What is name of reagent containing 0.6 M Sulphuric acid, 28 mM sodium phosphate, and 4 mM ammonium molybdate? and in which amount it should be taken to make a reagent?

The name of the reagent you described is not provided. However, to make this reagent, you would need to follow these steps:

Step 1: Calculate the amount of each component required:
- For 0.6 M Sulphuric acid: Determine the volume needed based on the desired final volume of the reagent.
- For 28 mM sodium phosphate: Determine the mass or volume of sodium phosphate needed based on the molarity and desired final volume.
- For 4 mM ammonium molybdate: Determine the mass or volume of ammonium molybdate needed based on the molarity and desired final volume.

Step 2: Prepare the reagent by combining the calculated amounts of each component in a suitable container.

Note: It is important to wear appropriate safety equipment and follow proper handling procedures when working with reagents such as Sulphuric acid.

To determine the name and amount of the reagent, we need to calculate its composition. The composition is given as a concentration of each component: 0.6 M Sulphuric acid, 28 mM sodium phosphate, and 4 mM ammonium molybdate.

The name of the reagent will depend on its purpose or the specific chemical reaction it is used in. Without further context, we cannot provide an exact name for the reagent. However, based on the components provided, it appears to be a reagent commonly used in analytical chemistry for phosphate determination, called the molybdenum blue method. This method is used to detect and quantify phosphates in various materials.

To calculate the amount of each component needed to prepare the reagent, you should consider the desired final volume of the reagent. Let's assume you want to prepare 500 mL of the reagent.

First, we need to convert the concentrations into moles per liter (M) for sulphuric acid and millimoles per liter (mM) for sodium phosphate and ammonium molybdate.

- 0.6 M Sulphuric acid: This means there are 0.6 moles of sulphuric acid per liter. For a 500 mL reagent, you will need 0.6 x 0.5 = 0.3 moles of sulphuric acid.
- 28 mM Sodium phosphate: This means there are 0.028 moles of sodium phosphate per liter. For a 500 mL reagent, you will need 0.028 x 0.5 = 0.014 moles of sodium phosphate.
- 4 mM Ammonium molybdate: This means there are 0.004 moles of ammonium molybdate per liter. For a 500 mL reagent, you will need 0.004 x 0.5 = 0.002 moles of ammonium molybdate.

To calculate the mass of each component needed, you will also require the molar masses of each substance:
- Sulphuric acid (H2SO4): 98.09 g/mol
- Sodium phosphate (Na3PO4): 163.94 g/mol
- Ammonium molybdate [(NH4)6Mo7O24·4H2O]: 1235.94 g/mol

The mass of each component can then be calculated using the equation:

Mass (g) = Moles x Molar Mass

For example, to calculate the mass of sulphuric acid needed:

Mass of sulphuric acid = 0.3 moles x 98.09 g/mol = 29.43 g

Similarly, you can calculate the masses of sodium phosphate and ammonium molybdate using their respective moles and molar masses.

Please note that this calculation assumes you are starting with concentrated forms of these chemicals. If you have different starting concentrations or the reagents are already in a different form (such as solutions or powders), the calculations may vary.

Remember to handle reagents carefully and follow proper safety protocols when working with chemicals.