Which one of the following statements is not true concerning 2.00 l of a 0.100 m solution of ca3(po4)2?

(a) this solution contains 0.200 mol of ca3(po4)2.
(b) this solution contains 0.800 mol of oxygen atoms.
(c) 1.00 l of this solution is required to furnish 0.300 mol of ca2+ ions.
(d) there are 6.022 × 1023 phosphorus atoms in 5.0 l of this solution.
(e) this solution contains 0.600 mol of ca2+ ions.

The correct answer is Option B.

Explanation:

To calculate the molarity of solution, we use the equation:

    .......(1)

Molarity of calcium phosphate solution = 0.100 M

Volume of solution = 2.00 L

Putting values in equation 1, we get:

Moles of calcium phosphate = 0.200 moles

1 mole of calcium phosphate contains 3 moles of calcium atoms, 2 moles of phosphate atoms and 8 moles of oxygen atoms.

So, 0.200 moles of calcium phosphate will contain = moles of oxygen atoms.

Moles of oxygen atoms = 1.6 moles

Molarity of calcium phosphate solution = 0.100 M

Volume of solution = 1.00 L

Putting values in equation 1, we get:

Moles of calcium ions = moles

Molarity of calcium phosphate solution = 0.100 M

Volume of solution = 5.00 L

Putting values in equation 1, we get:

Moles of phosphorus atoms = moles

According to mole concept:

1 mole of a compound contains number of atoms

Number of phosphorus atoms in 0.500 moles of calcium phosphate will be =

1 mole of calcium phosphate contains 3 moles of calcium ions and 2 moles of phosphate ions.

So, 0.200 moles of calcium phosphate will contain = moles of calcium ions

Moles of calcium ions = 0.600 moles

Hence, the correct answer is Option B.

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