For conjugate acid–base pairs, how are K a and K b related? Consider the reaction of acetic acid in water CH 3 CO 2 H ( a q ) + H 2 O ( l ) ⇌ CH 3 CO 2 − ( a q ) + H 3 O + ( a q ) where K a = 1.8 × 10 −5 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH 3 CO 2 − ) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH 3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming K a for a monoprotic strong acid is 1 × 10 6 , calculate K b for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li + , K + , Rb + , Cs + , Ca 2+ , Sr 2+ , and Ba 2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH) 2 , Sr(OH) 2 , and Ba(OH) 2 . Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. ( Hint: Weak gives you weak and strong gives you worthless.)
For conjugate acid–base pairs, how are K a and K b related? Consider the reaction of acetic acid in water CH 3 CO 2 H ( a q ) + H 2 O ( l ) ⇌ CH 3 CO 2 − ( a q ) + H 3 O + ( a q ) where K a = 1.8 × 10 −5 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH 3 CO 2 − ) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH 3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming K a for a monoprotic strong acid is 1 × 10 6 , calculate K b for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li + , K + , Rb + , Cs + , Ca 2+ , Sr 2+ , and Ba 2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH) 2 , Sr(OH) 2 , and Ba(OH) 2 . Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. ( Hint: Weak gives you weak and strong gives you worthless.)
Solution Summary: The author explains the relationship between the conjugate base of a weak acid and the base dissociation constant.
For conjugate acid–base pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water
CH
3
CO
2
H
(
a
q
)
+
H
2
O
(
l
)
⇌
CH
3
CO
2
−
(
a
q
)
+
H
3
O
+
(
a
q
)
where Ka = 1.8 × 10−5
a. Which two bases are competing for the proton?
b. Which is the stronger base?
c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2−) as a weak base? Use an appropriate reaction to justify your answer.
In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid.
To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 × 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
(f) SO:
Best Lewis Structure
3
e group geometry:_
shape/molecular geometry:,
(g) CF2CF2
Best Lewis Structure
polarity:
e group arrangement:_
shape/molecular geometry:
(h) (NH4)2SO4
Best Lewis Structure
polarity:
e group arrangement:
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
Sketch (with angles):
1.
Problem Set 3b
Chem 141
For each of the following compounds draw the BEST Lewis Structure then sketch the molecule (showing
bond angles). Identify (i) electron group geometry (ii) shape around EACH central atom (iii) whether the
molecule is polar or non-polar (iv)
(a) SeF4
Best Lewis Structure
e group arrangement:_
shape/molecular geometry:
polarity:
(b) AsOBr3
Best Lewis Structure
e group arrangement:_
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
(c) SOCI
Best Lewis Structure
2
e group arrangement:
shape/molecular geometry:_
(d) PCls
Best Lewis Structure
polarity:
e group geometry:_
shape/molecular geometry:_
(e) Ba(BrO2):
Best Lewis Structure
polarity:
e group arrangement:
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
Sketch (with angles):
Chapter 14 Solutions
Study Guide for Zumdahl/Zumdahl/DeCoste’s Chemistry, 10th Edition
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