Tell how to make a 1 M solution of Mg3(PO4)2 and a 0.1 M solution of CaSO4.
To make a 1 M solution of Mg3(PO4)2 and a 0.1 M solution of CaSO4, you will need the required amounts of each compound and a specified volume of solvent, usually water. Here's how you can calculate it:
1. Start with Mg3(PO4)2:
- Calculate the molar mass of Mg3(PO4)2:
- Mg (Magnesium): 24.31 g/mol
- P (Phosphorus): 30.97 g/mol
- O (Oxygen): 16.00 g/mol
- Multiply the atomic masses by the respective subscripts in the formula, and sum them up:
Molar mass = 3(24.31) + 2(30.97) + 8(16.00) g/mol
= 262.86 g/mol
- Calculate the mass of Mg3(PO4)2 required to prepare a 1 M solution:
- 1 M solution means 1 mole of the compound dissolved in 1 liter (1000 mL) of solvent.
- The mass needed can be calculated using the formula:
Mass (g) = Molarity (M) x Molar mass (g/mol) x Volume (L)
Since we want 1 M solution with 1 L of volume:
Mass (g) = 1 M x 262.86 g/mol x 1 L
= 262.86 g
- Measure 262.86 grams of Mg3(PO4)2 and dissolve it in 1 liter of solvent (water) to prepare a 1 M solution.
2. Moving on to CaSO4:
- Calculate the molar mass of CaSO4:
- Ca (Calcium): 40.08 g/mol
- S (Sulfur): 32.06 g/mol
- O (Oxygen): 16.00 g/mol
Molar mass = 40.08 + 32.06 + 4(16.00) g/mol
= 136.14 g/mol
- Calculate the mass of CaSO4 needed to prepare a 0.1 M solution:
- Similar to the Mg3(PO4)2 calculation:
Mass (g) = Molarity (M) x Molar mass (g/mol) x Volume (L)
Assuming you want a 0.1 M solution with 1 L of volume:
Mass (g) = 0.1 M x 136.14 g/mol x 1 L
= 13.614 g
- Measure 13.614 grams of CaSO4 and dissolve it in 1 liter of solvent (water) to prepare a 0.1 M solution.
Remember to accurately measure the mass of the compounds and dissolve them in the specified volume of solvent. Observe safety precautions while handling chemicals and follow appropriate lab procedures if you are in a laboratory setting.