Express the ph to two decimal places answer correct

Express the pH to two decimal places.
ANSWER:
Correct
The buffer composed of 0.12 of propionic acid and 9.0 × 10
− 2
of its conjugate base, propionate, is made more basic through the addition of a
strong base, . Therefore, the values of the weak acid and its conjugate weak base should be adjusted accordingly. The appropriate
Henderson-Hasselbalch equation, using the amounts in moles, is
Part C
What is the of the buffer after the addition of 0.02 of ?
Express the pH to two decimal places.
ANSWER:
Correct
The buffer composed of 0.12 of propionic acid and 9.0 × 10
− 2
of its conjugate base, propionate, is made more acid through the addition of a
strong acid, . Therefore, the values of the weak acid and its conjugate weak base should be adjusted accordingly. The appropriate Henderson-
Hasselbalch equation, using the amounts in moles, is
Problem 17.24 Custom
A buffer is prepared by adding 11.0 of ammonium chloride to 230 of 1.00 solution.
Part A
pH
= 4.76
pH
mol mol pK
a
pH
pH
pH = p + log K
a
9.0 × mol 10
− 2
0.12mol
pH mol NaOH
= 4.93
pH
mol mol
NaOH
pH = 4.9 + log
9.0 × mol+0.02mol 10
− 2
0.12mol − 0.02mol
pH mol HI
= 4.59
pH
mol mol
HI
pH = 4.9 + log
9.0 × mol − 0.02mol 10
− 2
0.12mol+0.02mol
g (N Cl) H
4
mL MNH
3
pH

4/4/15, 12:51 PM Hw17-Chapter17
Page 9 of 32
What is the of this buffer?
ANSWER:
Correct
Part B
Write the net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer.
Express your answer as a chemical equation. Identify all of the phases in your answer.
ANSWER:
Correct
Part C
Write the net ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer.
Express your answer as a chemical equation. Identify all of the phases in your answer.
ANSWER:
Correct
± Titrations Custom
Learning Goal:
To learn about titration types and how to calculate at different points of titration.
In an acid-base titration, a titrant (solution of a base or acid) is added slowly to an analyte (solution of an acid or base). The titration is often monitored using a
meter. A plot of as a function of the volume of titrant added is called a titration curve .
Prior to the titration, the is determined by the concentration of the analyte. When the titrant is added, it begins to neutralize the analyte. The decrease in the
analyte concentration changes the . At the equivalence point , equivalent quantities of acid and base have been mixed together such that the acid-base
reaction is complete, and the is determined by the product. In the case of a strong acid-strong base titration, the salt formed is neutral, and . In a
weak acid-strong base titration, a basic salt is produced, and . In a weak base-strong acid titration, the salt is acidic, and . After the
equivalence point, the is determined by the concentration of excess titrant.