A solution of an unknown hydrate of calcium chlorate ($Ca(CIO_3)_2$⋅n$H_2O$) is made by dissolving 4.164g in 150.0 cm33 of water. The resulting solution of calcium chlorate has a concentration of 0.1142 mol dm$^{−3}$
1.1.Determine the number of moles and the mass of calcium chlorate present in the solution.
2.Determine the mass of water and then the number of moles of water that was present in the hydrate used to make the original solution.
3.Determine the value of n in the hydrate formula,($Ca(CIO_3)_2$⋅n$H_2O$)
2.The calcium chlorate solution made above is then mixed with 200.0cm$^{3}$ of 0.07500 mol dm$^{−3}$ sodium phosphate ($Na_3PO_4 $), producing a precipitate of calcium phosphate, $Ca_3(PO_4)_2$
1.Write the net ionic equation for this reaction, including state symbols.
2.Determine the limiting reactant in this reaction, showing your work.
3.If 1.535g of calcium phosphate is recovered, determine the percent yield in this reaction.
4.Determine the concentration of phosphate ions remaining in the solution after removing the precipitate, assuming that is the only loss of phosphate ions.
