Answer:
Explanation:
pH and pOH.....
The pH is a way of expressing the hydrogen ion concentration.
pH = -log[H+] ............. where [x] means "the concentration of x in moles per liter."
From pH you can compute pOH since at 25C pH + pOH = 14.00 .......... (but only at 25C)
pH = -log(2.6x10^-6) = 5.585 ..... which should be rounded to two significant digits: pH = 5.59
When taking the log of a number, only the digits to the right of the decimal reflect the precision in the original number. Since 2.6x10^-6 has two significant digits, a pH of 5.59 has two significant digits.
pOH + pH = 14.00
pOH = 14.00 - pH = 14.00 - 5.59 = 8.41 ......... at 25C
We can also use the H+ ion concentration to get the hydroxide ion concentration and from that the pOH.
Kw = [H+][OH-] = 1.00x10^-14 .......... at 25C .... like any Kc, the value changes with temperature
[OH-] = Kw / [H+] = 1.00x10^-14 / 2.6x10^-6 = 3.846x10^-9 .... to a couple of guard digits
pOH = -log[OH-] = -log(3.846x10^-9) = 8.415 ...... round to two significant digits: pOH = 8.42 ..... at 25C
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Just for grins, you might want to know how Kw changes with temperature, and how [H+] and [OH-] are related at some other temperatures. The pH is the pH of a neutral solution at various temperatures. For instance at 10C a neutral solution has a pH of 7.27. That's not a basic pH. 7.27 is the pH of a neutral solution, but at a different temperature. In a neutral solution at 10C [H+] = [OH-] = 5.41x10^-8M.
pH and Kw for a neutral solution at different temperatures
T .........pH ......... Kw
0......... 7.47....... 0.114 x 10-14
10....... 7.27....... 0.293 x 10-14
20....... 7.08....... 0.681 x 10-14
25....... 7.00....... 1.008 x 10-14
30....... 6.92....... 1.471 x 10-14
40....... 6.77....... 2.916 x 10-14
50....... 6.63....... 5.476 x 10-14
100..... 6.14....... 51.3 x 10-14
