Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.)
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