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Rates, equilibrium and pH

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Question 19

In an intracellular buffer system, dihydrogenphosphate (H2PO4−\text{H}_2\text{PO}_4^-H2​PO4−​) and hydrogencarbonate (HCO3−\text{HCO}_3^-HCO3−​) ions react to establish the following equilibrium:

H2PO4−(aq)+HCO3−(aq)⇌HPO42−(aq)+H2CO3(aq) \text{H}_2\text{PO}_4^-(\text{aq}) + \text{HCO}_3^-(\text{aq}) \rightleftharpoons \text{HPO}_4^{2-}(\text{aq}) + \text{H}_2\text{CO}_3(\text{aq}) H2​PO4−​(aq)+HCO3−​(aq)⇌HPO42−​(aq)+H2​CO3​(aq)

What are the Brønsted–Lowry bases in this equilibrium mixture?

H2PO4−\text{H}_2\text{PO}_4^-H2​PO4−​ and H2CO3\text{H}_2\text{CO}_3H2​CO3​

H2PO4−\text{H}_2\text{PO}_4^-H2​PO4−​ and HCO3−\text{HCO}_3^-HCO3−​

HPO42−\text{HPO}_4^{2-}HPO42−​ and H2CO3\text{H}_2\text{CO}_3H2​CO3​

HCO3−\text{HCO}_3^-HCO3−​ and HPO42−\text{HPO}_4^{2-}HPO42−​

Rates, equilibrium and pH Questions

  1. A Level
  2. /Chemistry
  3. /Rates, equilibrium and pH