Chemical test to distinguish between copper nitrate and lead nitrate
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A nitrate test is a chemical test used to determine the presence of nitrate ion in solution. Testing for the presence of nitrate via wet chemistry is generally difficult compared with testing for other anions, as almost all nitrates are soluble in water. In contrast, many common ions give insoluble salts, e.g. halides precipitate with silver, and sulphate precipitate with barium.
The nitrate anion is an oxidizer, and many tests for the nitrate anion are based on this property. Unfortunately, other oxidants present in the analyte may interfere and give erroneous results.
A common nitrate test, known as the brown ring test can be performed by addingiron(II) sulphate to a solution of a nitrate, then slowly adding concentrated sulphuric acidsuch that the acid forms a layer below the aqueous solution. A brown ring will form at the junction of the two layers, indicating the presence of the nitrate ion.Note that the presence of nitrite ions will interfere with this test.
The overall reaction is the reduction of the nitrate ion by iron(II) which is oxidised to iron(III) and formation of a nitrosonium complex where nitric oxide is reduced to NO−
2HNO3+ 3H2SO4 + 6FeSO4 --->> 3Fe2(SO4)3+ 2NO + 4H2O(Remaining)[Fe(H2O)6]SO4 + NO = [Fe(H2O)5(NO)]SO4+ H2O
This test is sensitive up to 2.5 micrograms and a concentration of 1 in 25,000 parts.
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The nitrate anion is an oxidizer, and many tests for the nitrate anion are based on this property. Unfortunately, other oxidants present in the analyte may interfere and give erroneous results.
A common nitrate test, known as the brown ring test can be performed by addingiron(II) sulphate to a solution of a nitrate, then slowly adding concentrated sulphuric acidsuch that the acid forms a layer below the aqueous solution. A brown ring will form at the junction of the two layers, indicating the presence of the nitrate ion.Note that the presence of nitrite ions will interfere with this test.
The overall reaction is the reduction of the nitrate ion by iron(II) which is oxidised to iron(III) and formation of a nitrosonium complex where nitric oxide is reduced to NO−
2HNO3+ 3H2SO4 + 6FeSO4 --->> 3Fe2(SO4)3+ 2NO + 4H2O(Remaining)[Fe(H2O)6]SO4 + NO = [Fe(H2O)5(NO)]SO4+ H2O
This test is sensitive up to 2.5 micrograms and a concentration of 1 in 25,000 parts.
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Answer: Add NH40H
Explanation:Copper---> Pale Blue ppt. insoluble in excess of NaOH
Lead---->White ppt. that dissolves in excess of NaOH forming colourless solution.
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