A scientist wants to make a solution of tribasic sodium phosphate, Na3PO4, for a laboratory experiment….
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Question “A scientist wants to make a solution of tribasic sodium phosphate, Na3PO4, for a laboratory experiment….”
A scientist wants to make a solution of tribasic sodium
phosphate, Na3PO4, for a laboratory experiment. How many grams of
Na3PO4 will be needed to produce 750. mL of a solution that has a
concentration of Na+ ions of 1.00 M ?
Express your answer to three significant figures and include the
appropriate units.
Answer
Let’s do it!
[Na+] =1.00M
Volume of solution =750 mL = 0.750L
The given data can be used to calculate the moles of Na +ions.
Number of moles Na +ions = Molarity x Volum(L)
= 1.50M x 0.750L
Number of moles Na +ions = 0.75 Moles of Na + ions
Now; 1 mole Na 3PO 4 = 3 Moles of Na +ions
This is 0.75 moles Na+ions x (1 mole of Na3PO4/3moles Na+ions) = 0.25 Moles Na3PO4.
These moles of Na 3PO 4 can now be converted to grams
0.25 moles Na 3PO 4 x(163.94g/1mole), =40.9855 g Na 3PO 4
Thus, 41.0g OR40.9g Na 3PO 4 are required to make 750.0mL solution containing a concentration of Na + ion at 1.00M.
Conclusion
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