Answer :
Answer:
1) [H3O+] = 2.24 *10^-5 M
2) [OH-] = 2.24 *10^-5 M
Explanation:
Step 1: Data given
pH + pOH = 14
pH = -log [H+]
Step 2:
What is the hydronium ion concentration in a solution of HCl that has a pH of 4.65?
pH = 4.65
-log [H+] = 4.65
[H+] = 10^-4.65 M
[H+] = 2.24 *10^-5 M
[H+] = [H3O+] = 2.24 *10^-5 M
Step 3:
What is the hydroxide ion concentration in a solution of NH3 with a pOH of 4.65?
pOH = 4.65
-log[OH-] = 4.65
[OH-] = 10^-4.65 M
[OH-] = 2.24 *10^-5 M
1) [tex][H_3O^+] = 2.24 *10^{-5} M[/tex]
2) [tex][OH^-] = 2.24 *10^{-5} M[/tex]
Given:
pH + pOH = 14
pH = -log [H+]
Calcluation for Hydronium ion concentration:
pH = 4.65
-log [H+] = 4.65
[H+] = [tex]10^{-4.65}[/tex] M
[H+] = [tex]2.24 *10^{-5}[/tex] M
[H+] = [H₃O+] = [tex]2.24 *10^{-5}[/tex] M
Calculation for hydroxide ion concentrartion:
pOH = 4.65
-log[OH-] = 4.65
[OH-] = [tex]10^{-4.65}[/tex] M
[OH-] = [tex]2.24 *10^{-5}[/tex] M
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