Equilibrium

The heat of neutralisation of a strong acid and a strong alkali is 57.0 kJ mol^-1.The heat released when 0.5 mole of HNO₃ solution is mixed with 0.2 mole of KOH is 

• 57.0 kJ

• 11.4 kJ

• 28.5 kJ

• 34.9 kJ

Ammonium acetate which is 0.01 M, is hydrolysed to 0.001 M concentration. Calculate the change in pH in 0.001 M solution, if initially pH = pK_a

• 5

• 10

• 100

• 1

The solubility product of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4 \mathrm{is} 32 \times {10}^{-12}$. What is the concentration of ${\mathrm{CrO}}_4^{2-}$ ions in that solution?

• $2 \times {10}^{-4}$

• $16 \times {10}^{-4}$

• $8 \times {10}^{-4}$

• $12\times {10}^{-4}$

Conjugate acid-base pair differ by

• electron

• proton

• neutron

• hydroxyl group

Which is not an example of common ion effect?

• NaCl+ AgCl

• H₂S+ HCl

• CH₃COOH+ NaOH

• NH₄OH+ NH₄Cl

NH₄Cl is acidic due to

• cationic hydrolysis

• anionic hydrolysis

• its ionic nature

• pH > 7

An acid solution of pH = 6 is diluted 1000 times, the pH of the final solution becomes

• 6.01

• 9

• 3.5

• 6.99

The conjugate acid of HS^- is

• S^2-

• H₂S

• Both (a) and (b)

• None of these

Which of the following is a weak acid?

• C₆H₆

• CH₃COOH

• CH₂=CH₂

• CH₃COCH₃

The hydrogen ion concentration of a solution is 3.98 × 10^-6 mole per liter. The pH value of this solution will be

• 6.0

• 5.8

• 5.4

• 5.9