
  • A > B < C > D
The maximum pH of a solution which is 0.1 M in Mg2+ from which Mg(OH)2 is not precipitated is
  • 4.96
  • 6.96
  • 7.54
  • 9.04
‘a’ moles of a monoacidic base are dissolved in one litre of the solution. The pH of the solution will be
  • –log a
  • 14 - log a
  • 14 + log a
  • –log (14 - a)
0.01 M solution of H2A has pH equal to 4. If Ka1 K for the acid is 4.5 × 10-7, the concentration of HA- ion in solution would be
  • 0.01 M
  • 4.45 × 10-5
  • 8.0 × 10-5
  • unpredictable
The solubility product (Ksp) of ferric hydroxide in aqueous solution is 3.8 × 10-38 at 298 K. The solubility of Fe3+ ions will increase when
  • pH is increased
  • pH is 7
  • saturated solution is exposed to atmosphere
  • pH is decreased
  • saturated solution is exposed to atmosphere.
Three sparingly soluble salts M2X, MX and MX3 have the same solubility product. Their solubilities will be in the order
  • MX3 > MX > M2X
  • MX3 > M2X > MX
  • MX > MX3 > M2X
  • MX > M2X > MX3
The pH values 1 M solutions of CH3COONa
(I), CH3COOH
(II), CH3COONH4
(III) NaOH
(IV) will be in the order
  • IV > I > III > II
  • IV > III >I > II
  • II > III > I > IV
  • I > II > III > IV
Given Ka1, Ka2 for H2S = 1.1 × 10-21 M3 1 L solution of 0.1 M H2S having [H+] = 0.1 M contains S2- ions is equal to
  • 6.62 × 103
  • 6.62 × 104
  • 6.62 × 105
  • 6.62 × 106

Chemistry-Equilibrium-3997.png

  • Chemistry-Equilibrium-3998.png
  • 2)
    Chemistry-Equilibrium-3999.png

  • Chemistry-Equilibrium-4000.png

  • Chemistry-Equilibrium-4001.png

Chemistry-Equilibrium-4003.png

  • Chemistry-Equilibrium-4004.png
  • 2)
    Chemistry-Equilibrium-4005.png

  • Chemistry-Equilibrium-4006.png

  • Chemistry-Equilibrium-4007.png

Chemistry-Equilibrium-4008.png

  • Chemistry-Equilibrium-4009.png
  • 2)
    Chemistry-Equilibrium-4010.png
  • RT

  • Chemistry-Equilibrium-4011.png

Chemistry-Equilibrium-4013.png

  • Chemistry-Equilibrium-4014.png
  • 2)
    Chemistry-Equilibrium-4015.png

  • Chemistry-Equilibrium-4016.png

  • Chemistry-Equilibrium-4017.png
Which one of the following statements is not true ?

  • Chemistry-Equilibrium-4018.png
  • 2)
    Chemistry-Equilibrium-4019.png

  • Chemistry-Equilibrium-4020.png
  • NH3 is a lewis base

Chemistry-Equilibrium-4022.png

  • Chemistry-Equilibrium-4023.png
  • 2)
    Chemistry-Equilibrium-4024.png

  • Chemistry-Equilibrium-4025.png

  • Chemistry-Equilibrium-4026.png

Chemistry-Equilibrium-4027.png

  • Chemistry-Equilibrium-4028.png
  • RT

  • Chemistry-Equilibrium-4029.png
  • 1.0

Chemistry-Equilibrium-4030.png

  • Chemistry-Equilibrium-4031.png
  • 2)
    Chemistry-Equilibrium-4032.png
  • 0.02
  • 50
Hydrogen ion concentration in mol /L in a solution of PH = 5.4 will be,

  • Chemistry-Equilibrium-4034.png
  • 2)
    Chemistry-Equilibrium-4035.png

  • Chemistry-Equilibrium-4036.png

  • Chemistry-Equilibrium-4037.png

Chemistry-Equilibrium-4039.png
  • reaction becomes fast
  • reaction becomes slow
  • equilibrium state disturbs
  • equilibrium state remains undisturbed

Chemistry-Equilibrium-4040.png

  • Chemistry-Equilibrium-4041.png
  • 120.48

  • Chemistry-Equilibrium-4042.png

  • Chemistry-Equilibrium-4043.png

Chemistry-Equilibrium-4044.png
  • KC remains unchanged,unchanged ,increase
  • KC increases.increases,decreases
  • KC remains unchanged ,increase,unchanged
  • KC decreases,increases,unchanged.

Chemistry-Equilibrium-4045.png

  • Chemistry-Equilibrium-4046.png
  • 2)
    Chemistry-Equilibrium-4047.png

  • Chemistry-Equilibrium-4048.png

  • Chemistry-Equilibrium-4049.png

Chemistry-Equilibrium-4050.png

  • Chemistry-Equilibrium-4051.png
  • 2)
    Chemistry-Equilibrium-4052.png

  • Chemistry-Equilibrium-4053.png

  • Chemistry-Equilibrium-4054.png
0:0:1


Answered Not Answered Not Visited Correct : 0 Incorrect : 0

Practice Chemistry Quiz Questions and Answers