Y1 Acids, Bases and Salts Flashcards
Definition of an ‘Acid’
A proton donor
Definition of a ‘Base’
A proton acceptor
Definition of an ‘Alkali’
A water soluble base that releases OH- ions
Definition of a ‘Weak Acid’
An acid that will partially dissociate in aqueous solution
Definition of a ‘Strong Acid’
An acid that will fully dissociate in aqueous solution
Definition of a ‘Salt’
Ionic compounds formed when the H+ ions in acids are replaced by metal or ammonium ions
What is the test for halide ions?
Add aqueous silver nitrate (AgNO3)
What colour precipitate does AgCl(s) form and what concentrations of ammonia is it soluble in?
A white precipitate is formed and is soluble in both dilute and concentrated ammonia
What colour precipitate does AgBr(s) form and what concentrations of ammonia is it soluble in?
A cream precipitate is formed and is soluble in only concentrated ammonia
What colour precipitate does AgI(s) form and what concentrations of ammonia is it soluble in?
A yellow precipitate is formed and is not soluble in either dilute or concentrated ammonia
What is the ionic equation for the reaction between halide ions and aqueous silver chloride?
Ag+(aq) + Cl-(aq) 🔜 AgCl(s)
What is the test for sulfate (SO4 2-) ions?
Add barium chloride (BaCl2), a BaSO4(s) precipitate will form if sulfate ions are present
What is the test for (CO3 2-) carbonate ions?
Add an acid and CO2 will form if carbonate ions are present. Effervescence will occur and limewater will turn cloudy if it is used.
What is the test for (NH4 +) ammonium ions?
Add sodium hydroxide and ammonia (NH3) will form if ammonium ions are present. This will turn damp red litmus paper blue because it is an alkali.
What is the ionic equation for the reaction between ammonium ions and sodium hydroxide?
(NH4)+ 2(aq) + 2OH-(aq) 🔜 2NH3(g) + 2H2O(l)
