When calcium chloride and ammonium phosphate are mixed, an insoluble precipitate of calcium phosphate forms and falls out of solution. After careful analysis of the purified precipitate, 8.16 * 10^25 atoms of calcium are found in the solid. How many other atoms are in the purified precipitate? (Note: the precipitate is only calcium phosphate)

The ppt is Ca3(PO4)2.

You have 8.16E25 atom Ca ions.
That's 8.16E25 x (1 mol/6.02E23) = ? mols Ca and divided by 3 = mols Ca3(PO4)2.
From there you know you have twice that mols P atoms (mols P x 6.02E23 = atoms P) and 8x that number of mols O atoms (atoms O = mols O x 6.02E23).

To determine the number of other atoms present in the purified precipitate of calcium phosphate, we need to determine the ratio of atoms between calcium and phosphate in calcium phosphate.

The formula for calcium phosphate is Ca3(PO4)2. This means that for every 3 calcium atoms, there are 2 phosphate ions.

Given that 8.16 * 10^25 atoms of calcium are found in the solid, we can calculate the number of phosphate ions by the following steps:

1. Determine the number of moles of calcium:
- Calculate the molar mass of calcium (Ca):
Molar mass of Ca = 40.08 g/mol
- Convert the given number of atoms to moles:
Moles of Ca = (8.16 * 10^25 atoms) / (6.022 * 10^23 atoms/mol)

2. Determine the number of moles of calcium phosphate:
- Using the ratio of calcium to phosphate ions, we know that for every 3 moles of calcium, there are 2 moles of phosphate ions.
- Moles of phosphate ions = (2/3) * Moles of Ca

3. Calculate the number of atoms of phosphate ions:
- Convert the moles of phosphate ions to atoms:
Number of atoms of phosphate ions = Moles of phosphate ions * (6.022 * 10^23 atoms/mol)

Therefore, by following these calculations, you can find the number of other atoms (phosphate ions) in the purified precipitate.

To find the number of other atoms in the purified precipitate, we need to first determine the chemical formula of calcium phosphate. Calcium phosphate is composed of one calcium ion (Ca2+) and two phosphate ions (PO43-).

Given that 8.16 * 10^25 atoms of calcium are found in the solid, we can assume that we have the same number of calcium ions. Since each calcium phosphate molecule contains one calcium ion, we can conclude that we have 8.16 * 10^25 calcium phosphate molecules.

To determine the number of phosphate ions, we need to consider the ratio between calcium and phosphate ions in calcium phosphate. The ratio is 1:2, meaning there are two phosphate ions for every calcium ion. Therefore, the total number of phosphate ions is twice the number of calcium ions.

Number of phosphate ions = 2 * (8.16 * 10^25) = 1.632 * 10^26

Now, to find the total number of atoms in the purified precipitate, we need to consider that each calcium phosphate molecule contains one calcium ion and two phosphate ions.

Total number of atoms = (number of calcium ions) + (number of phosphate ions) + (number of phosphate ions)
= (8.16 * 10^25) + (1.632 * 10^26) + (1.632 * 10^26)
= 8.16 * 10^25 + 3.264 * 10^26
= 4.08 * 10^26

Therefore, there are approximately 4.08 * 10^26 other atoms in the purified precipitate.