Answer:
mass of sodium phosphate required = 25.37 g
Explanation:
Equations of reactions:
3CaCl₂ + 2Na₃PO₄ ---> Ca₃(PO₄)₂ + 6NaCl
3Mg(NO₃)₂ + 2Na₃PO₄ ---> Mg₃(PO₄)₂ + 6NaNO₃
Number of moles of the ions = molarity x volume
Ca²⁺ : 0.052 M x 1.6 L = 0.0832 moles
Mg²⁺ : 0.093 x 1.6 L = 0.1488 moles
From the equations of reaction, number of moles of sodium phosphate required to react with each ion is given as;
For calcium: 2/3 x 0.0832 = 0.0555 moles
For magnesium: 2/3 x 0.1488 = 0.0992 moles
Total number of moles of sodium phosphate required = 0.0555 + 0.0992 = 0.1547 moles
Mass of sodium phosphate = number of moles x molar mass
molar mass of sodium phosphate = 164 g/mol
Mass of sodium phosphate = 0.1547 moles x 164 g/mol = 25.37 g
Therefore, mass of sodium phosphate required = 25.37 g
