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(3c) (i)Wear protective gear: Wear laboratory goggles, gloves, and a lab coat to protect yourself from skin and eye irritation and splashes. (ii)Handle chemicals with care: Handle the acid and sodium hydroxide solutions with care, as they can cause skin and eye irritation. Make sure to label the solutions correctly and store them in appropriate locations. (iii)Use the correct volume of indicator: Add the correct volume of methyl orange indicator to the acid solution, as excess indicator can affect the accuracy of the titration results.

(3a) (i)The salt solution was acidic in nature, as it reacted with sodium trioxocarbonate(IV) (sodium carbonate) to produce effervescence and a white precipitate. (ii)The salt solution contained a calcium or magnesium ion, as these ions form a white precipitate with sodium carbonate. (iii)The reaction was exothermic, as the test tube became warm, indicating the release of heat energy. (3b) (i) PbSO4 (lead(II) sulfate) would not readily dissolve in water, as it is insoluble in water. (ii) NaHCO3 (sodium hydrogen carbonate) produces effervescence with dilute mineral acids, as it reacts with acids to produce carbon dioxide gas. (iii) NH4Cl (ammonium chloride) decomposes on heating, as it breaks down into ammonia and hydrogen chloride gases. (iv) NaHCO3 (sodium hydrogen carbonate) dissolves in water to form an alkaline solution, as it is a basic salt. (v) NH4Cl (ammonium chloride) sublimes on heating, as it changes directly from a solid to a gas without going through the liquid phase.

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