The concentration of carbonic acid is proportional to partial pressure of CO2
[H2CO3] = K X pCO2 = 0.032 X 7.1 X 10^-4 = 2.272 X 10^-5 M
Now dissociation constant of carbonic acid H2CO3 <--> H+ (aq) + HCO3- (aq), Ka = 2.5 x 10^-4
So [H+] = (Ka X [H2CO3] )1/2
[H+] = (2.5 X 10^-4 X [2.272 X 10^-5] )1/2 = 0.753 X
10^-4
pH = -log [H+] = 4.123
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO_2. Dissolved CO_2...
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation CO2(gas)<------>CO2(aq) K=0.032 M*atm-1 The acid dissociation constants listed in most standard reference texts for carbonic acid actually apply to dissolved CO2. For a CO2 partial pressure of 3.1×10-4 atm in the atmosphere, what is the pH of water in equilibrium with the atmosphere?
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation. CO2 (g) <--> CO2 (aq) K= 0.032 M atm-1 The acid dissociation constants listed in most standard reference texts for carbonic acid actually apply to dissolved CO2. For a CO2 partial pressure of 8.8×10-4 atm in the atmosphere, what is the pH of water in equilibrium with the atmosphere?
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation The acid dissociation constants listed in most standard reference texts for carbonic acid actually apply to dissolved CO2. For a CO2 partial pressure of 1.8×10–4 bar in the atmosphere, what is the pH of water in equilibrium with the atmosphere? (For carbonic acid Ka1 = 4.46× 10–7 and Ka2 = 4.69× 10–11). Carbon dioxide dissolves in water to form carbonic...
(8 pts) Carbon dioxide in the atmosphere dissolves in water to establish an equilibrium that can increase the acidity of aqueous solutions in the environment. This equilibrium is CO2 (g) ⇌ CO2 (aq), Kh = 3.1 * 10^2 at 25°C. Kh is called the Henry’s law constant, which relates the solubility of the gas CO2 in the aqueous solution, [CO2], to the partial pressure of CO2 over the solution, p(CO2): [CO2] (M) = Kh * p(CO2) (atm) During the preceding...
Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 12.4 g of carbonic acid? H2CO3 → H2O + CO2
(8 pts) Carbon dioxide in the atmosphere dissolves in water to establish an equilibrium that can increase the acidity of aqueous solutions in the environment. This equilibrium is CO2(g) = CO2 (aq), Kn= 3.1 x 10-2 at 25°C. Kh is called the Henry's law constant, which relates the solubility of the gas CO2 in the aqueous solution, [CO2), to the partial pressure of CO2 over the solution, p(CO2): [CO2] (M)= Kn · p(CO2) (atm) During the preceding decades, the atmospheric...
Part A Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 3.10 g of carbonic acid? H2CO3 + H2O + CO2 4.379 2.20 g 10.7 g 3.10 9 0.900 g Submit Request Answer Provide Feedback
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