Question

Please help with this problem, Thanks!

HCI molar mass = 36.46 g/mol /// VU 1. If 25.88 ml of a 0.435 M HCl solution was titrated with 0.726 M NaOH solution, how much of NaOH would be required to reach the equivalence point? In addition, what would be the pH at the equivalence point? GRAA.435APHI

*Extra Info given:

NaOH molar mass= 40.00g/mol

HCl molar mass= 34.46g/mol

Answer 1

1)

a)

Balanced chemical equation is:

HCl + NaOH ---> NaCl + H2O

Here:

M(HCl)=0.435 M

M(NaOH)=0.726 M

V(HCl)=25.88 mL

According to balanced reaction:

1*number of mol of HCl =1*number of mol of NaOH

1*M(HCl)*V(HCl) =1*M(NaOH)*V(NaOH)

1*0.435 M *25.88 mL = 1*0.726M *V(NaOH)

V(NaOH) = 15.51 mL

Answer: 15.51 mL

b)

Since this is titration of strong acid and strong base, the pH at titration equivalence point should be 7.00

Answer: 7.00