100 grams of sodium phosphate contains how many sodium ions? what is the formula?
There are 3 Na^+ in a mole of Na3PO4.
moles in 100 g Na3PO4 = 100/molar mass Na3PO4.
There will be 3x that number of Na^+.
To determine the number of sodium ions in 100 grams of sodium phosphate and identify its formula, you need to follow a few steps.
Step 1: Find the molar mass of sodium phosphate.
The molar mass of sodium phosphate (Na3PO4) can be calculated by adding up the atomic masses of its constituent elements:
Sodium (Na) has an atomic mass of 22.99 g/mol.
Phosphorus (P) has an atomic mass of 30.97 g/mol.
Oxygen (O) has an atomic mass of 16.00 g/mol.
So, the molar mass of sodium phosphate (Na3PO4) is:
(3 * Na) + P + (4 * O) = (3 * 22.99) + 30.97 + (4 * 16.00) = 163.94 g/mol.
Step 2: Calculate the number of moles of sodium phosphate in 100 grams.
To convert the mass of sodium phosphate to moles, you divide the given mass by the molar mass:
Number of moles = Mass (g) / Molar mass (g/mol) = 100 g / 163.94 g/mol ≈ 0.609 mol.
Step 3: Determine the number of sodium ions in 0.609 moles of sodium phosphate.
Since each formula unit of sodium phosphate (Na3PO4) contains 3 sodium ions (Na), you can multiply the number of moles by 3:
Number of sodium ions = Number of moles of Na3PO4 * Number of sodium ions per formula unit = 0.609 mol * 3 = 1.827 mol.
Step 4: Convert the number of sodium ions from moles to particles.
Since 1 mole of a substance contains approximately 6.022 × 10^23 particles (Avogadro's number), you can multiply the number of moles by Avogadro's number to obtain the number of sodium ions:
Number of sodium ions = Number of moles of Na * Avogadro's number ≈ 1.827 mol * 6.022 × 10^23/mol = 1.099 × 10^24 sodium ions.
Therefore, 100 grams of sodium phosphate (Na3PO4) contains approximately 1.099 × 10^24 sodium ions.