General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.147QP
Related questions
Question
100%
ANSWER 16.11
![16.9
Which of the following solutions can act as a buffer?
(a) KCl/HCl, (b) KHSO4/H₂SO4, (c) Na₂HPO4/
NaH₂PO4, (d) KNO₂/HNO₂.
16.11 Calculate the pH of the buffer system made up of
0.15 M NH3/0.35 M NH4Cl.
16.13 The pH of a bicarbonate-carbonic acid buffer is
8.00. Calculate the ratio of the concentration of car-
bonic acid (H₂CO3) to that of the bicarbonate ion
(HCO3).
16.15 The pH of a sodium acetate-acetic acid buffer is
4.50. Calculate the ratio [CH3COOT]/[CH₂COOH].
16.17 Calculate the pH of the 0.20 M NH3/0.20 M NHẠCI
buffer. What is the pH of the buffer after the addi-
tion of 10.0 mL of 0.10 M HCl to 65.0 mL of the
buffer?
16.19 A diprotic acid, H₂A, has the following ionization
constants: K₁₁ = 1.1 × 10³ and K₁₂ = 2.5 × 10-6.
In order to make up a buffer solution of pH 5.80,
which combination would you choose? NaHA/H₂A
or Na₂A/NaHA.
16.45 Write balanced equations and solubility product ex-
pressions for the solubility equilibria of the follow-
ing compounds:
(d) Hg₂Cl₂,
(c) Ag₂CRO4,
(f) Mn3(PO4)2.
16.50 From the solubility data given, calculate the solubil-
ity products for the following compounds: (a) SrF2,
7.3 × 10-2 g/L, (b) Ag3PO4, 6.7 × 10¯³ g/L.
16.51 The molar solubility of MnCO3 is 4.2 × 10-6 M.
What is Ksp for this compound?
16.54 Using data from Table 16.2, calculate the molar sol-
ubility of CaF2.
16.57 If 20.0 mL of 0.10 M Ba(NO3)2 are added to 50.0 mL
of 0.10 M Na₂CO3, will BaCO3 precipitate?
16.58 A volume of 75 mL of 0.060 M NaF is mixed
with 25 mL of 0.15 M Sr(NO3)2. Calculate the
concentrations in the final solution of NO3, Na+,
Sr²+, and F¯. (Kp for SrF₂ = 2.0 × 10-¹⁰.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf556497-e613-4f4b-a188-280991ce40d5%2F9975e51b-115b-4718-a325-e039972e5311%2Fco4mk6m_processed.png&w=3840&q=75)
Transcribed Image Text:16.9
Which of the following solutions can act as a buffer?
(a) KCl/HCl, (b) KHSO4/H₂SO4, (c) Na₂HPO4/
NaH₂PO4, (d) KNO₂/HNO₂.
16.11 Calculate the pH of the buffer system made up of
0.15 M NH3/0.35 M NH4Cl.
16.13 The pH of a bicarbonate-carbonic acid buffer is
8.00. Calculate the ratio of the concentration of car-
bonic acid (H₂CO3) to that of the bicarbonate ion
(HCO3).
16.15 The pH of a sodium acetate-acetic acid buffer is
4.50. Calculate the ratio [CH3COOT]/[CH₂COOH].
16.17 Calculate the pH of the 0.20 M NH3/0.20 M NHẠCI
buffer. What is the pH of the buffer after the addi-
tion of 10.0 mL of 0.10 M HCl to 65.0 mL of the
buffer?
16.19 A diprotic acid, H₂A, has the following ionization
constants: K₁₁ = 1.1 × 10³ and K₁₂ = 2.5 × 10-6.
In order to make up a buffer solution of pH 5.80,
which combination would you choose? NaHA/H₂A
or Na₂A/NaHA.
16.45 Write balanced equations and solubility product ex-
pressions for the solubility equilibria of the follow-
ing compounds:
(d) Hg₂Cl₂,
(c) Ag₂CRO4,
(f) Mn3(PO4)2.
16.50 From the solubility data given, calculate the solubil-
ity products for the following compounds: (a) SrF2,
7.3 × 10-2 g/L, (b) Ag3PO4, 6.7 × 10¯³ g/L.
16.51 The molar solubility of MnCO3 is 4.2 × 10-6 M.
What is Ksp for this compound?
16.54 Using data from Table 16.2, calculate the molar sol-
ubility of CaF2.
16.57 If 20.0 mL of 0.10 M Ba(NO3)2 are added to 50.0 mL
of 0.10 M Na₂CO3, will BaCO3 precipitate?
16.58 A volume of 75 mL of 0.060 M NaF is mixed
with 25 mL of 0.15 M Sr(NO3)2. Calculate the
concentrations in the final solution of NO3, Na+,
Sr²+, and F¯. (Kp for SrF₂ = 2.0 × 10-¹⁰.)
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning