30 ml of 0.3 M NaOH are required to titrate H3PO4 to the equivalence point.How many moles of H3PO4 are needed to reach the equivalence point. Show steps please :)
the balanced equation for the above reaction is as follows; 3NaOH + H₃PO₄ ---> Na₃PO₄ + 3H₂O stoichiometry of NaOH to H₃PO₄ is 3:1 the number of NaOH moles in the solution - molarity x volume number of NaOH moles - 0.3 mol/L x 0.030 L = 0.009 mol for complete neutralisation 3 mol of NaOH requires 1 mol of H₃PO₄ therefore 0.009 mol of NaOH requires - 1/3 x 0.009 = 0.003 mol of H₃PO₄ therefore 0.003 mol of H₃PO₄ are needed to reach the equivalence point
