Question 1 D Buffer solutions containing Naz CO, and NaHCO, range in pH from 10.0 to 11.0. The chemical equation below represents the equilibrium between CO, and H20, and the table lists the composition of four different buffer solutions at 25°C Co,? (ag) + H20(1) 2 HCO, (ag) + OH (ag) K, = 2.1 x 104 at 25"C Buffer [NAHCO,) [Na, COs] pH 1 0.150 0.100 2 0.200 0.200 10.32 3 0.100 0.100 10.32 4 0.100 0.200 Which of the following chemical equilibrium equations best shows what happens in the buffer solutions to minimize the change in pH when a small amount of a strong base s added? A H,O* (aq) + OH (aq) 2H,O(1) HCO: (aq) + OH (ag) CO (aq) + HzO(I) в c) Co, (ag) + HsO' (aq) =HC0, (aq) + H2O(I) D co,? (ag) + H2O(I) =HCO; (ag) + OH (aq)
Question 1 D Buffer solutions containing Naz CO, and NaHCO, range in pH from 10.0 to 11.0. The chemical equation below represents the equilibrium between CO, and H20, and the table lists the composition of four different buffer solutions at 25°C Co,? (ag) + H20(1) 2 HCO, (ag) + OH (ag) K, = 2.1 x 104 at 25"C Buffer [NAHCO,) [Na, COs] pH 1 0.150 0.100 2 0.200 0.200 10.32 3 0.100 0.100 10.32 4 0.100 0.200 Which of the following chemical equilibrium equations best shows what happens in the buffer solutions to minimize the change in pH when a small amount of a strong base s added? A H,O* (aq) + OH (aq) 2H,O(1) HCO: (aq) + OH (ag) CO (aq) + HzO(I) в c) Co, (ag) + HsO' (aq) =HC0, (aq) + H2O(I) D co,? (ag) + H2O(I) =HCO; (ag) + OH (aq)
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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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![Question 1 A
Buffer solutions containing Naz CO; and NaHCO, range in pH from 10.0 to 11.0. The chemical equation below represents the equilibrium between CO, and H2O, and the table lists the composition of four different buffer solutions at 25 C
2-
Co, (aq) + H20(1) 2HCO, (aq) + OH (aq)
K, = 2.1 x 10-4 at 25°C
Buffer
NaHCO,
[Na, COs]
pH
1
0.150
0.100
2
0.200
0.200
10.32
3
0.100
0.100
10.32
4
0.100
0.200
Which of the following chemical equilibrium equations best shows what happens in the buffer solutions to minimize the change in pH when a small amount of a strong base
added?
A H,O* (ag) +OH (aq) 2H;O(1)
B) HCO, (ag) + OH (aq) 2 CO3 (aq) + H2O(1)
c) Co, (ag) + H;O' (ag) =HCO, (aq) + H2O(1)
D Co,? (ag) + H;O(I) =HCO, (ag) + OH (aq)
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Transcribed Image Text:Question 1 A
Buffer solutions containing Naz CO; and NaHCO, range in pH from 10.0 to 11.0. The chemical equation below represents the equilibrium between CO, and H2O, and the table lists the composition of four different buffer solutions at 25 C
2-
Co, (aq) + H20(1) 2HCO, (aq) + OH (aq)
K, = 2.1 x 10-4 at 25°C
Buffer
NaHCO,
[Na, COs]
pH
1
0.150
0.100
2
0.200
0.200
10.32
3
0.100
0.100
10.32
4
0.100
0.200
Which of the following chemical equilibrium equations best shows what happens in the buffer solutions to minimize the change in pH when a small amount of a strong base
added?
A H,O* (ag) +OH (aq) 2H;O(1)
B) HCO, (ag) + OH (aq) 2 CO3 (aq) + H2O(1)
c) Co, (ag) + H;O' (ag) =HCO, (aq) + H2O(1)
D Co,? (ag) + H;O(I) =HCO, (ag) + OH (aq)
P Type here to search
Esc
FnLk
F1
F2
F3
888
Home
End
F4
F5
F6
F7
F8
F10
F11
F12
@
2
%2#3
4
1
&
5
6
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