What is the poh of a
2.6 x 10-6 m h+ solution?

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

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

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so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer