Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH, (aq) and 0.100 M in NH Cl(aq). Consult the table of ionization constants as needed. ApH = Calculate the change in pH when 7.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH = OCT 12 MacBook Pro Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: Unive LI A

A certain weak acid, HAHA, with a KaKaK_a value of 5.61×10−65.61×10−6, is titrated with NaOHNaOH. A solution is made by titrating 8.00 mmolmmol (millimoles) of HAHA and 1.00 mmolmmol of the strong base. What is the resulting pH?   More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 47.0 mL ?

Determine the pH at the equivalence point in titration of 25.0 mL of 0.690 M HCOOH with 0.18 M NaOH. The Ka of HCOOH is 1.8 × 10−4.HCOOH (aq) + NaOH (aq) → NaHCOO (aq) + H2O (l)