Chemical Equilibrium Questions for NEET

What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed

At 25°C, the dissociation constant of a base, BOH, is 1.0 × 10^–12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be

Which of the following is not a Lewis acid?

Buffer solutions have constant acidity and alkalinity because

The strongest conjugate base is

If a is the dissociation constant, then the total number of moles for the reaction, 2HI → H₂ + I₂ will be

Conjugate acid of NH₂^– is

The solubility product of a sparingly soluble salt AX2 is 3.2 × 10^–11. Its solubility (in moles/L) is

The solubility of MX2 type electrolytes is 0.5 × 10^–4 mol/lit., then find out Ksp of electrolytes.

The dissociation constant of a weak acid is 1 × 10^–4. In order to prepare a buffer solution with a pH = 5, the [Salt]/[Acid] ratio should be

Ionization constant of CH₃COOH is 1.7 × 10^–5 and concentration of H⁺ ions is 3.4 × 10^–4. Then find out the initial concentration of CH₃COOH molecules.

Aqueous solution of acetic acid contains

Which compound is electron deficient?

The solubility of M2S salt is 3.5 × 10^–6 then find the solubility product.

At 100°C the Kw of water is 55 times its value at 25°C. What will be the pH of neutral solution? (log 55 = 1.74)

Which one of the following information can be obtained on the basis of the Le Chatelier principle?

Which of the following pairs constitutes a buffer?

Calculate the pOH of a solution at 25°C that contains 1 × 10^–10 M of hydronium ions, i.e. H₃O⁺.

Which one of the following molecular hydrides acts as a Lewis acid?

Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?

Which one of the following pairs of solutions is not an acidic buffer?

What is the [OH^–] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)₂?

A weak acid, HA, has a Ka of 1.00 × 10^–5. If 0.100 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to

In the Haber process, 30 liters of dihydrogen and 30 liters of dinitrogen were taken for the reaction which yielded only 50% of the expected product. What will be the composition of a gaseous mixture under the aforesaid condition in the end?

The pH value of N/10 NaOH solution is

The pH value of a 10 M solution of HCl is

Repeated use of which one of the following fertilizers would increase the acidity of the soil?

The pH of 0.01 M NaOH(aq) solution will be

Which has the highest pH?

If the value of the equilibrium constant for a particular reaction is 1.6 × 10¹², then at equilibrium the system will contain

Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the H⁺ ion concentration in the mixture?

Aqueous solution of which of the following compounds is the best conductor of electric current?

At 80°C, distilled water has [H₃O⁺] concentration equal to 1 × 10^–6 mole/liter. The value of Kw at this temperature will be

Which one of the following statements is not true?

The hydrogen ion concentration of a 10^–8 M HCl aqueous solution at 298 K (Kw = 10^–14) is

The ionization constant of ammonium hydroxide is 1.77 × 10^–5 at 298 K. Hydrolysis constant of ammonium chloride is

Which of the following salts will give highest pH in water?

Which one of the following compounds is not a protonic acid?

Conjugate base for Bronsted acids H₂O and HF are

0.1 M solution of which one of these substances will act basic?

The solubility of a saturated solution of calcium fluoride is 2 × 10^–4 moles per liter. Its solubility product is

The ionic product of water at 25°C is 10^–14. Its ionic product at 90°C will be,

Which of the following molecules acts as a Lewis acid?

In liquid-gas equilibrium, the pressure of vapors above the liquid is constant at

Which of the following fluoro-compounds is most likely to behave as a Lewis base?

Which of the following cannot act both as Bronsted acid and as Bronsted base?