0
[OH-] = 1x10^-3 M
[H+][OH-] = 1x10^-14
[H+] = 1x10^-14/1x10^-3 = 1x10^-11
pH = -log 1x10^-11 = 11
Done another way:
pOH = -log [OH-] = -log 1x10^-3 = 3
pH + pOH = 14
pH = 14 - 3 = 11
Wiki User
∙ 7y ago
Olabanji Muftau Akin...
Wiki User
∙ 11y agoThe pH of 1 M KOH is 13.0
The pH of 0,1 M KOH is 1,3
Wiki User
∙ 13y ago11 or 11.0 it doesnt matter both are right answers
Wiki User
∙ 13y ago14.
Calculus:
pOH = -log(conentration of OH-)= -log(1.0)= 0.0
pH = 14-pOH = 14 -0.0 = 14.0 (at 250C)
Wiki User
∙ 12y agopOH= -log[0,01]= 2 pH= 14-pOH= 14-2 = 12
Wiki User
∙ 14y agothe pH value is 13.
Wiki User
∙ 11y ago11
Wiki User
∙ 13y ago11
Add your answer:
Earn +20 pts
What is the pH of a 10-5 m of koh solution?
9
What is the PH of a 1.0x10 to the negative fourth power M solution of KOH?
-log(1.0 X 10^-4 M KOH) = 4 14 - 4 = 10 pH KOH ----------------
What is the pH of a 1 x 10-5 M KOH solution?
9
What has a pH of 13?
concentrated solution of NaOH and KOH have the pH value about 13.
What is the pH of a 0.04 M KOH solution?
0.04 M KOH produces an OH- concentration of 0.04 M. Thus, the pOH is -log 0.04 = 1.4 and the pH will be 14 - 1.4 = 12.6
What is the pH of a 10-5 m of koh solution?
9
What is the PH of a 1.0x10 to the negative fourth power M solution of KOH?
-log(1.0 X 10^-4 M KOH) = 4 14 - 4 = 10 pH KOH ----------------
What is the pH of a 1 x 10-5 M KOH solution?
9
When KOH is added to water what does the pH of the water solution do?
The pH of water increase.
What has a pH of 13?
concentrated solution of NaOH and KOH have the pH value about 13.
What is the pH of 3.5 x 10 -4 M solution of KOH?
-log(3.5 X 10^-4 M) = 3.4559 14 - 3.4559 = 10.5 pH
What is the pH of a 0.04 M KOH solution?
0.04 M KOH produces an OH- concentration of 0.04 M. Thus, the pOH is -log 0.04 = 1.4 and the pH will be 14 - 1.4 = 12.6
Does a strong alkali have a pH of 14?
Yes, a concentrated solution of NaOH and KOH may have pH=14
What solution has a greater concentration of hydrogen ions a solution with a pH of 3 of a pH of 5 Explain?
1/103 = 0.001 M ========( pH 3 ) 1/105 = 0.00001 M ============( pH 5 ) As you see, a pH of 3 has a 100 times concentration of 5 pH ( 10 * 10 devalued ) This is the scale; logarithmic.
Why pH electrode is dipped in saturated KOH solution?
You think probable to potassium chloride.
What is the H ion concentration in a 4.8x10-2 M KOH solution?
pOH = -log(10)[OH^-] pOH = -log(10) [ 48. x 10^-2] pOH = - (-1.31875...) pOH = 1.31875... pH = 14 - pOH pH = 14 - 1.31875... pH = 12.68124... pH = 12.68
What is the pH of 0.067 0 M KOH solution?
[H3O+]= Kw/[OH-] = 1.00*10-14/6.70*10-2 =1.49*10-13 MpH= -log [H3O+] = -log (1.49*10-13)=12.8
