On the weak base/strong acid titration curve, label A. the point where the pH corresponds to a solution of the weak base (B) in water; B. the point where the pH corresponds to a solution of the conjugate acid (BH+) in water; C. the point where pH = pK for BH+. Answer Bank C A B 7- Hd

Consider the titration of 30.0 mL of 0.263 M weak base B (Kb = 1.3 x 10 10) with 0.150 M HI. How many mL of the HI would be required to reach the halfway point?

A titration of 200.0 mL of 2.55 MH 2A was done with 1.00 M NaOH. For the diprotic acid H 2A, Ka1 =2.5 x 10-5, Ka2=3.1 x 109. Calculate the pH before any 1.00 M NaOH has been added. Oa. 11.83 Ob.8.68 O c. 9.66 Od.2.17 Oe. 4.20

ETUSTUOto 3JAT 0 520 | CHAPTER 14 Acids and Bases 49. A 25.00-mL sample of an H₂SO4 solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 41.22 mL of KOH is required to reach the equivalence point. What is the concentration of the un- known H₂SO4 solution? 52 51. What volume in milliliters of a 0.121 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 10.0-mL sample of 0.102 M sulfuric acid? NG AND WEAK ACIDS AND BASES assify each acid as strong or weak. HCI HF Br 2SO3 50. 52 5

a. What was the concentration of the NaOH? Concentration = м b. What is the pH at the equivalence point? рн - c. Which indicator, bromothymol blue, phenolpl

For each of the series of electron-pushing arrows, please draw the respective products. Also, indicate if each reaction is an example of initiation, propagation, or termination.

What is the pH after 8.0 mL of 0.10 M HCl is added to 20.0 mL of 0.10 M NH3? (Kb=1.8 x 10-5)