Soluble Salts (GCSE Chemistry)

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

When preparing a soluble salt by reacting an insoluble metal oxide with acid, why is it common to add the metal oxide until it is in excess before filtering?

Which statement about the solubility of salts is correct?

Which of these describes the correct sequence of steps to obtain dried crystals from a clear salt solution?

Which of the following is a safe practice when preparing and heating solutions to crystallise salts?

A teacher asks which of these salts is soluble in water at room temperature. Which is correct?

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?

Which of the following is the best reason crystals are washed with a small amount of cold solvent (usually cold distilled water) after filtration?

Which method is best for preparing pure crystals of a soluble salt such as sodium sulfate from its aqueous solution?

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

Why is a water bath preferred over direct flame when gently heating a filtrate to form crystals?