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1 markAcid/Base Equilibria

CAPE Chemistry Unit 1 · 2009 · Paper 2 · Question 5(d)(i)

Consider the following equation for a reversible reaction. Equation 2: H2S + H2O ⇌ H3O+ + HS-; Ka = 8.9 x 10-8

Define the term 'Brönsted - Lowry base'.

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Other parts of this question

  1. 5(a)State Le Chatelier's Principle.[2 marks]
  2. 5(b)(i)State the effect of EACH of the following on the equilibrium position of the reaction in Equation 1: An increase in pressure[2 marks]
  3. 5(b)(ii)State the effect of EACH of the following on the equilibrium position of the reaction in Equation 1: An increase in temperature[2 marks]
  4. 5(c)(i)When SO2 and O2 are mixed in a 2 : 1 ratio at 303 K the total equilibrium pressure of the system is 101.3 kPa. Calculate Kp at 303 K for the reaction in…[4 marks]
  5. 5(c)(ii)Comment on the value for Kp at 695 K for the reaction in Equation 1.[1 mark]
  6. 5(d)(ii)Identify TWO bases in Equation 2.[2 marks]
  7. 5(e)Calculate the pH of a 0.05 mol dm-3 solution of Ba(OH)2.[3 marks]

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