JEE Questions for Chemistry Equilibrium Quiz 8 - MCQExams.com

Equal volumes of two solution of PH 3 and 4 are mixed.The PH of the resulting solution will be
  • 7
  • 3.5
  • 2.96
  • 3.26
PH of 10-8 M solution of HCl in water is
  • 8
  • -8
  • between 7 and 8
  • between 6 and 7
Calculate concentration of sodium acetate which should be added to 0.1 M solution of
Chemistry-Equilibrium-3627.png
  • 1.0 M
  • 0.1 M
  • 0.2 M
  • 10.0 M
Which of the following is a base according to lowry-bronsted concept ?
  • I –
  • H3O+
  • HCl
  • NH+4
According to lowry-bronsted concept which one of the following is considered as an acid ?
  • H3O+
  • BF3
  • OH–
  • Cl–

Chemistry-Equilibrium-3629.png

  • Chemistry-Equilibrium-3630.png
  • 2)
    Chemistry-Equilibrium-3631.png

  • Chemistry-Equilibrium-3632.png

  • Chemistry-Equilibrium-3633.png
Conjugate base of hydrazoic acid is

  • Chemistry-Equilibrium-3634.png
  • 2)
    Chemistry-Equilibrium-3635.png

  • Chemistry-Equilibrium-3636.png

  • Chemistry-Equilibrium-3637.png

Chemistry-Equilibrium-3639.png
  • (i) and (ii)
  • (ii) and (iii)
  • (iii) and (iv)
  • (i) and (iii)
One of the following is a bronsted acid but not a bronsted base :
  • H2S
  • H2O

  • Chemistry-Equilibrium-3640.png
  • NH3
With increase in temperature, ionic product of water
  • Decreases
  • Increases
  • Remains same
  • May increase or decrease.
EDTA is a/an
  • Arrhenius acid
  • Bronsted base
  • Lewis base
  • All of above
According to lowry and bronsted system, the chloride ion (Cl-) in aqueous solution is a
  • Weak base
  • Strong base
  • Weak acid
  • Strong acid
The PH of a buffer containing equal molar concentration of a weak base and its chlorides is (Kb for weak base = 2 × 10-5) (log 2 = 0.3010)
  • 5
  • 9
  • 4.7
  • 9.3

Chemistry-Equilibrium-3773.png

  • Chemistry-Equilibrium-3774.png
  • 2)
    Chemistry-Equilibrium-3775.png

  • Chemistry-Equilibrium-3776.png

  • Chemistry-Equilibrium-3777.png
Solution of 0.1 N NH4 OH and 0.1N NH4Cl has PH 9.25.Then PKbis
  • 9.25
  • 4.75
  • 3.75
  • 8.25
The least soluble compound (salt) of the following is

  • Chemistry-Equilibrium-3643.png
  • 2)
    Chemistry-Equilibrium-3644.png

  • Chemistry-Equilibrium-3645.png

  • Chemistry-Equilibrium-3646.png

Chemistry-Equilibrium-3647.png

  • Chemistry-Equilibrium-3648.png
  • 2)
    Chemistry-Equilibrium-3649.png

  • Chemistry-Equilibrium-3650.png

  • Chemistry-Equilibrium-3651.png
What is the [OH-] in the final solution prepared by mixing of 20.0 ml of 0.05 M HCl with 30.0 ml of 0.1 M Ba(OH)2 ?
  • 0.4 M
  • 0.05 M
  • 0.12 M
  • 0.1 M
Equimolar solution of the following were prepared in water separately. Which one of the solutions will record the highest PH ?
  • SrCl2
  • BaCl2
  • MgCl2
  • CaCl2
When H+ ion concentration of a solution increases
  • PH increses
  • PH decreases
  • no change in PH
  • POH decreases
Which one of the following has the lowest PH value ?
  • 0.1 M HCl
  • 0.1 M KOH
  • 0.01 M HCl
  • 0.01 M KOH
PH of a soda water bottle is
  • > 7
  • = 7
  • < 7
  • unpredictable
For preparing a buffer solution of PH 6 by mixing sodium acetate and acetic acid , the ratio of concentration of salt and acid should be, (Ka = 10-5)
  • 1 : 10
  • 10 : 1
  • 100 : 1
  • 1 : 100
The PH of neutral water is 6.8 .Then the temperature of H2O
  • is 250 C
  • is more than 250 C
  • is less than 250 C
  • can not be predicted.
The ionzation constant of formic acid is 7.8 × 10-4 . Calculate ratio of sodium formate & formic acid in a buffer of PH 4.25
  • 9.63
  • 3.24
  • 6.48
  • 3.97
The ionization constant of formic acid is 1.8 × 10-4 around what PH will its mixture with sodium formate give buffer solution of highest capacity
  • 3.74
  • 7.48
  • 4.37
  • 3.96
A certain buffer solution contains equal concentrations of X- and HX. The Ka for HX is 10-8 .The PH of buffer is
  • 7
  • 8
  • 3
  • 4

Chemistry-Equilibrium-3661.png
  • 2.48
  • 8.2
  • 5.26
  • 9.6
The PH of solution obtained by mixing 50ml 0.4 N HCl & 50ml 0.2 N NaOH is
  • - log 2
  • 1.0
  • - log 0.2
  • 2.0
In the reversible reaction A + B ⇌ C + D , the concentration of each C and D at equilibrium was 0.8 mol litre, then the equilibrium constant KC will be.
  • 6.4
  • 0.64
  • 0.16
  • 16.0
4 moles of A are mixed with 4 moles of B.At equilibrium for the reaction A + B ⇌ C + D 2 moles of C and D are formed . The equilibrium constant for reaction will be
  • 1/4
  • 4
  • 1/2
  • 1
A reversible chemical reaction having two reactants in equilibrium. If the concentration of the reactants are doubled, then equilibrium constantwill
  • become double
  • become half
  • become 4 times
  • remains same
If in the reaction N2O4 ⇌ 2NO2 , α is that part of N2O4 will dissociate, then the number of moles at equilibrium will be,
  • 3
  • (1 + α)
  • (1 – α)
  • 1
4.5 moles each of hydrogen and iodine heated in a sealed ten litre vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for H2(g) + I2(g) ⇌ HI(g) is
  • 1
  • 5
  • 10
  • 0.33

Chemistry-Equilibrium-3668.png

  • Chemistry-Equilibrium-3669.png
  • 2)
    Chemistry-Equilibrium-3670.png

  • Chemistry-Equilibrium-3671.png

  • Chemistry-Equilibrium-3672.png
If concentration of reactants is increased by \'x\' then k become
  • ln( k / x )
  • k / x
  • k + x
  • k

Chemistry-Equilibrium-3674.png
  • 10–11
  • 10–3
  • 11
  • 3
Select the pKa value of strongest acid from following
  • 1.0
  • 3.0
  • 2.0
  • 4.5

Chemistry-Equilibrium-3675.png

  • Chemistry-Equilibrium-3676.png
  • 2)
    Chemistry-Equilibrium-3677.png

  • Chemistry-Equilibrium-3678.png

  • Chemistry-Equilibrium-3679.png
The PH of a 0.01 M solution of acetic acid having degree of dissociation 1.25% is
  • 5.623
  • 2.903
  • 3.723
  • 4.503
By adding 20 ml 0.1 N HCl to 20 ml 0.1 N KOH the PH of obtained solution will be :
  • 0
  • 7
  • 2
  • 9

Chemistry-Equilibrium-3680.png

  • Chemistry-Equilibrium-3681.png
  • 2)
    Chemistry-Equilibrium-3682.png

  • Chemistry-Equilibrium-3683.png
  • None of these
Upto what PH must a solution containing a precipitate of (Cr(OH)3) be adjusted so that all precipitate dissolves
  • upto 4.4
  • upto 4.1
  • upto 4.2
  • upto 4.0
The initial rate of hydrolysis of methyl acetate (1M) by a weak acid (HA, 1 M) is 1/100th of that of a strong acid (HX, 1 M) at 25o C. The Ka HA is equal to
  • 1 × 10-4
  • 1 × 10-5
  • 1 × 10-6
  • 1 × 10-3
For the following three reactions I, II and III, equilibrium constants are given
I. CO (g) + H2O ⇌ CO2 (g) + H2 (g), K1
II. CH4 (g) + H2O (g) ⇌ CO (g) + 3H2 (g), K2
III. CH4 (g) + 2H2O (g) ⇌ CO2 (g) + 4H2 (g), K3
Which of the following relations is correct ?
  • K1 √K2 = K3
  • K2 K3 = K1
  • K3 = K1 K2
  • K3 K22 = K12

Chemistry-Equilibrium-3685.png
  • 1 × 10-10
  • 0.5
  • 5 × 10-8
  • 1 × 10-5
2.5 mL of 2/5 M weak monoacidic base (Kb =1 × 10-12 at 25oC) is titrated with 2/15 M HCl in water at 25oC. The concentration of H+ at equivalence point is (Kw = 1 × 10-14 at 25o C )
  • 3.7 × 10-13M
  • 3.2 × 10-7M
  • 3.2 × 10-2M
  • 2.7 × 10-2M
Look at the following reactions carried out in closed vessels:
(i) PCl5 → PCl3 + Cl2
(ii) N2 + O2 → 2NO
(iii) 2KClO3 → 2KCl + 3O2
(iV) Fe3+ + SCN– → Fe(SCN)2+
Which one of them is irreversible ?
  • (i)
  • (ii)
  • (iii)
  • (iv)
According to law of Mass Action, for the reaction 2A + B → Products
  • Rate = k [A] [B]
  • Rate = k [A]2 [B]
  • Rate = k [A] [B]2
  • Rate = k [A]1/2 [B]
If Δn = (np – nr) is the change in the number of moles of gaseous substances during a reaction, then equilibrium constants Kp and Kc are related as
  • Kp = Kc(RT)–Δn
  • Kc = Kp(RT)–Δn
  • Kp = (RT)Δn/ Kc
  • Kc – Kp = (RT)Δn
0:0:1


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