RAG - Red

Salt + Hydrogen

Salt + Water

Salt + Water + Carbon Dioxide

Salt + Water

Magnesium Chloride + Hydrogen (salt + hydrogen)

Copper Sulfate + Water (salt + water)

Copper Chloride + Water + Carbon Dioxide (salt + water + carbon dioxide)

Sodium Nitrate + Water (salt + water)

• Use a measuring cylinder to add dilute hydrochloric acid to a beaker. • Dip a clean glass rod into the contents of the beaker. Use it to transfer a drop of liquid to a piece of universal indicator paper on a white tile. Wait for 30 seconds then match the colour to a pH colour chart and record the pH. • Add a level spatula of calcium hydroxide powder to the beaker. • Stir thoroughly, then estimate and record the pH. • Repeat this until there are no more changes in pH.

• Place the sulphuric acid in a conical flask and warm it in a warm water bath. • Add a spatula of copper oxide powder to the acid and stir with a glass rod. • Continue adding the copper oxide powder until it is in excess. • Filter the mixture to remove the excess copper oxide. • Pour the filtrate into an evaporating basin. • Heat the copper Sulfate solution to evaporate half the water. • Leave the solution by a window to allow all the water to evaporate.

• Use the pipette and pipette filler to add a measured volume of alkali to a clean conical flask. • Add a few drops of indicator and put the conical flask on a white tile. • Fill the burette with acid and note the starting volume. • Slowly add the acid from the burette to the alkali in the conical flask, swirling to mix. • Stop adding the acid when the end-point is reached (when the indicator first permanently changes colour). Note the final volume reading. • Repeat steps 1 to 5 until you get concordant titres. • More accurate results are obtained if acid is added drop by drop near to the end-point.

• to accurately measure the volume of a reactant before transferring it to a conical flask.

• to add small, measured volumes of one reactant to the other reactant.

Chloride salts

Nitrate salts

• Produces Sulfate salts

• Add some dilute hydrochloric acid to a beaker. • Add powdered insoluble reactant to some acid in a beaker, one spatula at a time, stirring to mix. The mixture will effervesce. Continue adding powder until some unreacted powder is left over - it is in excess. • Filter the mixture in the beaker to remove the excess powder. • Allow the water in the solution to evaporate (by heating and/or leaving for a few days) to obtain pure dry crystals of the salt.

• contains a relatively small amount of dissolved solute

• contains a relatively large amount of dissolved solute

• Strong acids completely dissociate into ions in solution. • For example, hydrochloric acid is a strong acid. • It completely dissociates to form hydrogen ions and chloride ions.

• Weak acids only partially dissociate into ions in solution. • For example, ethanoic acid is a weak acid. • It only partially dissociates to form hydrogen ions and ethanoate ions.

• Ionic compounds that are: • in the molten state (heated so they become liquids). Or • dissolved in water. • Under these conditions, the ions in electrolytes are free to move within the liquid or solution.

• a process in which electrical energy, from a direct current (dc) supply, decomposes electrolytes. • The free moving ions in electrolytes are attracted to the oppositely charged electrodes, which connect to the dc supply.

• Positively charged ions are called cations. • They move towards the negatively charged electrode, which is called the cathode.