Identify the chemical species in the carbonate system, and explain the significance of the system. Hence, on the bases of the following equilibria, determine the concentrations carbonate system species in a stream with a pH of 5.8.
CO2(g) ↔ CO2(aq) KH = 3.4 x 10-2 mol L-1 atm-1;
CO2(aq) + H2O ↔ H2CO3; Kr = 2 x 10-3 mol L-1 atm-1;
H2CO3(aq) ↔ H+ + HCO3-; Ka1 = 4.47 x 10-7 M.
HCO3- ↔ H+ + CO32-; Ka2 = 4.68 x 10-11 M.
Identify the chemical species in the carbonate system, and explain the significance of the system...
Given the set of reactions below, combine the first two equations and then model the system resulting from the resulting two reactions as if it were a diprotic acid system. Include a fractional composition plot of the α of species CO2 (aq), HCO3 – (aq) and CO3 2– (aq) as a function of pH. CO2 (aq) + H2O ⇄ H2CO3(aq) H2CO3(aq) + H2O ⇄ HCO3 – (aq) + H3O+ HCO3 – (aq) + H2O ⇄ CO3 2– (aq) + H3O+...
What is the pH of a 1.25 L carbonate buffer which was prepared by mixing 0.4098 M of Na2CO3 and 0.550 M NaHCO3. (Ka of HCO3- = 4.70 x 10-11) HCO3- (aq) + H2O (l) ↔ CO32- (aq) + H3O+ (aq)
What is the pH of rainwater in pristine environments? Assume the temperature is 25°C, the total pressure is 1 atm and the rainwater is in equilibrium with the atmosphere. Solution: 5 species are present in the aqueous phase H2CO3(aq), HCO3-(aq), CO3-2(aq), H+ and OH- Equations: 1H2CO3 → H+ + HCO3- (carbonic acid dissociation) K1 = [H+][HCO3-]/[H2CO3] = 4.47 x 10-7M
a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beverages contain measurably less water than the same volume of pure water. C. rainwater is slightly acidic b) A 1.0 M solution of a weak monoprotic acid with Ka = 1.0 10-6 would have a pH of: A. 1 B. 2 C. 3 D. 6 c) Ascorbic acid is a diprotic acid with Ka1 =...
8. The normal pH of human blood is about 7.4. The carbonate buffer system in the blood uses the following reaction: CO2(+ 2H2O() H2CO3(aq) HCO3(aq) + H:04) The concentration of carbonic acid, H2CO3, is approximately 0.0012M and the concentration of the hydrogen carbonate ion, HCO3 is around 0.024M. Calculate the pH of blood
a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beverages contain measurably less water than the same volume of pure water. C. rainwater is slightly acidic b) A 1.0 M solution of a weak monoprotic acid with Ka = 1.0 10-6 would have a pH of: A. 1 B. 2 C. 3 D. 6 c) Ascorbic acid is a diprotic acid with Ka1 =...
You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11. a) What will the initial pH of the solution be? b) What volume of 0.1 M NaOH will you need to add to reach the second equivalence point( remember carbonic acid deprotonates to bicarbonate HCO3- and then can deprotonate further to CO32-? c) At the second equivalence point, what will the...
Estimate the pH of natural rainwater, assuming the only substance effecting it is the adsorption of CO2 from the atmosphere. Assume the concentration of CO2 is 390 ppm, and the temperature and pressure are 25 "C and 1 atmosphere. Steps. Assume the absorption of CO2 adds only the carbonate system ions so the ionic present must balance, and are due to Ht, OH, HCO3, and CO32. Establish your charges charge balance equation-+'s = -'s i. Assuming the rainfall is slightly...
Plankton, shellfish, and corals have an exoskelton made up of calcium carbonate (CaCO3). These organism need to have the carbonate ion (CO3:2) in seawater in order to make their shells. In the ocean, carbonate is in equilibrium with the bicarbonate ion according to the following equation HCO3 (aq) + H2O(l) = CO2 (aq) + H30+(aq) Ka2 = 4.7 x 10-11 The pH of the ocean is decreasing. What effect does this have on the concentration of the carbonate ion? Answer:
1) why is CO2 the conjugate acid of bicarbonate? Please explaing CO2 (g) + H2O(l) ⇄ H2CO3 (aq) 2) Exercise increases metabolism and thus increase the amount of CO2 in the blood. Following a bout of intense exercise, the pH of your blood was found to be 7.1 and the HCO3− concentration in the blood to be 8 mM. Remember the overall reaction for the bicarbonate buffering system in the blood can be written as: H2CO3 (aq) ⇄ HCO3- (aq)...