Please be aware that this problem does not require a concentration to be given in the problem. We know the K_{sp} and we know the solution is saturated. This information will be sufficient.

Warning: you need to know about K_{sp} AND acid base ideas to do this problem type. If you lack one or the other of these skills, just be aware you just might struggle a little in your understanding of this problem type.

To solve the problem, we must first calculate the [OH¯]. To do this, we will use the K_{sp} expression and then, at the end, we will use acid base concepts to get the pH.

Final Note: K_{sp} are almost always given at 25.0 °C in reference sources. All problems in this tutorial are taken to be at 25.0 °C. If you were to see a problem where the specified temperature was different, it's probably just that the reference source gave a K_{sp} that, for whatever reason, was not at 25.0 °C.

**Example #1:** Calculate the pH of a saturated solution of AgOH, K_{sp} = 2.0 x 10¯^{8}

**Solution:**

AgOH ⇌ Ag^{+}+ OH¯K

_{sp}= [Ag^{+}] [OH¯]2.0 x 10¯

^{8}= (s) (s)s = 1.4 x 10¯

^{4}M (this is the [OH¯])pOH = −log [OH¯] = −log 1.4 x 10¯

^{4}= 3.85I actually took the negative log of 1.414 . . . x 10¯

^{4}; I did not use just 1.4Because pH + pOH = 14, we have pH = 14 − 3.85 = 10.15

**Example #2:** Calculate the pH of a saturated solution of Mg(OH)_{2}, K_{sp} = 5.61 x 10¯^{12}

**Solution:**

Mg(OH)_{2}⇌ Mg^{2+}+ 2 OH¯K

_{sp}= [Mg^{2+}] [OH¯]^{2}5.61 x 10¯

^{12}= (s) (2s)^{2}= 4s^{3}After dividing by 4 and then taking the cube root:

s = 1.12 x 10¯

^{4}MThis is an important point: what we have calculated is 's' and it is NOT the [OH¯]. That value is '2s.'

[OH¯] = 2.24 x 10¯

^{4}MpOH = −log 2.24 x 10¯

^{4}= 3.650pH = 14 − 3.650 = 10.350

**Example #3:** Calculate the pH of a saturated solution of Ba(OH)_{2}, K_{sp} = 5.0 x 10¯^{3}.

**Solution:**

5.0 x 10¯^{3}= (s) (2s)^{2}s = 0.10772 M

2s = [OH¯] = 0.21544 M

pOH = 10¯

^{0.21544}= 0.67pH = 14 − 0.67 = 13.33

**Example #4:** What is the pH in a saturated solution of Al(OH)_{3}? The K_{sp} of Al(OH)_{3} is 1.80 x 10¯^{33}. (By the way, there is quite a bit of variance in reported K_{sp} values for Al(OH)_{3}. I don't know why that should be so, but I felt it should be mentioned so you wouldn't feel it necessary to email me and tell me I'm using a wrong K_{sp} value.)

**Solution:**

1) Write the K_{sp} expression for Al(OH)_{3}:

K_{sp}= [Al^{3+}] [OH¯]^{3}

2) Solve the K_{sp} expression for the hydroxide concentration:

1.8 x 10¯^{33}= (s) (3s)^{3}s = 2.85744 x 10¯

^{9}M

3) Determine the pOH, then the pH:

pOH = −log 2.85744 x 10¯^{9}= 8.544pH = 14 − 8.544 = 5.456

4) THIS IS WRONG!! Notice that you added a base (Al(OH)_{3}) to the solution and you obtained an acidic pH. THIS CANNOT BE!!

5) The mistake is that, in this situation, we cannot ignore the hydroxide contribution from the water (which is 1.00 x 10¯^{7} M). Normally we can, but not in this instance. An approximate answer can be obtained by adding the two hydroxide contributions together:

1.00 x 10¯^{7}M + 2.85744 x 10¯^{9}M = 1.0285744 x 10¯^{7}M

6) Now, do the pOH and the pH:

pOH = −log 1.0285744 x 10¯^{7}= 6.988pH = 14 − 6.988 = 7.012

WHOOSH!! That was a close one!!

**Example #5:** Calculate the pH of a saturated solution of Cu(OH)_{2}, K_{sp} = 1.6 x 10¯^{19}

**Solution:**

1) Write the chemical equation:

Cu(OH)_{2}⇌ Cu^{2+}+ 2 OH¯

2) Write the K_{sp} expression:

K_{sp}= [Cu^{2+}] [OH¯]^{2}1.6 x 10¯

^{19}= (s) (2s)^{2}s = 3.42 x 10¯

^{7}M

3) This is an important point: what we have calculated is 's' and it is NOT the [OH¯]. The value we want is represented by '2s.'

[OH¯] = 6.84 x 10¯^{7}MpOH = −log 6.84 x 10¯

^{7}= 6.165pH = 14 − 6.165 = 7.835

4) The natural contribution of hydroxide from water molecules ionizing is 1.00 x 10¯^{7} M. What is the new pH if we take the hydroxide from water into consideration?

(6.84 x 10¯^{7}M) + (1.00 x 10¯^{7}M) = 7.84 x 10¯^{7}MpOH = −log 7.84 x 10¯

^{7}= 6.106pH = 14 − 6.016 = 7.894

5) Adding the two hydroxide amounts only gives a crude estimate. A truer picture would only arise with more complex calculations that are beyond the scope of this website.

The following three examples are all of the form X(OH)_{2}. These are the ones most commonly asked on tests and in worksheets. Calculate the pH of a saturated solution of:

**Example #6:** Ca(OH)_{2}, K_{sp} = 7.9 x 10¯^{6} (pH = 12.10)

**Example #7:** Mn(OH)_{2}, K_{sp} = 4.6 x 10¯^{14} (no answer provided)

**Example #8:** Ni(OH)_{2}, K_{sp} = 2.8 x 10¯^{16} (no answer provided)