Soluble Salts (GCSE Chemistry)

Why is it important to repeat an experiment and take a mean when preparing a soluble salt or measuring yield?

When making zinc sulfate by reacting zinc metal with sulfuric acid, which observation indicates hydrogen gas is being produced?

What is the main reason for filtering a reaction mixture when preparing a soluble salt from an insoluble base and acid?

When carrying out a titration to make a pure salt solution, which indicator colour change is commonly used for strong acid vs strong base titrations?

Why is excess insoluble base used rather than excess acid when making a soluble salt by reacting an acid with an insoluble base?

Why is it better to crystallise a salt from a warm concentrated solution rather than evaporating to dryness?

A student makes a soluble salt by reacting a soluble base with an acid and obtains a cloudy filtrate due to an impurity. Which step should be added to purify the salt solution before crystallisation?

When preparing sodium chloride crystals by evaporating seawater, which step produces the pure crystalline salt?

Which of the following is the correct ionic equation for the reaction between zinc and hydrochloric acid that produces zinc chloride and hydrogen?

A student obtains a maximum theoretical mass of salt of 12.5 g but actually produces 11.6 g. What is the percentage yield (to one decimal place)?

If 25.0 cm3 of a salt solution contains 0.500 g of dissolved salt, what is the concentration in g/dm3?