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On addition of the KI to your copper (II) solution, you formed Copper (I) iodine solid and produced the tri-iodide ion. It is the tri-iodide ion that you are titrating with the sodium thiosulfate. The tri-iodine ion is what itercalates into the starch molecules to form the dark blue color you are using as an end point in the titration. Some the the tri-iodide ion formed will adsorb to the surface of the solid copper (I) iodine formed. This must be desorbed for a complete titration. The addition of the potassium thiocyanate, displaces the adsorbed tri-iodine ion, and liberates it for titration.
Some of the metal ion that is estimated (especially Cu2+) may get trapped within starch indicator. When KCNS is added, copper thiocyanate or Cu(CNS)2 complex is formed which then reacts with the KI added, giving correct results.
It is simply because they could not be found together!! copper can be estimated by treating with potassium iodide and iodine will be liberated in the reaction which is titrated against sodium thiosulphate during the reaction we will add sulphuric acid to prevent the hydrolysis of copper sulphate and we follow by, adding ammonia to neutralize sulphuric as it may hinder the reation between iodide and copper!! now again we will add acetic acid to neutralize ammonia.. and the indicator is added at the last because it will get absorbed with the iodine!! now atlast we add ammonium, thiocyanate to prevent the excess of iodine getting added to copper iodide. end point is disappearance of blue color.
how the end point is determined
None. Anhydrous simply means ..... (not in solution). The opposite is aqueous (in solution).Added:..... crystalised without hydrate in the solid crystals.mono-hydrate means it is crystallised with 1 (one) molecule H2O per molecule salt.CuSO4.5H2O means : penta-hydrate of copper sulfate
On addition of the KI to your copper (II) solution, you formed Copper (I) iodine solid and produced the tri-iodide ion. It is the tri-iodide ion that you are titrating with the sodium thiosulfate. The tri-iodine ion is what itercalates into the starch molecules to form the dark blue color you are using as an end point in the titration. Some the the tri-iodide ion formed will adsorb to the surface of the solid copper (I) iodine formed. This must be desorbed for a complete titration. The addition of the potassium thiocyanate, displaces the adsorbed tri-iodine ion, and liberates it for titration.
copper (thiocyanate)2 and potassium nitrate
On addition of the KI to your copper (II) solution, you formed Copper (I) iodine solid and produced the tri-iodide ion. It is the tri-iodide ion that you are titrating with the sodium thiosulfate. The tri-iodine ion is what itercalates into the starch molecules to form the dark blue color you are using as an end point in the titration. Some the the tri-iodide ion formed will adsorb to the surface of the solid copper (I) iodine formed. This must be desorbed for a complete titration. The addition of the potassium thiocyanate, displaces the adsorbed tri-iodine ion, and liberates it for titration.
Cu2CuN2S2
Some of the metal ion that is estimated (especially Cu2+) may get trapped within starch indicator. When KCNS is added, copper thiocyanate or Cu(CNS)2 complex is formed which then reacts with the KI added, giving correct results.
Cu2I2 is precipitates in light pink colour due to adsorption of I2 and the precipitate releases I2 very slowly. Therefore very small amount of potassium thiocyanate is added towards the end point which helps to displace the adsorbed I2 quickly by combining with Cu2I2 to form CuSCN which has less tendency to adsorb I2.
It is simply because they could not be found together!! copper can be estimated by treating with potassium iodide and iodine will be liberated in the reaction which is titrated against sodium thiosulphate during the reaction we will add sulphuric acid to prevent the hydrolysis of copper sulphate and we follow by, adding ammonia to neutralize sulphuric as it may hinder the reation between iodide and copper!! now again we will add acetic acid to neutralize ammonia.. and the indicator is added at the last because it will get absorbed with the iodine!! now atlast we add ammonium, thiocyanate to prevent the excess of iodine getting added to copper iodide. end point is disappearance of blue color.
how the end point is determined
None. Anhydrous simply means ..... (not in solution). The opposite is aqueous (in solution).Added:..... crystalised without hydrate in the solid crystals.mono-hydrate means it is crystallised with 1 (one) molecule H2O per molecule salt.CuSO4.5H2O means : penta-hydrate of copper sulfate
analysis purpase
The end-point of the titration is more sharper if NH4CNS exist in the solution;
Prepare a sample of tetraamine copper (II) sulfate. (Despite the name it's very easy to produce). Analyze the percent by mass of copper ion, sulfate and ammonia in your compound. Very easy and impressive experiment if you have access to some standard lab equipment. Copper is analyzed by titration, sulfate is precipitated out with barium (II) chloride and measured using simple stoichiometry, ammonia is analyzed by back titration. Feel free to message me if you have any questions.