Consider these two equilibrium processes.
(i) CaF2 (s) ↔ Ca2+ + 2 F− Kosp = 3.2 x 10−11
(ii) HF ↔ H+ + F− Koa = 6.8 x 10−4
(a) (0.6 pt) Use equations (i) and (ii), and their K’s to find Kooverall for this process:
(iii) CaF2 (s) + 2 H+ ↔ Ca2+ + 2 HF Keq = ??
(b) (0.6 pt) Find Ksp, conditional for reaction (iii) when the pH is such that the fraction of CHF that is F− is 0.25. (i.e., its alpha-function, a1, is 0.25)
(c) (0.6 pt) Calculate the pH at which a1 (fraction of F−) is 0.25.
Please explain!!
Consider these two equilibrium processes. (i) CaF2 (s) ↔ Ca2+ + 2 F−
When answering Parts a-h, consider only the molecules and ions,
Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq),
and Cr2O7^2-(aq), under standard state conditions. (1 pt each)
Use standard reduction table.
a) Which of these molecules and ions are oxidizing agents?
b) Which of these molecules and ions are reducing agents?
c) List the oxidizing agents from part a in DECREASING order of
oxidizing agent strength. (strongest OA to weakest OA)
d) List the reducing agents from part b in DECREASING order of...