Learning Goal: To calculate the pH at the equivalence point for various types of titrations. The equivalence point in an acid-base titration is the point at which stoichiometrically equivalent quantities of acid and base have been mixed together. At this point the reaction is complete because all analyte has been consumed by titrant. On a titration curve, the equivalence point is represented by the point of inflection (where the curve changes concavity). The figure (Eigure 1) shows the titration of 40.0 mL of 0.100 M HCl with 0.100 M NaOH. When 40.0 mL of the NaOH solution is added, the acid-base neutralization reaction is complete. When analyzing titrations involving weak acids or bases, consider how the neutralization reaction will impact the pH of the system. For example, when titrating a weak acid with a strong base, at the equivalence point all the base has been used to neutralize the acid forming its conjugate weak base. Figure E 14 12 10 8 6 4 2 0 0 Equivalence point 20.0 40.0 60.0 80.0 mL of 0.100 M NaOH added < 1 of 1 > ▾ Part B A 60.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 30.0 mL of KOH at 25 °C. Express the pH numerically. ▸ View Available Hint(s) pH = Submit Part C pH = Submit Consider the titration of 50.0 mL of 0.20 M NH3 (Kb-1.8 x 10) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 °C. Express the pH numerically. ▸ View Available Hint(s) ▾ Part D IVE ΑΣΦ pH = IVE ΑΣΦ 1 A C IL]ΑΣΦΗ ? A 30.0-mL volume of 0.50 M CH3COOH (Ka-1.8 x 105) was titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0 mL of NaOH at 25°C. Express the pH numerically. ▸ View Available Hint(s) ⒸIF ? C ?
Learning Goal: To calculate the pH at the equivalence point for various types of titrations. The equivalence point in an acid-base titration is the point at which stoichiometrically equivalent quantities of acid and base have been mixed together. At this point the reaction is complete because all analyte has been consumed by titrant. On a titration curve, the equivalence point is represented by the point of inflection (where the curve changes concavity). The figure (Eigure 1) shows the titration of 40.0 mL of 0.100 M HCl with 0.100 M NaOH. When 40.0 mL of the NaOH solution is added, the acid-base neutralization reaction is complete. When analyzing titrations involving weak acids or bases, consider how the neutralization reaction will impact the pH of the system. For example, when titrating a weak acid with a strong base, at the equivalence point all the base has been used to neutralize the acid forming its conjugate weak base. Figure E 14 12 10 8 6 4 2 0 0 Equivalence point 20.0 40.0 60.0 80.0 mL of 0.100 M NaOH added < 1 of 1 > ▾ Part B A 60.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 30.0 mL of KOH at 25 °C. Express the pH numerically. ▸ View Available Hint(s) pH = Submit Part C pH = Submit Consider the titration of 50.0 mL of 0.20 M NH3 (Kb-1.8 x 10) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 °C. Express the pH numerically. ▸ View Available Hint(s) ▾ Part D IVE ΑΣΦ pH = IVE ΑΣΦ 1 A C IL]ΑΣΦΗ ? A 30.0-mL volume of 0.50 M CH3COOH (Ka-1.8 x 105) was titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0 mL of NaOH at 25°C. Express the pH numerically. ▸ View Available Hint(s) ⒸIF ? C ?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 108QRT
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Question
![Learning Goal:
To calculate the pH at the equivalence point for various types of titrations.
The equivalence point in an acid-base titration is the point at which stoichiometrically equivalent
quantities of acid and base have been mixed together. At this point the reaction is complete because
all analyte has been consumed by titrant.
On a titration curve, the equivalence point is represented by the point of inflection (where the curve
changes concavity).
The figure (Figure 1) shows the titration of 40.0 mL of 0.100 M HCl with 0.100 M NaOH. When
40.0 mL of the NaOH solution is added, the acid-base neutralization reaction is complete.
When analyzing titrations involving weak acids or bases, consider how the neutralization reaction will
impact the pH of the system. For example, when titrating a weak acid with a strong base, at the
equivalence point all the base has been used to neutralize the acid forming its conjugate weak base
Figure
E
14
12
10
8
6
4
2
0
0
Equivalence point
20.0 40.0
mL of 0.100 M NaOH added.
60.0
80.0
< 1 of 1 >
Part B
A 60.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 30.0 mL of KOH at 25 °C.
Express the pH numerically.
▸ View Available Hint(s)
pH =
Submit
Part C
pH =
Submit
Consider the titration of 50.0 mL of 0.20 M NH3 (Kb-1.8 x 10) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 °C.
Express the pH numerically.
▸ View Available Hint(s)
▾ Part D
IVE]ΑΣΦ
pH =
IVE ΑΣΦ
1 A C
IΫΠΙΑΣΦΗ
?
A 30.0-mL volume of 0.50 M CH3COOH (K₂ -1.8 x 105) was titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0 mL of NaOH at 25°C.
Express the pH numerically.
▸ View Available Hint(s)
C
?
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Transcribed Image Text:Learning Goal:
To calculate the pH at the equivalence point for various types of titrations.
The equivalence point in an acid-base titration is the point at which stoichiometrically equivalent
quantities of acid and base have been mixed together. At this point the reaction is complete because
all analyte has been consumed by titrant.
On a titration curve, the equivalence point is represented by the point of inflection (where the curve
changes concavity).
The figure (Figure 1) shows the titration of 40.0 mL of 0.100 M HCl with 0.100 M NaOH. When
40.0 mL of the NaOH solution is added, the acid-base neutralization reaction is complete.
When analyzing titrations involving weak acids or bases, consider how the neutralization reaction will
impact the pH of the system. For example, when titrating a weak acid with a strong base, at the
equivalence point all the base has been used to neutralize the acid forming its conjugate weak base
Figure
E
14
12
10
8
6
4
2
0
0
Equivalence point
20.0 40.0
mL of 0.100 M NaOH added.
60.0
80.0
< 1 of 1 >
Part B
A 60.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 30.0 mL of KOH at 25 °C.
Express the pH numerically.
▸ View Available Hint(s)
pH =
Submit
Part C
pH =
Submit
Consider the titration of 50.0 mL of 0.20 M NH3 (Kb-1.8 x 10) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 °C.
Express the pH numerically.
▸ View Available Hint(s)
▾ Part D
IVE]ΑΣΦ
pH =
IVE ΑΣΦ
1 A C
IΫΠΙΑΣΦΗ
?
A 30.0-mL volume of 0.50 M CH3COOH (K₂ -1.8 x 105) was titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0 mL of NaOH at 25°C.
Express the pH numerically.
▸ View Available Hint(s)
C
?
?
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