0
-log(3.5 X 10^-4 M)
= 3.4559
14 - 3.4559
= 10.5 pH
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What is the pH of a solution that has hydrogen equals 2.3 x 10-4?
Molarity of hydrogen solution equals 2.3 X 10^-4 -log(2.3 X 10^-4) = 3.6 pH
A water solution whose pH is 10?
Is always basic.
What is the pH of a solution with a H plus equals 10 -8?
2
What is the pH of a solution with H plus equals 2.3 10-12?
- log(2.3 X 10 -12 ) = 11.6 pH -----------------very little H + concentration in this solution.
What is the pH of a solution with H plus equals 9.40 x 10-4?
-log(9.40 X 10^-4) = 3 pH
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 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
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
If a solution has a pH of 10 that solution is?
...that solution is alkaline or basic.
If a solution has a hydrogen ion concentration of 10-5M what is its pH?
The pH of a solution is defined as -log10[H+]. Thus a solution with a hydrogen ion concentration of 10-5M has a pH of 5. [H+] = 10-5 pH = -log[H+] pH = - log [10-5] pH = 5
