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Acids
GCSE chemistry and combined chemistry
| Question | Answer |
|---|---|
| What does soluble mean? What does insoluble mean? | Dissolves in water. Does not dissolve in water |
| Define acid in terms of pH | A substance with a pH of less than 7 |
| Define acids in terms of ions | A substance which releases H⁺ ions in solution |
| State the three common acids and give their formulae | Hydrochloric acid, HCl(aq), Sulphuric acid, H₂SO₄(aq), Nitric acid, HNO₃ |
| Which ions do the common acids form in solution? | HCl forms H⁺ and Cl⁻, H₂SO₄ forms 2H⁺ and SO₄²⁻, HNO₃ forms H⁺ and NO₃⁻ |
| What is a neutral solution? | A solution with a pH of 7. Water is an example. |
| How do you measure pH? | With an indicator or pH probe. |
| What is a base? | A metal oxide, hydroxide or carbonate that will react with an acid. E.g. copper oxide |
| What is an alkali? | A soluble base. E.g. sodium hydroxide |
| Which ions are always present in a solution of an alkali? | OH⁻ |
| What is a salt? | A compound formed when some or all of the hydrogen from an acid is replaced by a metal. E.g. CuSO₄, copper sulphate, where copper has replaced H from H₂SO₄ |
| What type of salts are formed by the three main acids? | Hydrochloric acid produces chlorides, sulphuric acid = sulphates, nitric acid = nitrates |
| What is a neutralisation reaction? Write an ionic equation for neutralisation. | A reaction involving an acid that results in a neutral solution. H⁺ + OH⁻ → H₂O |
| Which ions always react together in a neutralization reactions between acids and alkalis? | H⁺ and OH⁻ |
| metal + acid → | → salt + hydrogen gas |
| metal hydroxide + acid → | → salt + water |
| metal oxide + acid → | → salt + water |
| metal carbonate + acid → | → salt + water + carbon dioxide |
| How do you make a soluble salt from an acid? | React the acid with a base. E.g. to make copper sulphate react copper oxide with sulphuric acid |
| If a salt is in solution, how do you extract it as a solid? | Allow the water to evaporate off and it will leave the salt behind as a solid. |
| What is a strong acid? | An acid which completely splits up into its ions in water. E.g. when HCl is in water all the HCl molecules split up into H⁺ and Cl⁻. |
| What is a weak acid? | An acid which will have some molecules which do not split up into their ions. E.g. in ethanoic acid only some of the molecules will have split up into the ethanoate ion and H⁺ ions. |
| What is the relationship between an acid of pH2 and an acid of pH 3? | pH 2 is 10 times more hydrogen ions than pH 3 |
| What is a concentrated acid? | An acid where there are lots of acid particles in the water. |
| What is a dilute acid? | An acid where there are fewer acid particles in the water. |
| How is pH measured? | pH is related to the concentration of H⁺ in a solution. |
| How can hydrogen be tested for? | Makes a squeaky pop when a splint is placed in it |
| How can carbon dioxide be tested for? | Bubble through limewater, turns it milky (cloudy) |
| What colour is litmus in acid and alkali? | Acid – red, alkali – blue |
| What colour is methyl orange in acid and alkali? | Acid – red, alkali – yellow |
| What colour is phenol phthalein in acid and alkali? | Acid – colourless, alkali – pink |
| How do you prepare a sample of a soluble salt from a base and an acid? | Neutralisation, filtration, crystallisation |
| How do you prepare a sample of a soluble salt from an acid and an alkali? | Titration, repeat titration without indicator, crystallisation |
| How do you prepare a sample of an insoluble salt from two solutions | Combine, filtration. |
| Soluble or insoluble? nitrates | Soluble |
| Soluble or insoluble? Sodium salts | Soluble |
| Soluble or insoluble? Chloride salts | Soluble, except silver and lead compounds |
| Soluble or insoluble? sulphates | Soluble, except lead, barium and calcium compounds |
| Soluble or insoluble? carbonates | Insoluble, except sodium, potassium and ammonium |
| Soluble or insoluble? hydroxides | Insoluble, except sodium, potassium and ammonium |
Created by:
JBearfield
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