Question

if 5.00ml of 1.25ml chloric acid is titrated with 0.095M sodium hydroxide, what a volume of base will be required to reach the equivalence point?

Answer 1

The formula of chloric acid is HClO₃

Number of moles of HClO₃ is , n = Molarity x volume in L

                                                = 1.25M x (5.00/1000) L

                                                = 0.00625 moles

The balanced equation between HClO₃ & NaOH is

HClO₃ + NaOH NaClO₃ + H2O

According to the balanced reaction ,

1 mole of HClO₃ reacts with 1 mole of NaOH for neutralization

0.00625 mole of HClO₃ reacts with 0.00625 mole of NaOH for neutralization

Given molarity of NaOH = 0.095 M

So volume of NaOH required , V = number of moles / Molarity

                                               = 0.00625 mol / 0.095 M

                                               = 0.0658 L

                                               = 0.0658 x 1000 mL         Since 1L = 1000 mL

                                               = 65.8 mL

Therefore the volume of NaOH required is 65.8 mL