Analysis of Simple Salts - Chemistry Experiments

A colorless and odorless gas that turns lime water milky. It is released when a carbonate reacts with an acid.

A test used to identify the presence of carbonate ions (CO3^2-) in a sample. The sample is reacted with an acid, and the production of carbon dioxide gas is observed.

A reddish-brown gas that is produced when a nitrate reacts with concentrated sulfuric acid.

A test used to identify the presence of nitrate ions (NO3-) in a sample. The sample is reacted with concentrated sulfuric acid, and the production of nitrogen dioxide gas is observed.

A deep yellow precipitate that forms when a phosphate reacts with ammonium molybdate solution.

A test used to identify the presence of phosphate ions (PO4^3-) in a sample. The sample is reacted with nitric acid, and ammonium molybdate solution is added, resulting in a yellow precipitate if phosphate is present.

A white precipitate that is insoluble in dilute hydrochloric acid, formed when a barium chloride solution is added to a solution containing sulfate ions.

A test to identify the presence of sulfate ions (SO4^2-) in a sample: The addition of a barium chloride solution to the sample produces a white precipitate that is insoluble in dilute hydrochloric acid, indicating the presence of sulfate ions.

Adding neutral ferric chloride solution to a salt solution results in a deep red color, indicating the presence of acetate.

Heating a salt solution strongly in a dry test tube, resulting in the evolution of pleasant smelling, flammable vapors, confirms the presence of acetate.

Adding dilute nitric acid and silver nitrate solution to a salt solution forms a white curdy precipitate that dissolves in excess ammonium hydroxide, confirming the presence of chloride.

Adding lead nitrate solution to a salt solution forms a white precipitate soluble in hot water, confirming the presence of chloride.

Adding ferrous sulfate solution followed by concentrated sulfuric acid to a salt solution results in a brown ring at the interface, confirming the presence of nitrate.

Heating a salt solution with zinc dust and sodium hydroxide solution produces a smell of ammonia, confirming the presence of nitrate.

Adding lead acetate solution to a salt solution forms a white crystalline precipitate, confirming the presence of sulfate.

Adding ammonium acetate solution to the precipitate formed by adding lead acetate to a sulfate solution dissolves the precipitate, further confirming the presence of sulfate.

A chemical test used to confirm the presence of barium in a sample. It involves mixing the sample with concentrated hydrochloric acid, creating a paste, and introducing it into a Bunsen flame. A green colored flame indicates the presence of barium.

A chemical test to confirm the presence of calcium. The sample is mixed with concentrated hydrochloric acid to create a paste, which is then introduced into a Bunsen flame. A brick red flame indicates the presence of calcium.

A chemical test to confirm the presence of magnesium. The sample is mixed with Magneson reagent and excess sodium hydroxide solution, forming a blue precipitate. Alternatively, the sample is boiled with nitric acid and cobalt nitrate solution, and dipped onto filter paper, which is then burnt to ash, resulting in a pink ash.

A chemical test to confirm the presence of a specific chemical element in a sample, usually involving a color change, precipitate formation, or other observable phenomenon.

The process of determining the chemical composition of a substance, often involving multiple chemical tests to identify both the cation and anion present.

A blue precipitate forms when ammonium hydroxide is added drop by drop to a copper salt solution. This precipitate dissolves in excess ammonium hydroxide, resulting in a deep blue solution, confirming the presence of copper.

Adding acetic acid and potassium ferrocyanide to a copper salt solution produces a chocolate brown precipitate, providing another way to confirm the presence of copper.

Adding sodium hydroxide drop by drop to an aluminum salt solution leads to the formation of a white gelatinous precipitate. This precipitate dissolves in excess sodium hydroxide, confirming the presence of aluminium.

Heating an aluminium salt solution with concentrated nitric acid and cobalt nitrate, then burning a filter paper dipped in this solution results in a blue-tinted ash, providing an alternative confirmation for aluminium.

Adding potassium ferrocyanide to a zinc salt solution forms a white precipitate, confirming the presence of zinc.

Similar to the aluminium ash test, heating a zinc salt solution with nitric acid and cobalt nitrate, then burning a filter paper dipped in this solution produces a green-tinted ash, offering additional confirmation for zinc.

Adding sodium hydroxide in excess to a manganese salt solution creates a white precipitate, which turns brown upon standing, confirming the presence of manganese.

Heating a manganese salt with nitric acid and lead dioxide, then cooling and observing the solution reveals a pink supernatant if manganese is present. This is another way to confirm manganese.

A white gelatinous precipitate indicates the presence of aluminum in the solution. This test differentiates aluminum from other Group III cations.

If no precipitate forms after adding ammonium chloride and excess ammonium hydroxide, it suggests the absence of Group III cations.

A white precipitate indicates the presence of zinc in the solution, while a flesh-colored precipitate signifies manganese.

A white precipitate indicates the presence of barium or calcium in the solution. The test with ammonium carbonate solution is a good starting point for identifying these Group V cations.

If no precipitate forms after adding ammonium chloride, ammonium hydroxide, and excess ammonium carbonate solution, it indicates the absence of Group V cations.

The formation of a white crystalline precipitate, especially when the test tube is scratched, suggests the presence of magnesium. This test confirms the presence of magnesium in the group VI cations.

The evolution of a pungent, colorless gas that forms dense white fumes with concentrated hydrochloric acid confirms the presence of ammonium ions.

The formation of a yellow precipitate that dissolves in hot water and reappears as golden sparkles on cooling confirms the presence of lead.