Question

can get the answer for all these questions

1. Calculate the pH in a solution that is 0.98 M in NaC2H3O2 and 0.56 M in HC2H3O2. (Ka = 1.8 x 10–5)

2. Given 15.0 mL of a buffer that is 0.87 M in HOCl and 0.95 M in NaOCl, what is the pH after 2.0 mL of 0.10 M NaOH has been added? (Ka for HOCl = 3.5  10–8)

3. The molar solubility of Mg3(PO4)2 is 6.26 x 10–6 M. Calculate the value of Ksp for Mg3(PO4)2.

4. A 20.00-mL solution of 0.120 M nitrous acid (Ka = 4.0 × 10–4) is titrated with a 0.215 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution at the equivalence point of titration? (if needed: Kw = 1.00 × 10–14)

5. You have two salts, AgX and AgY, with very similar Ksp values. You know that Ka for HX is much greater than Ka for HY. Which salt is more soluble in acidic solution? (2pts) [MUST GIVE SOME EXPLAINATION OF ANSWER FOR CREDIT]

a) AgX

b) AgY

c) They are equally soluble in acidic solution.

d) Cannot be determined by the information given.

e) None of these (A-D).

6. Which of the following solid salts should be more soluble in 1.0 M HCl than in water? (2pts) (circle all that apply) [MUST GIVE SOME WORK/EXPLAINATION OF ANSWER FOR CREDIT] a) Na2CO3 b) KCl c) AgBr d) KNO3 e) RbF

9.What is the solubility (s) of Mg(OH)2 (Ksp = 8.9 x 10–12) in 1.0 L of a solution buffered (with large capacity) at pH 9.85

7. The Ksp for Co3(AsO4)2 is 6.8 x 10–29. When 0.20 mL of 0.010 M Na3AsO4 is mixed with 0.20 mL of 0.010 M CoCl3, will a precipitate form?

8. What is the maximum concentration of iodide ions that will precipitate AgI but not PbI2 from a solution that is 6.7  10–3 M each in Ag+ and Pb2+? For AgI, Ksp = 1.5 × 10–16 and for PbI2, Ksp = 1.4 × 10–8 .

10. Calculate the concentration of aqueous ammonia necessary to initiate the precipitation of chromium(III) hydroxide from an equilibrium solution 0.050 M solution of CrBr3. Ksp = 3.0 x 10-29 Kb = 1.8 x 10-5

Answer 1