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2.6.3Inorganic Chemistry

Reactions of Acids — Edexcel International GCSE Science Double Award 4SD0 - Chemistry Revision Notes & Topical Questions

5 min read 7 parts Lesson 29 of 52

📚 Edexcel International GCSE Science Double Award 4SD0 - Chemistry Hub / Topical Revision
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Curriculum Equation Key pH & Acid-Base Equilibrium FormulasFast Exam Solution
pH = -log[H⁺] | pOH = -log[OH⁻] | pH + pOH = 14 | [H⁺][OH⁻] = 10⁻¹⁴
Word Equation & Conditions: pH + pOH = 14
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Part 1 of 5Acids and metals

General reaction
  • General reaction metal + acid → salt + hydrogen.
  • Only metals above hydrogen in the reactivity series react with dilute acids, and the more reactive the metal, the more vigorous the reaction.
Examples
  • Examples Mg + 2HCl → MgCl2 + H2.
  • Zn + H2SO4 → ZnSO4 + H2.
  • Very reactive metals such as potassium and sodium react explosively and should never be tried.
Test for hydrogen
  • Test for hydrogen A lit splint held at the mouth of the test tube gives a squeaky pop.

Part 2 of 5Naming the salt

AcidSalt formedExample
Hydrochloric acid, HClChlorideSodium chloride, NaCl
Sulfuric acid, H2SO4SulfateCopper sulfate, CuSO4
Nitric acid, HNO3NitrateZinc nitrate, Zn(NO3)2

Part 3 of 5Acids with oxides, hydroxides and carbonates

Acid reactions
Metal oxide or hydroxide
  • Metal oxide or hydroxide acid + base → salt + water. Example: CuO + H2SO4 → CuSO4 + H2O.
  • AnotherNaOH + HCl → NaCl + H2O.
Metal carbonate
  • Metal carbonate acid + carbonate → salt + water + carbon dioxide. Example: CuCO3 + 2HCl → CuCl2 + H2O + CO2.
Observation clue
  • Observation clue Fizzing (effervescence) shows a carbonate is reacting. Carbon dioxide turns limewater milky.
Nitric acid example
  • Nitric acid example Na2CO3 + 2HNO3 → 2NaNO3 + H2O + CO2.

Part 4 of 5Neutralisation as an ionic equation

1Full equation
  • Full equation HCl + NaOH → NaCl + H2O.
2Show the ions
  • Show the ions H+ + Cl− + Na+ + OH− → Na+ + Cl− + H2O.
3Remove spectators
  • Remove spectators Na+ and Cl− appear unchanged on both sides, so they are spectator ions.
4Net equation
  • Net equation H+(aq) + OH−(aq) → H2O(l), the same for any acid and alkali (HT only).

Part 5 of 5Safety

Dilute acids
  • Dilute acids Usually irritants; wear eye protection.
Concentrated acids
  • Concentrated acids Corrosive, so wear gloves as well. Nitric acid is also oxidising and can intensify a fire.
Hydrogen
  • Hydrogen Flammable gas, so keep away from naked flames when collecting it.

Key terms

TermMeaning
SaltA compound formed when the hydrogen of an acid is replaced by a metal or ammonium ion.
NeutralisationThe reaction of an acid with a base to form a salt and water.
EffervescenceFizzing caused by the release of a gas.
Spectator ionAn ion that is present but does not take part in a reaction.
Reactivity seriesA list of metals in order of how readily they react.

Avoid these mistakes

1
Calling the reaction of an acid with a metal neutralisation. It makes a salt and hydrogen, with no water.
2
Forgetting that carbonates also produce water as well as carbon dioxide.
3
Choosing the wrong salt namehydrochloric acid gives chlorides, not sulfates.
4
Including spectator ions in an ionic equation.

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