Question

What is the pH of a solution of 20.00 mL of 3.00 M HCL that is titrated with 10.00 mL of a 6.00 M solution of NaOH ? (Note both acid and base are strong)

Answer 1

HCl + NaOH → NaCl + H2O Volume of acid HC1 = 20.00mL L = 20.00mL 1000 ml = 0.0200L Concentration of HCl = 3.00 M No of moles of HC1 = 0.0200 L *3.007 = 0.0600 mol Volume of NaOH added = 10.00 mL = 10.00mL L 1000mL =0.0100L Concentration of NaOH=6.00M No of moles of NaOH added =0.0100 x6.00 mor = 0.0600 mol No of moles of acid left out = (0.0600-0.0600) mol = 0.000mol Therefore, pH of the solution is 7.00