For a weak base (B), a 0.0100 M and a 0.100 M solution was made. Students...
For a weak base (B), a 0.0100 M and a 0.100 M solution was made. Students obtained the following pH value for the solution. Fill in the table. Report all answers (except pH or pOH values) in scientific notation.
|
0.0100 M B |
0.100 M B |
|
|
pOH |
4.32 |
3.48 |
|
[OH-] |
|
|
|
[BH+] |
|
|
|
[B] (at equilibrium) |
|
|
|
Kb |
|
|
For the same solution fill out the following information:
|
0.0100 M B |
0.100 M B |
|
|
pH (Do not use scientific notation for this answer) |
||
|
[H3O+] |
|
|
|
Ka |
|
|
Homework Answers
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For a weak base (B), a 0.0100 M and a 0.100 M solution was made.
Students...
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A 0.645 M solution of a weak base (B:) is made. The solution has a pH of 11.99. Calculate the Kb of this base. Report your answer in scientific notation with 3 sig figs.
A 0.771 M solution of a weak base (B:) is made. The solution has a pH...
A 0.771 M solution of a weak base (B:) is made. The solution has a pH of 11.35. Calculate the Kb of this base. Report your answer in scientific notation with 3 sig figs. Preview
(a) Determine the Kb of a weak base if a 0.847 M aqueous solution of the...
(a) Determine the Kb of a weak base if a 0.847 M aqueous solution of the base at 25°C has a pH of 10.88. (Enter your answer in scientific notation.) (b) Determine the concentration of a solution of ammonium chloride (NH4Cl) that has pH 5.19 at 25°C. (c) Calculate the pH of a 0.011 M NaF solution. (Ka for HF = 7.1 × 10−4.)
A 0.324 M solution of a weak base (B:) is made. The Kb for this acid...
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1. A 0.100 M solution of a weak acid has a pH of 1.96. Calculate the [H3O+] in the solution. 2. Suppose you have a 0.100 M solution of a weak acid that has a pH of 2.07. Calculate the Ka for this acid. *Report your answer to 2 significant figures.
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For a 0.0100 M solution of CH3COOH acid, ka = 1.75 x10-5 to 25 C) express:...
For a 0.0100 M solution of CH3COOH acid, ka = 1.75 x10-5 to 25 C) express: a) all the reactions that occur and their corresponding equilibrium constants. b) the expressions of mass balance and load balances of the system c) the concentration of H3O+ d) the pH of the system and the pOH e) the concentration of OH- of the system
If a buffer solution is 0.100 M in a weak base (Kb = 5.0 * 10%)...
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41.
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1) A 0.224 M solution of a weak acid (HA) is made. The Ka for this acid is 7.73 ⋅ 10-5 . -What is the pH of this solution? -What is the pOH of this solution? 2)A 0.238 M solution of a weak base (B:) is made. The Kb for this acid is 7.34⋅10-3. -What is the pOH of this solution? -What is the pH of this solution?
A 0.771 M solution of a weak base (B:) is made. The solution has a pH of 11.35. Calculate the Kb of this base. Report your answer in scientific notation with 3 sig figs. Preview
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41.
What is the pH of a 0.128 M solution of the weak base B if AH° = -28.0 kJ and AS° = -175 J/K for the following equilibrium reaction at 25°C? B(aq) + H2O(1) 5 BH(aq) + OH (aq) pH =
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