Respuesta :
The given question is incomplete. The complete question is:
A sample of household ammonia has a pH of 11.50. What is the hydronium ion concentration of this solution?
Answer: The hydronium ion concentration of the solution is [tex]1.58\times 10^{-12}M[/tex]
Explanation:
pH or pOH is the measure of acidity or alkalinity of a solution.
pH is calculated by taking negative logarithm of hydrogen ion concentration. Acids have pH ranging from 1 to 6.9 and bases have pH ranging from 7.1 to 14.
[tex]NH_3+H_2O\rightarrow NH_4^++OH^-[/tex]
[tex]pH=-\log [H^+][/tex]
[tex]11.8=-log [H^+][/tex]
[tex][H^+]=antilog(-11.8)[/tex]
[tex][H^+]=1.58\times 10^{-12}M[/tex]
Thus hydronium ion concentration of this solution is [tex]1.58\times 10^{-12}M[/tex]
Answer:
The concentration is 1.58*10^-12 M
Explanation:
Step 1: Data given pH of ammonia = 11.8
pH = -log[H+] = -log[H3O+]
Step 2: Calculate the concentration
2H20(l) ⇆ H3O+ + OH-
Kw = [H3O+][OH-]
-pKw = log[H3O+] + log[OH-] = log 10^-14
-14 = log[H3O+] + log [OH-]
14 = - log[H3O+] - log[OH-]
14 = pH + pOH
[H3O+] = 10^-11.8
[H3O+] = [H+] = 1.58 * 10^-12 M
The concentration is 1.58*10^-12 M
