Acids, bases and equilibrium

What is the pH of 0.01 M hydrochloric acid?

• 1 12
• 2 7
• 3 1
• 4 2

What is the pH of 0.001 M sodium hydroxide at 25 degrees C?

• 1 11
• 2 10
• 3 3
• 4 13

What is the conjugate base of H2SO4?

• 1 SO4 2-
• 2 H3SO4+
• 3 OH-
• 4 HSO4-

For N2 + 3H2 <-> 2NH3, increasing the pressure shifts the equilibrium:

• 1 To the left
• 2 To the right
• 3 It does not change
• 4 Only if a catalyst is added

A buffer solution is made of:

• 1 A strong acid and a strong base
• 2 Pure water and a salt
• 3 Two salts of strong acids
• 4 A weak acid and its salt

What is the pOH of a solution whose pH is 4 at 25 degrees C?

• 1 14
• 2 4
• 3 7
• 4 10

Which expression gives the solubility product Ksp of AgCl?

• 1 [Ag+] x [Cl-]
• 2 [Ag+] / [Cl-]
• 3 [AgCl]
• 4 [Ag+] + [Cl-]

A larger value of Ka means that the acid is:

• 1 Weaker
• 2 Stronger
• 3 More basic
• 4 Unable to ionise

The pH of a solution with a hydrogen ion concentration of 1 × 10⁻³ mol/dm³ is:

• 1 11
• 2 3
• 3 −3
• 4 7

A buffer solution is one that:

• 1 Changes colour at its end point
• 2 Resists a change in pH when small amounts of acid or base are added
• 3 Has a pH of exactly 7
• 4 Contains only a strong acid

For the reaction N₂ + 3H₂ ⇌ 2NH₃ (exothermic), increasing the pressure shifts the equilibrium:

• 1 Towards ammonia
• 2 Towards nitrogen and hydrogen
• 3 Not at all
• 4 Towards the side with more moles of gas