Answer:
The answer is C) 0.0300 mol
Explanation:
First you need to get the total amount of moles is dissolved in the solution. This can be obtained doing the following:
Molarity = moles of solute / liters of solution
moles of solute = molarity x liters of solution
First, the volume has to be in liters, then :
100. ml x (1 L / 1000 mL) = 0.100 L
(We then substitute)
moles of solute = 0.100 mol/L x 0.1 L = 0.0100 mol of solute (In this case Na3PO4)
Having the moles of the solute, we now need to find how many moles of Na+ ions are there.
We need the conversion factor of 3 Na+ moles per 1 mole of Na3PO4
We then find the amount of moles doing as follows:
0.0100 mol Na3PO4 x (3 mol Na+ / 1 mol Na3PO4) = 0.0300 mol Na+.
The number of moles of [tex]Na^+[/tex] are 0.0300 and further calculation can be defined as follows:
Given that:
Molarity of [tex]Na_3PO_4[/tex] = 0.100 M
Volume of a solution = 100. mL
To find:
Moles of [tex]Na^+[/tex] ions
Formula used to calculate the number of moles when molarity is given is:
[tex]\text{Molarity of solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (mL)}}[/tex]
Put the values in the above formula:
[tex]0.100M=\frac{\text{Moles of }Na_3PO_4\times 1000}{100 mL}\\\\\text{Moles of }Na_3PO_4=\frac{0.100\times 100}{1000}\\\\\text{Moles of }Na_3PO_4=0.01 moles[/tex]
Since, 1 mole of [tex]Na_3PO_4[/tex] contains 3 moles of [tex]Na^+[/tex] and 1 mole of [tex]PO_4^{3-}[/tex] ions.
Moles of [tex]Na^+[/tex] ions = [tex](3\times 0.0100)=0.0300mol[/tex]
So, the required moles of [tex]Na^+[/tex] ions are 0.0300 moles.
Learn more about molarity: https://brainly.com/question/16587536
