Question

The Kw of water varies with temperature. Calculate the pH of water at 46⁰C with a Kw = 3.219 x 10-14. Show all calculations leading to an answer
can someone help me with 1 question im trying to finish up and been on it for a while and getting nowhere and would appreciate it
its chem :)

Answer 1

The Kw of water varies with temperature. Calculate the pH of water at 46⁰C with a Kw = 3.219 x 10-14. Show all calculations leading to an answer

Answer 2

the KW of water is its equilibrium constant, yes?

and the equilibrium constant is always found the same way. When water dissociates, \[H_2O(l) \rightarrow H^{+1} + OH^{-1}\]

Answer 3

whenever water dissociates, the number of \(H^{+1}\) ions formed and the number of \(OH^{-1}\) ions formed will ALWAYS be equal.

Answer 4

the equilibrium constant is always set up the same way:\[K_W = [H^{+1}]*[OH^{-1}]\]and in this case will be equal to \(3.22*10^{-14}\)

Answer 5

you don't know what the ion concentrations are, but we know that they are EQUAL\[K_W = [H^{+1}]*[OH^{-1}] = [x]*[x] = 3.22*10^{-14}\]