Question

1. What is the pH of a 0.000682 M solution of NaOH? 2. a)What is the kb for F- given that the ka for HF is 6.8*10-4 b)What is the pH of a 0.292 M solution of NaF? 3. What is the pH of a 0.03 M solution of CaO? HINT: CaO is ionic and dissociates into ions. What is the oxygen ion that results? What kind of an acid or base is it? You need to write out the acid/base reaction to get the stoichiometry right. pH = 4. (A)What is the pH of a 0.0124 M solution of HClO with ka = 3.0*10-8? (B)In part A you probably made the approximation that 0.0124 - x 0.0124. Check the approximation by calculating the % that x is of 0.0124. 5. The pH of a 0.0188 M solution of a certain weak acid is 4.14. What is the percent ionization of this acid? What is the Ka? 6. What is the pH of a 0.191 M solution of HN3 with ka = 1.9*10-5? 7. What is the pH of a 0.178 M solution of NaN3? HINT: To find kb use the ka in the last problem and read the note packet section on salts. Note: Don't confuse the weak base N3- with the strong base N3-. 8. What is the pH of a 0.1 M H2S solution with kA1 = 9.5*10-8 for the first proton and kA2 = 1*10-19 for the second proton. Read up on polyprotic acids in your note packet. 9. An aqueous solution of 0.062 M KCN is made. At equilibrium this solution will be acidic, basic, or neutral? Suppose you need to calculate the pH of an aqueous KCN solution. How many of these statements should you be thinking about in advance? The mass action equation will be set equal to Ka -log[x] = pOH not pH I need an ICE table and a Kb or Kw/Ka pH should be > 7 don't forget pH = 14 - pOH pH should be < 7 pH = -log[x] What is the pH of a 0.062 M KCN solution. The Ka for HCN is 8.0×10^-10

Answer 1