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Equilibrium – Chemistry | NEET Online Mock Test

Online Mock Test Description

Mock TestEquilibrium
ExamNEET Medical Test
SubjectChemistry
Marks100
No. Questions50 Questions
Time50 Minutes

2

Equilibrium - NEET (Chemistry)

Best of Luck!

1 / 50

The pH of the solution containing a salt of weak acid and a weak base

  1. Is always greater than 7
  2. Is always equal to 7
  3. Is always less than 7
  4. Can't be predicted unless Ka and Kb values are known

2 / 50

Which one has the highest solubility in H2O?

  1. Na2S
  2. Cu2S
  3. Ag2S
  4. CdS

3 / 50

Find Ksp for Hg2Cl2(s) if its solubility is 's' mol/L at 25°C

  1. √s
  2. s2
  3. 4s3
  4. 16s4

4 / 50

Find pH of a solution when 100 mL of 0.1 N HCI is mixed with 100 mL of 0.1 M NH4OH solution
[pKa(NH4+)=9.3]

5 / 50

Which of the following is the suitable indicator for H2SO4 & NH4OH titration reaction?

6 / 50

A+B ⇋ C+D for this reaction Kc=9. If A and B are taken in equal amounts, ratio of mole of C and A at equilibrium is

7 / 50

For CaCO3(s) ⇋ Cao(s)+CO2(g) the pressure of CO2 at equilibrium is 8 atm. Then the value of Kp is-

  1. 64 atm2
  2. 8 atm
  3. 8 atm-1
  4. 1/8 atm-1

8 / 50

log (Kp/Kc) +log RT=0 is a relationship for the reaction:-

  1. PCI5(g) ⇋ PCl3(g) + Cl2(g)
  2. H2(g) + l2(g) ⇋ 2HI(g)
  3. N2(g) +3H2(g) ⇋ 2NH3(g)
  4. 2SO2(g) + O2(g) ⇋ 2SO3(g)

9 / 50

Find the value of △Go for the reaction having Keq value 4x105 at 300K temperature.

10 / 50

The introduction of inert gas (at the same temperature) will affect the equilibrium if-

  1. Volume is constant and △ng = 0
  2. Volume is constant and △ng ≠ 0
  3. Pressure is constant and △ng ≠ 0
  4. Pressure is constant and △ng = 0

11 / 50

Select from the following molecules/species that can't act as amphiprotic

  1. SO42-
  2. HSO4-
  3. NH3
  4. H2PO4-

12 / 50

Find out the strongest conjugate base

  1. Cl-
  2. NH2-
  3. I-
  4. SO42-

13 / 50

Find the correct order of acidity-

  1. HCIO4>HCI>H2CO3>H2O
  2. H2CO3>HCIO >HCI>H2O
  3. HCI>HCIO4>H2CO3>H2O
  4. HCIO4 >HCI>H2O>H2CO3

14 / 50

If the [H+]=[OH-]=10-7 at 25°C then find pKa of 1L H2O. (dH2O = 1g/ml)

15 / 50

Calculate the pH of mixture of 400ml 0.01M HCI and 600ml H2O

16 / 50

Calculate the pOH of the equimolar mixture of NH4OH and NH4 Cl.
(given Kb for NH4OH = 2×10-5)

17 / 50

Calculate the value of the hydrolysis constant of KCN
(given Ka of HCN= 1x10-6)

  1. 10-8
  2. 10-12
  3. 10-20
  4. 10-2

18 / 50

The pH value of the aqueous solution of 0.1 M NaNO3 is-

19 / 50

The solubility product of AgCl is 1.8 x 10-10. Precipitation of AgCl will occur only when equal volumes of solutions of

  1. 10-7M Ag+ and 10-7 M Cl- are mixed
  2. 10-5M Ag+ and 10-5 M Cl- are mixed
  3. 10-4M Ag+ and 2 x 10-5 M Cl- are mixed
  4. 10-5M Ag+ and 2 x 10-5 M Cl- are mixed

20 / 50

Solubility of Ag2CrO4(s) is maximum in

  1. 0.1 M of AgNO3 Solution
  2. 0.1 M of H2CrO4 Solution
  3. 0.1 M of NaCN Solution
  4. Pure Water

21 / 50

The equilibrium constant for the reaction
A2(g) + B2(g) 2AB(g) is Kc = 10-2 at 27°C
The standard Gibbs free energy change for the reaction will be

22 / 50

1 mole of H2O and 1 mole of CO are taken in a 10 litre vessel and heated at 725K. At equilibrium, 40% of water (by mass) reacts with CO according to the equation.

H2O(g) +CO(g) ⇋ H2(g) + CO2(g) .Find the value of Kc

23 / 50

An equilibrium mixture of NO2 and N2O4 has a VD of 38.3 at 300K. What is Kp for the equilibrium N2O4(g) ⇋ 2NO2(g) if initially one mole of N2O4 is present and the equilibrium pressure is 1 atm?

  1. 0.166 atm
  2. 0.166 atm²
  3. 0.96 atm
  4. 0.96 atm²

24 / 50

The pH of 10-10 M NaOH solution is

25 / 50

A 0.05 N solution of CH3COOH is found to be 1.9% ionised. Calculate its Ka.

  1. 2.9×10-5
  2. 5.4×10-5
  3. 1.8×10-5
  4. 2.4×10-5

26 / 50

Calculate the pH of a solution of 0.1M NH3 Kb = 1.8 x 10-5

27 / 50

A buffer solution with pH 9 is to be prepared by mixing NH4CI and NH4OH. Calculate the number of moles of NH4Cl that should be added to 1 litre of 1M NH4OH, Kb = 1.8×10-5

28 / 50

pH of a solution decreased from 4 to 2 then the concentration of hydrogen ion will be

29 / 50

The solubility of lead iodide is 0.63g/lit. Calculate its Ksp. (Pb=207, I=127)

  1. 1×10-6
  2. 2×10-6
  3. 1×10-8
  4. 2×10-8

30 / 50

pKa of CH3COOH is 4.74. pH of a solution obtained by mixing 1L 1 M CH3COOH with 40g NaOH is

31 / 50

pH of an aqueous solution obtained by mixing 4 g NaOH in 500 mL water is:

32 / 50

The following reaction takes place in a 5L flask
2SO2(g) + O2(g) ⇋ 2SO3(g), Kc = 5 at a constant temperature. At equilibrium the moles of SO2 and SO3 are equal. The mole of O2 at equilibrium would be

33 / 50

If Kc for the reaction 2SO2 + O2 ⇋ 2SO3, is 27, the Kc1 (equilibrium constant) for
SO2+1/2O2 ⇋ SO3 would be nearly equal to

34 / 50

Vapour density of N2O4 is 45.86 at a certain temperature. The degree of dissociation of N2O4 at the same temperature would be approximately

35 / 50

Phosphorylation of glucose is non-spontaneous at 300K. △Go is found to be 14 kJ mol-1. The thermodynamic equilibrium constant will be

  1. 3.65 x 10-2
  2. 3.65 x 10-3
  3. 3.65 x 10-4
  4. 3.65 x 10-5

36 / 50

At a temperature T K, the concentration of OH- is 10-5.5, the value Kw would be 10x in absence of acid/base. The value of x is

37 / 50

Which of the following is not correctly matched?

  1. F- Lewis base
  2. Ag+ Lewis acid
  3. BH3 Lewis base
  4. FeCl3 Lewis acid

38 / 50

4.0 gm of hydrogen and 128g of hydrogen iodide are present in a 10-litre flask. The active mass of hydrogen iodide is

  1. 0.15(M)
  2. 0.1 mole L-1
  3. 0.01 mol L-1
  4. 0.2 mol L-1

39 / 50

Kp for the reaction, N2+3H2 ⇋ 2NH3 is 1.645×10-4 atm-2 at 400°C. What will be the Kp at 500°C? The heat of the reaction in this temperature range is -25.14 kcal.

  1. Greater than 1.645 x 10-4 atm-2
  2. Smaller than 1.645 x 10-4 atm-2
  3. Equal to 1.645 × 10-4 atm-2
  4. Greater than or equal to 1.645 x 10-4 atm-2

40 / 50

For the following reaction, 2SO3 ⇋ 2S02+0₂ if the observed vapour density of the mixture at equilibrium is 30 then find the degree of dissociation of SO3

41 / 50

In the dissociation of HI 20% is dissociated at equilibrium.
Calculate Kp for Hl(g) ⇋ 1/2 H2(g)+1/2 l2(g)

42 / 50

A ⟶ 2B+C Kc =1.987 x 10-8 mole2 litre-2 then at equilibrium the reaction mixture contains a greater number of moles of

43 / 50

At a certain temperature Kc = 1.8 litre2 mole-2 for N2+3H2 ⇋ 2NH3. How many moles of NH3 must be placed in one litre vessel in order to get 6 mole litre-1 H2 at equilibrium?

44 / 50

NH4HS(s) NH3(g)+H2S (g). At a certain temperature Kp = 1.44 atm2. If the partial pressure of NH3 at a certain extent is 1.08 atm. Then the reaction will proceed

45 / 50

Which one is the conjugate base of HSO4-?

  1. H2SO4
  2. HSO3
  3. SO3
  4. SO42-

46 / 50

Which one has the highest basic strength?

  1. CH3-
  2. NH2-
  3. HCO3-
  4. NO3-

47 / 50

If we increase the temperature, then the pH value of pure water

48 / 50

pH of 10-8M HCI is-

49 / 50

Which of the following statements is incorrect?

  1. Melting of ice increases due to an increase in pressure
  2. K2SO4 doesn't undergo hydrolysis
  3. Human blood is a basic buffer
  4. Solubility of NaCl in H2O decreases with an increase in temperature

50 / 50

Calculate the pH of the solution containing equal moles of (NH4)2SO4 & NH4OH. Kb for NH4OH is 2 x 10-5

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