Given that pKb for iodate ion (IO-3) is 13.83, find the quotient [HIO3]/[IO-3] in a solution of sodium iodate at (a) pH 7.00; (b) pH 1.00.

1b) Suppose you decreased the pH of the biotin solution from 7.0 to 3.0 - what would happen to the ionizable group on a molecule of biotin as the pH shifted from 7.0 to 3.0? Briefly explain why you would expect that to happen

Dihydrogen phosphate, H₂PO₄⁻(aq), undergoes the following acid base equilibria in blood: H₂PO₄⁻(aq) ⇌ H⁺(aq) + HPO₄²⁻(aq)⇌ H⁺(aq) + PO₄³⁻(aq). The pKa values for the first and second steps are 7.2 and 12.4, respectively. The pH of human blood is 7.37 and this is tightly regulated. Which of the following statements most accurately describes the concentrations of the different species for the above reactions in blood. (Hint, think of the titration curves for H₂PO₄⁻(aq) and HPO₄²⁻(aq) and their respective pKa's.) A) [H₂PO₄⁻(aq)] is much greater than [HPO₄²⁻(aq)] and [PO₄³⁻(aq)] B) [HPO₄²⁻(aq)] is much greater than [H₂PO₄⁻(aq)] and [PO₄³⁻(aq)]. C) [H₂PO₄⁻(aq)] and [HPO₄²⁻(aq)] are both present and greater than [PO₄³⁻(aq)]. D) [PO₄³⁻(aq)] is much larger than the other concentrations, [H₂PO₄⁻(aq)] and [HPO₄²⁻(aq)]

What is the pK(b) of ClO₂⁻?(b) What is the pKₐ of the dimethylammonium ion, (CH₃)₂NH₂⁺?