Calculate the pH of the following salt solutions?
0.1 M HBr
0.1 M CaI2
0.1 BaF2 Kb (F-)=1.4x10^-11
What do you not understand about these problems. I can't spend all night typing these in detail.
HBr is a strong acid, it ionizes completely, so the pH should be obvious.
CaI2 is a salt that doesn't hydrolyze. Again obvious.
I think there may be a problem with the problem. BaF2 isn't soluble in water, although since it gives a Kb I suppose we could go through the motions.
i don't understand how to get CaI2
The pH is 7.00
CaI2 is a soluble salt.
It is the salt of a strong base (Ca(OH)2) and a strong acid (HI); therefore, neither the cation nor the anion will hydrolyze with water (that is to say H2O is too strong a base to let the H go to I and it is too strong an acid to let the OH go to Ca. So it's just like a solution of NaCl. Neither ion hydrolyzes and the net effect in solution is you have the ionization of H2O and you know that is a pH of 7
(H^+)(OH^-) = 1 x 10^-14
Solve for (H^+).