Question

Titration of a strong acid with a strong base. The pH curve for titration of 50.0 mL of a 0.100 M solution of hydrochloric acid with a 0.100 M solution of NaOH (aq). For clarity, water molecules have been omitted from the molecular art.

Required:
What volume of NaOH(aq) would be needed to reach the equivalence point if the concentration of the added base were 0.270 M?

Answer 1

The volume of NaOH that would be needed to reach the equivalence point is :  19 mL

Given data

volume of HCL = 50 mL = 0.05 L

conc of HCL = 0.100 M

volume of NaOH = ?

conc of NaOH = 0.100 M

Determine the volume of NaOH needed to reach equivalence point

New conc of added base = 0.270 M

At equivalence ;

moles of OH⁻ ions = moles of H⁺ ions

              0.05 * 0.1 = 0.27 * v

therefore the volume ( v ) = ( 0.05 * 0.1 ) / 0.27

                                          = 0.019 L = 19 mL

Hence we can conclude that The volume of NaOH that would be needed to reach the equivalence point is :  19 mL .

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