Given pOH= 5.640
We know that pH+pOH=14
So pH = 14-pOH
= 14- 5.640
= 8.360
We know that pH= - log[H3O+]=8.360
[H3O+]=10^-8.360
= 4.37*10^-9 M
Therefore option C is correct.
What is the [H3O+] for a solution at 25°C that has pOH = 5.640? A. 2.34...
Question 6 Not yet answered Marked out of 1.00 Flag question What is the [H30*j for a solution at 25°C that has pOH = 5.640? Select one: -11 a. 4.27 x 10 M b. 8.360 M _9 c. 4.37 x 10 M -6 d. 2.29 x 10 M -4 e. 2.34 x 10 M
What is the (H30*) for a solution at 25°C that has pOH = 5.640? Multiple Choice points Зоо:41:46 О О 229 ~ 10-бм eBook О 4.27 = 10-1 м References О 8.360 м О О 4.37 10-9 м О 2.34 х 10-4 м
A) What is the pH for a solution at 25°C that has [OH-] = 1.9 x 10-10? B) What is the pOH for a solution at 25°C that has [H3O+] = 4.37 x 10-9?
A sodium hydroxide solution has a pOH of 9.8. What is the concentration of the H3O+ ions in this solution? a. 8.45 x 10^-11 mol/L b. 6.30 x 10^-11 mol/L c. 0 mol/L d. 1.58 x 10^-10 mol/L e. 1.85 x 10^-11 mol/L f. 9.8 mol/L g. 9.80 x 10^-11 mol/L h. 6.30 x 10^-5 mol/L (please show your work too)
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1.Calcuate the pH of a solution with [H3O+] = 6.54 x 10-3 M 2.Calcuate the pOH of a solution with [H3O+] = 8.5 x 10-9 M
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