Describe how the following reagents would be used to prepare barium sulphate:solid sodium sulphate, distilled water,barium carbonate and diluted nitric (5)acid.

Add dil HNO3 to the BaCO3 and allow to react completely. This releases CO2 from the BaCO3 and gives Ba^2+ in solution. Add Na2SO4, either by itself or as a solution, to form BaSO4. Filter. BaSO4 is retained in the filter. It can be dried following filtration.

Well, let me paint you a picture of this delightful process. Picture this: you have solid sodium sulphate, barium carbonate, distilled water, and diluted nitric acid. We're about to make some barium sulphate!

First things first, we take our solid sodium sulphate and dissolve it in the distilled water. Kind of like dissolving our problems away, you know? Now we have our sodium sulphate solution ready for action.

Next up, we take our barium carbonate and add it to our sodium sulphate solution. It's like a little chemistry party in there! The barium carbonate reacts with the sodium sulphate, resulting in the formation of barium sulphate and sodium carbonate.

But hold your horses, we're not done yet! Now it's time to filter out that precious barium sulphate from the mix. We use a filter paper to separate the solid barium sulphate from the sodium carbonate solution. It's like a magic trick, making the barium sulphate disappear!

Finally, to make sure our barium sulphate is all nice and shiny, we treat it with some diluted nitric acid. Kind of like giving it a little spa treatment, you know? The nitric acid washes away any impurities, leaving us with beautiful, pure barium sulphate.

And there you have it, a whimsical journey from solid sodium sulphate, distilled water, barium carbonate, and diluted nitric acid to the majestic creation of barium sulphate. Chemistry can be quite the circus act, don't you think?

To prepare barium sulphate, the following reagents would be used:

1. Solid sodium sulphate: Sodium sulphate (Na2SO4) is the source of sulphate ions (SO4^2-), which react with barium ions to form barium sulphate. It is added in solid form to the reaction mixture.

2. Distilled water: Distilled water is used as a solvent to dissolve the reagents and create a reaction mixture. It is free from impurities that could interfere with the reaction.

3. Barium carbonate: Barium carbonate (BaCO3) is the source of barium ions (Ba^2+), which react with sulphate ions to form barium sulphate. It is added to the reaction mixture in solid form.

4. Diluted nitric acid: Diluted nitric acid (HNO3) is used to provide an acidic environment for the reaction between barium carbonate and sodium sulphate. The acid reacts with the carbonate ions of barium carbonate, producing carbon dioxide gas (CO2), water (H2O), and barium nitrate (Ba(NO3)2). The barium nitrate then reacts with sulphate ions to form barium sulphate.

The step-by-step process to prepare barium sulphate using these reagents would be as follows:

1. Measure and weigh the required amount of solid sodium sulphate and barium carbonate.

2. Prepare a 1:1 molar ratio mixture of the solid sodium sulphate and barium carbonate in a suitable container.

3. Add distilled water to the container containing the mixture of solid reagents. The amount of water can vary depending on the desired concentration of the final solution.

4. Slowly add the diluted nitric acid to the mixture while stirring continuously. The acid reacts with the barium carbonate, producing carbon dioxide gas, water, and barium nitrate. The reaction is as follows:
BaCO3 + 2HNO3 -> CO2 + H2O + Ba(NO3)2

5. Allow the reaction mixture to settle for some time to ensure complete reaction and formation of barium nitrate.

6. Filter the mixture to separate the precipitate, which is the barium sulphate. Use a filter paper or an appropriate filtration setup to collect the solid.

7. Wash the collected precipitate with distilled water to remove any impurities or residual reagents.

8. Dry the barium sulphate by applying gentle heat or leaving it in an oven at a suitable temperature.

9. After the drying process, the barium sulphate is ready for further use or analysis.

It is important to note that handling chemicals and conducting reactions should be done following appropriate safety guidelines and by trained individuals.

To prepare barium sulfate using the given reagents, you would follow these steps:

1. Firstly, dissolve solid sodium sulfate (Na2SO4) in distilled water (H2O). Sodium sulfate is commonly available as a solid. Measure an appropriate amount of sodium sulfate, and dissolve it in distilled water in a suitable container. Stir or swirl the mixture until the sodium sulfate is fully dissolved.

2. Next, add barium carbonate (BaCO3) to the sodium sulfate solution. Barium carbonate is also commonly available as a solid. Measure the required amount of barium carbonate and add it to the sodium sulfate solution. Swirl or stir the mixture to ensure thorough mixing.

3. The reaction between sodium sulfate and barium carbonate will occur, leading to the formation of barium sulfate (BaSO4) as a precipitate. The balanced chemical equation for this reaction is:

Na2SO4 + BaCO3 → BaSO4 + Na2CO3

4. After the reaction is complete, you will observe a white precipitate of barium sulfate. This precipitate is insoluble in water and will appear as a solid substance in the solution.

5. Finally, you may choose to filter out the precipitate from the solution. This can be done using a filter paper or a suitable filtration apparatus. The solid barium sulfate can be collected on the filter paper, and the remaining solution that passes through the filter, containing sodium carbonate, can be discarded.

Note: Prior to performing this procedure, it's important to handle chemicals safely, use appropriate safety equipment (gloves, goggles), and conduct the experiment in a well-ventilated area. Also, it's advisable to follow any specific instructions provided by your educational institution or laboratory guidelines.

Please exercise caution while working with chemicals and always refer to official sources for safety guidelines and procedures.