to complex ( K2[Cu(C2O4)2]H2O, add 1 com of dil. H2SO4. Add KI; then add 1-2cm3 choloform and shake gently. what are the observations.
What's 1 com?
What were your observations? All you gotta do is look, unless, of course, you're doing a dry lab.
To determine the observations of the given reaction, we can break down the steps and analyze the chemical reactions involved.
Step 1: Adding dilute sulfuric acid (H2SO4) to complex K2[Cu(C2O4)2]H2O:
The acid is likely to react with the complex, resulting in the release of carbon dioxide gas (CO2) and water (H2O). The reaction can be represented as follows:
K2[Cu(C2O4)2]H2O + H2SO4 → CO2 + H2O + K2SO4 + [Cu(H2O)n]
Observations for this step:
- Effervescence (bubbling) due to the release of carbon dioxide gas.
- Formation of a soluble compound, potassium sulfate (K2SO4), which remains in solution.
- Formation of a new copper complex, [Cu(H2O)n], which may cause a change in color or precipitation.
Step 2: Adding potassium iodide (KI):
When KI is added, a redox reaction occurs, resulting in the formation of iodine (I2) and potassium sulfate (K2SO4). The reaction can be represented as follows:
2KI + H2SO4 → I2 + K2SO4 + H2O
Observations for this step:
- The color change from transparent to brownish or yellowish due to the formation of iodine.
- Precipitation of solid particles of potassium sulfate, indicating that not all of it dissolves.
Step 3: Adding chloroform (CHCl3):
When chloroform is added and the mixture is gently shaken, it acts as an organic solvent that can dissolve nonpolar substances. However, chloroform is immiscible with water, so it will form two layers - an upper chloroform layer and a lower aqueous layer.
Observations for this step:
- Separation into two distinct layers: upper layer of chloroform and lower layer of water.
- Depending on the presence of other nonpolar substances, the chloroform layer may change color or remain transparent.
Overall observations:
- Effervescence (bubbling) in the first step due to the release of carbon dioxide gas.
- Color changes, such as the formation of a new copper complex or the brownish/yellowish color due to iodine formation.
- Formation of precipitates, such as potassium sulfate and potentially other insoluble compounds.
- Separation into two layers, chloroform and water, in the final step.
It is important to note that these observations are speculative and depend on the specific conditions and concentrations of the reactants.