Reacting acids with carbonates
5 marks · HardA student adds an excess of dilute nitric acid to a sample of iron(II) carbonate in a beaker.
Write the balanced chemical equation for this reaction.
Name the salt formed in this reaction.
Write the total ionic equation for this reaction, omitting spectator ions.
Work this out on paper, then compare with the answer and worked solution below. With a free account you can submit written answers for marking.
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(a) \ce{FeCO3(s) + 2HNO3(aq) -> Fe(NO3)2(aq) + CO2(g) + H2O(l)}
(b) iron(II) nitrate
(c) \ce{FeCO3(s) + 2H^+(aq) -> Fe^{2+}(aq) + CO2(g) + H2O(l)}
Common mistakes: Incorrect balancing; Incorrect salt formula or name; Incorrect ionic charges or missing products
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Marking points
M1 (a) · 1 mark · Attempts equation with all correct reactants and products, with appropriate state symbols
A1 (a) · 1 mark · Equation is fully correctly balanced
B1 (b) · 1 mark · Correctly names the salt as iron(II) nitrate
M2 (c) · 1 mark · Correct ionic reactants and products, omitting spectator ions
A2 (c) · 1 mark · Fully balanced ionic equation with correct charges and state symbols
Worked solution
a) The balanced chemical equation is:
b) The salt formed is iron(II) nitrate.
c) The ionic equation, omitting nitrate (spectator) ions, is: