Question 1
Identify the Brønsted-Lowry acids in the following equilibrium. $$\ce{HCN(aq) + H2O(l) <=> CN^{-}(aq) + H3O^{+}(aq)}$$
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Chemistry · Unit 3 · Chemical equilibrium systems · Chemical equilibrium
Identify that acids are substances that can act as proton (hydrogen ion) donors.
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Question 2
Identify which substance acts as a proton donor in the following equilibrium: $$\text{NH}_4^+(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{NH}_3(\text{aq}) + \text{H}_3\text{O}^+(\text{aq})$$
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Question 3
Identify the Brønsted-Lowry acids in the following equilibrium. $$\mathrm{HCO_3^-(aq) + NH_3(aq) \rightleftharpoons CO_3^{2-}(aq) + NH_4^+(aq)}$$
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More in Chemical equilibrium
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Identify that acid-base indicators are a weak acid or a weak base where the conjugate acid - base pair have different colours and can be represented by HIn(aq) ⇋ H+(aq) + In−(aq) or BOH(aq) ⇋ B +(aq) + OH−(aq).
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Identify that amphiprotic species can act as Brønsted-Lowry acid (or base).