An analytical chemist is titrating 109.3 ml. of a 0.8700M solution of butanoic acid (HC,H,CO,) with a 0.9500M solution of NaOH. The pK, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 36.93 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = 0

= 116.072 g/mol) is titrated with 0.284 M KOH. Calculate the pH A 100.0 mL solution containing 0.790 g of maleic acid (MW of the solution after the addition of 48.0 mL of the KOH solution. Maleic acid has pK, values of 1.92 and 6.27. pH = At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated as H,M, HM, and M²-, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively. [M²-| = TOOLS x10 [HM¯] = [H,M] II

An analytical chemist is titrating 83.7 mL of a 0.3300M solution of isopropylamine ((CH,) CHNH, with a 0.5300M 2 solution of HNO3. The p K, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 42.4 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = | ?

An analytical chemist is titrating 179.6 mL of a 0.8400M solution of cyanic acid (HCNO) with a 1.200M solution of KOH. The p K, of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 144.3 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = |