Acids, alkalis and salts

Neutral - green Acid - Red Alkali - Blue

Acid-Red Alkali - Blue

Acid - red Alkali - Yellow Neutral - Orange

Acid - colourless Alkali - pink

0-3 strongly acidic - hydrochloric acid 4-6 weakly acidic - vinegar 7 - neutral - water 8-10 weakly alkaline - ammonia solution 11-14 - strongly alkaline - sodium hydroxide solution

Yes, because it reacts in water to form carbonic acid

Soluble bases, as it needs to be dissolvable in water to be acidic/alkaline. These are also proton acceptors as they react with H+ to form H2O

Metal + acid -> salt + hydrogen Metal oxide + acid -> Salt + water Metal hydroxide + acid -> Salt + water Metal carbonate + acid -> Salt + water + carbon dioxide Ammonia + acid -> Salt (contains ammonium)

When bases, e.g. metal oxides react with acids which neutralises to form water. OH+H=H2O

When a neutralisation reaction occurs between bases and alkalis where the reactant’s volumes are measured

proton donors as they dissociate with a hydrogen ion which gives water a proton as H+ has just a proton

Proton acceptors as they react with H+ (a proton). e.g., hydroxide accepts H+ to form water

soluble bases that form OH- in water

Depending on the position in the reactivity series. The reaction is more vigorous up the series.

Strong acid Weak acid Nature Fully dissociated Partially dissociated Examples Hydrochloric acid Ethanoic acid Reaction with Mg Lots of bubbles, warm Some bubbles Reaction with carbonates Bubbles Fewer bubbles Colour of universal indicator with typical solution Red Orange -red

soluble salt from acid and alkali (titration) soluble salt from an acid and insoluble base/metal/carbonate (crystallisation) insoluble salt from two soluble salt (precipitation reaction)

• add excess solid to the acid (to neutralise all the acid) and stir • filter to remove excess solid when all acid has been neutralised • Heat pure salt solution to evaporate some of the solution which concentrates the solution until some crystals form • cool, leading to crystals forming (as at lower temperatures less solute can be dissolved in a solvent) and then filter to separate out the crystals • Dry salts in warm oven

• add 25cm^3 of alkali/acid to a conical flask using a volumetric pipette. Add 4 drops of indicator • use a burette to add acid/alkali till the first permanent colour change(swirl at the same time) • Repeat the titration 3 times doing it drop by drop when the end point is approaching • Do a titration without indicator adding the average volume of acid : alkali • Heat pure salt solution to evaporate some of the solution which concentrates the solution until some crystals form • cool, leading to crystals forming (as at lower temperatures less solute can be dissolved in a solvent) and then filter to separate out the crystals • Dry salts in warm oven

• combine equal quantities of two solutions and stir • filter out the salt crystals (residue) • wash crystals with pure distilled water • dry salt crystals in warm oven

grams that will dissolve in 100 grams of water at a specific temperature

moles = vol * conc

y axis - g/100 g of water x axis - temperature

• add indicator in conical flask, as well as 25cm^3 of alkali with volumetric pipette and add in acid using a burette • stop when colour change occurs (ideally name colour change) • start value - end value gets change in volume • do dropwise/swirling/repeating and using concordont results