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Cards (41)

  • Observations when a dilute acid is added to carbonate ion?
    Effervesence, carbon dioxide is produced (which can be tested using limewater).
  • Observations when chloride ion in solution is mixed with a dilute nitric acid and aqeous silver nitrate?

    White precipitate forms
  • Observations when bromide anion is axidified with dilute nitric acid and aqueous silver nitrate?
    Cream precipitate
  • Observations when iodide anion is acidified with dilute nitric acid and aqeous silver nitrate?
    Yellow ppt
  • Observation when nitrate anion in solution is added to aqeous sodium hydroxide, then aluminium foils and is warmed?
    Ammonia is produced (which can be tested for by using damp litmus paper - will turn blue).
  • Observation when sulfate anion in solution is added acidified dilute nitric acid, then add aqeous barium nitrate?
    White ppt
  • Observation when sulfite anion is tested for by adding small voluem of acidified potassium manganate (VII)?

    Potassium manganate changes from purple to colourless.
  • Observations to test for Al+ in aqeous sodium hydroxide?
    White ppt. soluble in excess, colourless solution
  • Observations for NH4 (ammonium) in aqeous sodium hydroxide?
    Ammonia produced on warming - no ppt.
  • Observations for CA2+ in aqeous sodium hydroxide?
    White ppt
  • Observations of chromium (III), Cr3+ in aqeous sodium hydroxide?
    Green ppt, insolubel in excess.
  • Observations of Copper (11) Cu 2+ in aqeous sodium hydroxide?
    Light blue ppt, insoluble in excess,
  • Observations of iron (II) Fe2+ in aqeous sodium hydroxide?
    Green ppt, soluble in excess
  • Observations of iron (III) Fe3+ in aqeous sodium hydroxide?
    red-brown ppt, insoluble in excess
  • Observation of Zinc Zn2+ in aqeous sodium hydorxide?
    White ppt, soluble in excess and gives a coulourless solution
  • Observations of Al3+ in aqeous ammonia?
    White ppt. insoluble in excess
  • Observations of Ca2+ in aqeous ammonia?
    No ppt, or a slight white ppt
  • Observations of Cr3+ in aqeous ammonia?
    green ppt, insoluble in excess
  • Observations Cu2+ in aqeous ammonia
    Light blue ppt, soluble in excess, dark blue solution
  • Observations of Fe2+ in aqeous ammonia?
    green ppt, insolble in excess and turns brown near surface on standing
  • Observations of Fe3+ in aqeous ammonia?
    Red-brown ppt, insolble in excess
  • Observations of Zn2+ in aqeous ammonia?
    White ppt. SOluble in excess, gives a colourless solution
  • What is a saturated solution?
    A solution in which no more solute can dissolve at a given temperature.
  • Predict the state and colour of astantine at room temperature
    Black solid
  • How can you predict the states and colours of the halogens?
    The halogens get darker in colour as you go down the group - fluorine and chlorine are gases, bromine is a liquid and iodine and astantine are solids.
  • Predict the state and colour of fluorine?
    Gas, pale yellow
  • Predict the state and colour of chlorine?
    Gas, green
  • Predict the state and colour of bromine?
    State: Liquid Color: Red
  • Predict the state and colour of iodine?
    Solid, purple
  • If you were purifying nickel by electrolysis, what would the anode and cathode be made of?
    Anode: impure nickel Cathode: pure nickel
  • What is a reducing agent?
    A reducing agent is a substance that donates electrons and causes another substance to be reduced, while being oxidised itself.
  • What is an oxidising agent?
    A substance that causes oxidation by accepting electrons from another substance, however the oxdising substance itself is reduced.
  • What is the symbol reaction for the Haber process?
    N2 + 3H2 <=> 2NH3 (all gases)
  • Describe the Haber process
    The Haber process is the process in which ammonia is manufactured from hydrogen and nitrogen
  • What are the sources of nitrogen and hydrogen in the Haber process?
    Nitrogen: Air Hydrogen: Natural gas or methane
  • What are the conditions needed for the Haber process?
    Pressure of 200atm, temp of 450 degrees C and an iron catalyst.
  • What are the solubility rules of salts?
    Soluble salts can be made by reacting acids with soluble or insolbule reactants.
  • How are insoluble salts made?
    Precipitation reactions
  • How are soluble salts made?
    By reacting an acid with a base - titration
  • What is titration?
    Titration is a laboratory technique used to determine the concentration of a substance in a solution by reacting it with a known concentration of another substance.