A scientist wants to make a solution of tribasic sodium phosphate, \rm Na_3PO_4, for a laboratory experiment. How many grams of \rm Na_3PO_4 will be needed to produce 575 mL of a solution that has a concentration of \rm Na^+ ions of 1.00 \it M?
see above.
To determine the number of grams of Na3PO4 needed to make the desired solution, you need to use the molar mass of Na3PO4 and the given concentration of Na+ ions.
Step 1: Calculate the molar mass of Na3PO4
Na = 22.99 g/mol (sodium)
P = 30.97 g/mol (phosphorus)
O = 16.00 g/mol (oxygen)
Molar mass of Na3PO4 = (3 * Na) + P + (4 * O)
Step 2: Convert the given volume to liters
Given: Volume = 575 mL
1 L = 1000 mL
Volume = 575 mL / 1000 mL/L
Step 3: Calculate the number of moles of Na+ ions
Given: Concentration = 1.00 M
Concentration = Moles / Volume (in liters)
Rearrange the formula to solve for moles:
Moles = Concentration * Volume
Step 4: Calculate the number of moles of Na3PO4 needed
Since Na+ and Na3PO4 have a 1:1 molar ratio, the number of moles of Na+ ions is equal to the number of moles of Na3PO4.
Step 5: Calculate the mass of Na3PO4
Mass = Moles * Molar mass
Let's calculate the number of grams of Na3PO4 needed:
1. Calculate the molar mass of Na3PO4:
Molar mass of Na3PO4 = (3 * 22.99 g/mol) + 30.97 g/mol + (4 * 16.00 g/mol)
Molar mass of Na3PO4 = 163.94 g/mol
2. Convert the given volume to liters:
Volume = 575 mL / 1000 mL/L
Volume = 0.575 L
3. Calculate the number of moles of Na+ ions:
Moles = Concentration * Volume
Moles = 1.00 mol/L * 0.575 L
Moles = 0.575 mol
4. Calculate the number of moles of Na3PO4 needed:
Since Na+ and Na3PO4 have a 1:1 molar ratio, the number of moles of Na+ ions is equal to the number of moles of Na3PO4.
Moles of Na3PO4 = 0.575 mol
5. Calculate the mass of Na3PO4:
Mass = Moles * Molar mass
Mass = 0.575 mol * 163.94 g/mol
Mass = 93.97 g
Therefore, approximately 93.97 grams of Na3PO4 will be needed to produce 575 mL of a solution with a concentration of Na+ ions of 1.00 M.