A scientist wants to make a solution of tribasic sodium phosphate, , for a laboratory experiment. How many grams of will be needed to produce 350 of a solution that has a concentration of ions of 0.500 ?
You must provide dimensions with your numbers
procedure
To determine how many grams of tribasic sodium phosphate (Na3PO4) are needed to produce the desired concentration of ions in a 350 mL solution, we can follow a step-by-step approach:
1. Determine the molar mass of tribasic sodium phosphate (Na3PO4):
- The atomic mass of sodium (Na) = 22.99 g/mol
- The atomic mass of phosphorus (P) = 30.97 g/mol
- The atomic mass of oxygen (O) = 16.00 g/mol
- Calculate the molar mass of Na3PO4:
Molar mass (Na3PO4) = (3 * Na) + P + (4 * O)
= (3 * 22.99 g/mol) + 30.97 g/mol + (4 * 16.00 g/mol)
2. Calculate the molarity (M) of the solution using the given factors:
- Molarity (M) = moles of solute / volume of solution (in liters)
- Concentration of ions = 0.500 M
3. Convert the volume of the solution from milliliters to liters:
- Volume of solution = 350 mL รท 1000 mL/L
4. Rearrange the molarity formula to solve for moles of solute:
- Moles of solute = Molarity (M) * Volume of solution (L)
5. Finally, calculate the grams of tribasic sodium phosphate needed using the molar mass and moles of solute:
- Grams of Na3PO4 = Moles of solute * Molar mass (Na3PO4)
By plugging in the given values into these steps, you can find the answer.