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What is the pH of rainwater at 25°C in which atmospheric CO2 has dissolved, producing an...
What is the pH of rainwater at 25°C in which atmospheric CO2 has dissolved, producing an initial [H2CO3] of 1.96×10-5M ? Take into account the autoionization of water.
A sample of rainwater is observed to have a pH of 7.26. If only atmospheric CO2 at 400 ppm and limestone dust are present in the atmosphere to alter the pH from a neutral value, and if each raindrop has a volume of 0.0301 cm3, what mass of calcium (in ng) is present in each raindrop?
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
What is the pH of a sample of river water in which (HCO3-) = 2.0 x 10-4 M and the concentration of dissolved CO2 in equilibrium with atmospheric CO2 is 1.0 x 10-5 M? Chemical Equation: H2CO3(aq) + H2O(l) = HCO3-(aq) + H3O+(aq) pka = 6.37 Henderson Hasselbach equation: pH=pka+log [base]/[acid] A/
A soda pop has a pH = 3.80 at 25oC. Calculate the pressure of CO2 inside a closed-bottle of this soda pop at 25oC. Assume only water and CO2 are present and all dissolved CO2 is present as H2CO3. Ka1 (H2CO3) = 4.3 x 10^-7 and delta Gf naught (H2CO3 (aq)) = - 623.08 kJ/m
A soda pop has a pH = 3.80 at 25oC. Calculate the pressure of CO2 inside a closed-bottle of this soda pop at 25oC. Assume only water and CO2 are present and all dissolved CO2 is present as H2CO3. Ka,1(H2CO3) = 4.3 x 10-7 and ΔGfo(H2CO3,aq) = - 623.08 kJ/m Please include all math steps. The answer is Pco2=1.7atm
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...
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 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...
If a container of pure water is shaken in the air, the water will dissolve atmospheric carbon dioxide until the dissolved gas reaches the solubility of Co2, 1X10-5 M, the acidity constant K1, of the carbonic acid is 4*10t-7. What would be the pH o with Co2? f the water saturated