Equilibrium – Chemistry | NEET Online Mock Test

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 K_a and K_b values are known

Which one has the highest solubility in H₂O?

1. Na₂S
2. Cu₂S
3. Ag₂S
4. CdS

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

1. √s
2. s²
3. 4s³
4. 16s⁴

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

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

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

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

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

log (K_p/K_c) +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)

Find the value of △G^o for the reaction having K_eq value 4x10⁵ at 300K temperature.

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

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

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

1. SO₄^2-
2. HSO₄^-
3. NH₃
4. H₂PO₄^-

Find out the strongest conjugate base

1. Cl^-
2. NH₂-
3. I^-
4. SO₄^2-

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

If the [H⁺]=[OH^-]=10^-7 at 25°C then find pK_a of 1L H₂O. (d_H2O = 1g/ml)

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

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

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

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

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

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

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

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

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 K_c

An equilibrium mixture of NO₂ and N₂O₄ has a VD of 38.3 at 300K. What is K_p for the equilibrium N₂O_4(g) ⇋ 2NO_2(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

The pH of 10^-10 M NaOH solution is

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

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

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

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, K_b = 1.8×10^-5

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

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

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

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

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

The following reaction takes place in a 5L flask
2SO_2(g) + O_2(g) ⇋ 2SO_3(g), K_c = 5 at a constant temperature. At equilibrium the moles of SO₂ and SO₃ are equal. The mole of O₂ at equilibrium would be

If K_c for the reaction 2SO₂ + O₂ ⇋ 2SO₃, is 27, the K_c¹ (equilibrium constant) for
SO₂+1/2O₂ ⇋ SO₃ would be nearly equal to

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

Phosphorylation of glucose is non-spontaneous at 300K. △G^o 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

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

Which of the following is not correctly matched?

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

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

K_p for the reaction, N₂+3H₂ ⇋ 2NH₃ is 1.645×10^-4 atm^-2 at 400°C. What will be the K_p 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

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

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

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

At a certain temperature K_c = 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?

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

Which one is the conjugate base of HSO₄^-?

1. H₂SO₄
2. HSO₃
3. SO₃
4. SO₄^2-

Which one has the highest basic strength?

1. CH₃^-
2. NH₂^-
3. HCO₃^-
4. NO₃^-

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

pH of 10^-8M HCI is-

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

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