1. what is the pH of the following solutions? Tell whether the solution is acidic, basic or neutral
(a) H3O+ = 1.0 x 10^-2 M
(b) OH- = 1.0 x 10^-4 M
(c) H3O+ = 1.0M
(d) OH- = 3.6 x 10^-9M
(e) OH- 7.8 x 10^-4 M
(f) H3O+ = 4.22 x 10^-4M
2. What is the H3O+ of the following? Tell whether the solution is acidic, basic or neutral
(a) pH = 9.0
(b) pOH = 9.0
(c) pH = 2.30
(d) pH = 8.90
3. A solution has pOH =4. What is the pOH of a solution that os 1,000 times more acidic? What is the pOH of the solution that is 100 times more basic.
4. What is the pH of a 0.0034 M solution of the strong base KOH?
5. A weak base is 5.0% ionized in solution. What is the pH of a 0.25 M solution of this base? (Assume on OH- per formula unit)
Any help and/or explanation would be truly appreciated. Thank you
(a) H3O+ = 1.0 x 10^-2 M
(b) OH- = 1.0 x 10^-4 M
(c) H3O+ = 1.0M
(d) OH- = 3.6 x 10^-9M
(e) OH- 7.8 x 10^-4 M
(f) H3O+ = 4.22 x 10^-4M
2. What is the H3O+ of the following? Tell whether the solution is acidic, basic or neutral
(a) pH = 9.0
(b) pOH = 9.0
(c) pH = 2.30
(d) pH = 8.90
3. A solution has pOH =4. What is the pOH of a solution that os 1,000 times more acidic? What is the pOH of the solution that is 100 times more basic.
4. What is the pH of a 0.0034 M solution of the strong base KOH?
5. A weak base is 5.0% ionized in solution. What is the pH of a 0.25 M solution of this base? (Assume on OH- per formula unit)
Any help and/or explanation would be truly appreciated. Thank you
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1. You can solve all of these by knowing three pieces of information:
a) pH = -log [H3O+]
b) pOH = -log [OH-]
c) pH + pOH = 14
You can directly find the pH when given the H3O+ concentration and you can find the pOH when given [OH-], which you can use to find the pH.
2. You can use the same three pieces of information to solve these problems:
a) pH = -log [H3O+]
b) pOH = -log [OH-]
c) pH + pOH = 14
First, convert all pOH values to pH values. Then, solve for [H3O+].
3. Remember that pOH = -log[OH-]. So, [OH-] = 10^-pOH. Think about what would happen if you decreased [OH-] by a factor of 10^3 or if you increased it by a factor of 10^2.
4. pOH = 14 - pH = - log [OH-] = -log [KOH] --> pH = 14 + log [KOH]
5. The weak base will reach an equilibrium concentration of .25 x .95 = .2375. This is the concentration of OH-. You can find the pOH and then find the pH.
Hope this helps
a) pH = -log [H3O+]
b) pOH = -log [OH-]
c) pH + pOH = 14
You can directly find the pH when given the H3O+ concentration and you can find the pOH when given [OH-], which you can use to find the pH.
2. You can use the same three pieces of information to solve these problems:
a) pH = -log [H3O+]
b) pOH = -log [OH-]
c) pH + pOH = 14
First, convert all pOH values to pH values. Then, solve for [H3O+].
3. Remember that pOH = -log[OH-]. So, [OH-] = 10^-pOH. Think about what would happen if you decreased [OH-] by a factor of 10^3 or if you increased it by a factor of 10^2.
4. pOH = 14 - pH = - log [OH-] = -log [KOH] --> pH = 14 + log [KOH]
5. The weak base will reach an equilibrium concentration of .25 x .95 = .2375. This is the concentration of OH-. You can find the pOH and then find the pH.
Hope this helps