can get the answer for all these questions

1. Calculate the pH in a solution that is 0.98 M in NaC2H3O2 and0.56 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 Min NaOCl, what is the pH after 2.0 mL of 0.10 M NaOH has beenadded? (Ka for HOCl = 3.5  10–8)

3. The molar solubility of Mg3(PO4)2 is 6.26 x 10–6 M. Calculatethe 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 thetitrant. What is the pH of the acid solution at the equivalencepoint of titration? (if needed: Kw = 1.00 × 10–14)

5. You have two salts, AgX and AgY, with very similar Kspvalues. You know that Ka for HX is much greater than Ka for HY.Which salt is more soluble in acidic solution? (2pts) [MUST GIVESOME 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 in1.0 M HCl than in water? (2pts) (circle all that apply) [MUST GIVESOME 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) in1.0 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 0.010M Na3AsO4 is mixed with 0.20 mL of 0.010 M CoCl3, will aprecipitate form?

8. What is the maximum concentration of iodide ions that willprecipitate AgI but not PbI2 from a solution that is 6.7  10–3 Meach 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 toinitiate the precipitation of chromium(III) hydroxide from anequilibrium solution 0.050 M solution of CrBr3. Ksp = 3.0 x 10-29Kb = 1.8 x 10-5