Question

What is the ion-product constant, `K_w`?

Answer 1

For water, this is the measure of the `"autoprotolysis reaction"`....

Explanation:

`2H_2O(l) rightleftharpoonsH_3O^+ + HO^-`

And `K_w=[HO^-][H_3O^+]=10^-14` at `298*K`.

And when we take `-log_10` of both sides we get the useful expression...........

`pH+pOH=14`, where `pH=-log_10[H_3O^+]` etc.

How do you think `K_w` would develop if non-standard conditions pertained; e.g. if temperature was say `373*K`. Would `K_w` remain constant, decrease, increase? Remember that the autoprotolysis reaction as shown is a `"bond-breaking reaction"`.