Respuesta :
Answer: The correct answer is Option B.
Explanation:
To calculate the molarity of solution, we use the equation:
[tex]\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}[/tex] .......(1)
- For A:
Molarity of calcium phosphate solution = 0.100 M
Volume of solution = 2.00 L
Putting values in equation 1, we get:
[tex]0.100M=\frac{\text{Moles of }Ca_3(PO_4)_2}{2.00}\\\\\text{Moles of }Ca_3(PO_4)_2=(0.100mol/L\times 2.00L)=0.200mol[/tex]
Moles of calcium phosphate = 0.200 moles
- For B:
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 = [tex](8\times 0.200)=1.6[/tex] moles of oxygen atoms.
Moles of oxygen atoms = 1.6 moles
- For C:
Molarity of calcium phosphate solution = 0.100 M
Volume of solution = 1.00 L
Putting values in equation 1, we get:
[tex]0.100M=\frac{\text{Moles of }Ca_3(PO_4)_2}{1.00}\\\\\text{Moles of }Ca_3(PO_4)_2=(0.100mol/L\times 1.00L)=0.100mol[/tex]
Moles of calcium ions = [tex](0.100\times 3)=0.300[/tex] moles
- For D:
Molarity of calcium phosphate solution = 0.100 M
Volume of solution = 5.00 L
Putting values in equation 1, we get:
[tex]0.100M=\frac{\text{Moles of }Ca_3(PO_4)_2}{5.00}\\\\\text{Moles of }Ca_3(PO_4)_2=(0.100mol/L\times 5.00L)=0.500mol[/tex]
Moles of phosphorus atoms = [tex](0.500\times 2)=1.00[/tex] moles
According to mole concept:
1 mole of a compound contains [tex]6.022\times 10^{23}[/tex] number of atoms
Number of phosphorus atoms in 0.500 moles of calcium phosphate will be = [tex](1.00\times 6.022\times 10^{23})=6.022\times 10^{23}[/tex]
- For E:
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 = [tex](3\times 0.200)=0.600[/tex] moles of calcium ions
Moles of calcium ions = 0.600 moles
Hence, the correct answer is Option B.
