The binding of oxygen by hemoglobin (Hb), giving oxy-hemoglobin (HbO 2 ), is partially regulated by the concentration of H 3 O+ and dissolved CO 2 in the blood. Although the equilibrium is complicated, it can be summarized as HbO 2 ( a q ) + H 3 O + ( a q ) + CO 2 ( g ) ⇌ CO 2 − Hb − H + + O 2 ( g ) + H 2 O ( l ) (a) Write the equilibrium constant expression for this reaction. (b) Explain why the production of lactic acid and CO 2 in a muscle during exertion stimulates release of O 2 from the oxy-hemoglobin in the blood passing through the muscle.
The binding of oxygen by hemoglobin (Hb), giving oxy-hemoglobin (HbO 2 ), is partially regulated by the concentration of H 3 O+ and dissolved CO 2 in the blood. Although the equilibrium is complicated, it can be summarized as HbO 2 ( a q ) + H 3 O + ( a q ) + CO 2 ( g ) ⇌ CO 2 − Hb − H + + O 2 ( g ) + H 2 O ( l ) (a) Write the equilibrium constant expression for this reaction. (b) Explain why the production of lactic acid and CO 2 in a muscle during exertion stimulates release of O 2 from the oxy-hemoglobin in the blood passing through the muscle.
The binding of oxygen by hemoglobin (Hb), giving oxy-hemoglobin (HbO2), is partially regulated by the concentration of H3O+ and dissolved CO2 in the blood. Although the equilibrium is complicated, it can be summarized as
HbO
2
(
a
q
)
+
H
3
O
+
(
a
q
)
+
CO
2
(
g
)
⇌
CO
2
−
Hb
−
H
+
+
O
2
(
g
)
+
H
2
O
(
l
)
(a) Write the equilibrium constant expression for this reaction.
(b) Explain why the production of lactic acid and CO2 in a muscle during exertion stimulates release of O2 from the oxy-hemoglobin in the blood passing through the muscle.
Acetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions:
HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone
protons, H+ (aq), do not exist!).
(a) Write the equilibrium constant expression for the dissociation of acetic acid.
(b) Vinegar sold commercially is typically 0.8 − 1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures?
(c) What is the value of the equilibrium constant Keq for the dissociation according to the concentrations from part (b)?
(d) When starting with completely un-dissociated…
Acetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions:
HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone protons, H+ (aq), do not exist!).
(d) When starting with completely un-dissociated acetic acid, is it accurate to assume that [HOAc]0 = [HOAc]eq? Why or why not?
(e) A highly concentrated acetic acid solution contains 15.0M acetic acid at equilibrium. What are the equilibrium concentrations of the hydronium and acetate ions in this solution?
(f) Creating the concentrated acetic acid solution by dissolving liquid HOAc in water raises the temperature of the water by about 5°C from room temperature. At 50°C, do you expect the solution to contain more or less acetate ion OAc– than what you calculated in (c)? Why?
You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth.
Y2O + Y2O ⇌ Y3O+ + OY–
Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths place
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