show work please
3. What is the [H3O'] of a solution having a pH of 3.4? (Answer: 4 x 10-M)
a) Calcuate the pH of a solution with [H3O+] = 6.54 x 10-3 M b) Calcuate the pOH of a solution with [H3O+] = 8.5 x 10-9 M c) A solution has a pH = 2.420, what is the [OH-]? d) A solution has a pOH = 1.0, what is the [OH-]? e) Calcuate the pH of a solution with [OH-] = 5.9 x 10-6 M
If the pH of the solution is 2.6, what is the [H3O+]?
If the pH of the solution is 2.6, what is the [OH?]?
If the [H3O+] in a solution is 2×10?5M, what is the [OH?]?
If the [H3O+] in a solution is 2×10?5M, what is the pH of the
solution?
If the [H3O+] in a solution is 1×10?12M, what is the [OH?]?
If the [H3O+] in a solution is 1×10?12M, what is the pH of the
solution?
If the...
What is the pH of a solution with {H3O+] = 2 x 10^-5 M and is it an acidic or basic solution? NOTE: {2 x 10^-5} is the number 0.00002 written in scientific notation as much as possible with D2L.
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
Calculate the pH of a solution which has [H3O+] = 3.7 x 10-3 Type youf answer...
Calculate the pH of a solution which has [H3O+] = 8.0 x 10-12 .
QUESTION 3 Calculate the pH of solution that has an H30+ ion concentration of 3.4 x 10-9 M. 7.0 3.4 09 8.47 -8.47
A solution has [OH-] = 4.33 x 10-5 M. Calculate [H3O+] and pH of the solution. Then, tell whether the solution is acidic, basic, or neutral. Also, calculate pOH.
1.) If the Kb of a weak base is 3.4 x 10^-6, what is the pH of a 0.11M solution of this base? 2.) A certain weak base has a Kb of 7.00 x 10^-7. What concentration of this base will produce a pH of 10.16?