The hydrogen oxalate ion \( \ce{(HC2O4^{-})} \) is classified as amphiprotic.
Describe, using chemical equations, how this ion is amphiprotic. (2 marks)
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The hydrogen oxalate ion \( \ce{(HC2O4^{-})} \) is classified as amphiprotic.
Describe, using chemical equations, how this ion is amphiprotic. (2 marks)
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→ \(\ce{HC2O4−}\) is amphiprotic because it can either accept or donate an \(\ce{H+}\) as shown in the following equations:
\(\ce{HC2O4−(aq) + H+(aq) \rightleftharpoons H2C2O4(aq)}\)
\(\ce{HC2O4−(aq) + OH−(aq) \rightleftharpoons H2O(l) + C2O4^{2−}(aq)}\)
→ \(\ce{HC2O4−}\) is amphiprotic because it can either accept or donate an \(\ce{H+}\) as shown in the following equations:
\(\ce{HC2O4−(aq) + H+(aq) \rightleftharpoons H2C2O4(aq)}\)
\(\ce{HC2O4−(aq) + OH−(aq) \rightleftharpoons H2O(l) + C2O4^{2−}(aq)}\)
Sodium hydrogen carbonate is often used to clean up large spills of acids and alkalis.
Why is it a suitable chemical for this application?
`B`
→ Sodium hydrogen carbonate can donate and accept protons (amphiprotic).
→ This allows it to neutralise both acids and bases.
→ Sodium hydrogen carbonate usage also benefits from its stability.
`=>B`
Which of the following substances is amphiprotic in nature?
`A`
\(\ce{HSO4-}\) is amphiprotic.
→ It can accept a proton to form \(\ce{H2SO4}\)
→ It can donate a proton to form \(\ce{SO4^2-}\)
`=>A`
Which equation shows the hydrogen carbonate ion acting as a Brønsted-Lowry acid?
`C`
\(\ce{HCO3-}\) acts as a Bronsted-Lowry acid and donates a proton to \(\ce{NH3}\).
`=> C`