Question

I point

Given the ionization constant equation:
Kw = [H+][OH-]=1.0 x 10-14
For water at 25°C, which statement is true?
1) [H+] = [OH-]
2) [H+]> [OH-]
3) [H+] = 1.0 10-14 M
4) [OH-] = 1.0 × 10-14 M

Answer 1

The ionization constant equation is:

`K_(w)`=1.0 ×
`10^(-14)` at 25°C

the option is 1.

Step-by-step explanation:

Sometimes in pure water one proton of the water molecule(hydrogen ion) will get attracted to the lone pairs present in another water molecule.This causes the hydrogen ion to leave the present water(leaving the
`OH^(-)` behind) molecule ad gets attached to another water molecule leading to the formation of the hydronium ion(
`H^(3) O{+}`,hydronium ion).

This process is called auto-ionization of water because the water molecule ionizes into
`H^(+)` and
`OH^(-)` ions.

`H_(2)O`+
`H_(2) O`→
`H^(3) O{+}` +
`OH^(-)`

As such the equilibrium constant,which is measure of concentration of products to concentration of reactants,will be very slow.

∴the ionization constant of water at 25°C is 1.0 ×
`10^(-14)`.

(i.e.)option c is correct answer [
`H^(+)`]=[
`OH^(-)`]