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Chemistry
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18 Nov 2019

calculate the concentration of all species in a 0.175 M solution of H2CO3.

H2CO3
HCO3-
CO3 ^2-
H3O-
OH-

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Casey Durgan
Casey DurganLv2
23 Apr 2019

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Related questions

Calculate the concentration of all species in a 0.140 M solution ofH2CO3.

The species are H2CO3,HCO3-, CO3^2-, H30,OH.

Can anyone help show me how to solve this? There are a couple upalready, but they are not correct. Please help me out.

Carbonic acid is a weak diprotic acid whose dissociationreactions are:

H2CO3 (aq) + H2O (l) --> (forward/reverse arrow) H3O+ (aq) +HCO3- (aq) Ka1= 4.3 x 10^-7

HCO3^- (aq) + H2O (l) --> (forward/reverse arrow) H3O+ (aq) +CO3^2- (aq) Ka2= 4.8 x 10^-11

a. What is the equilibrium pH of a carbonic acid solution, whoseoriginal concentration is 0.034 M?

b. What are the concentrations of the other two species?

Calculate the concentration of each species in the equations at a wavelength of: 624.0383911 and Absorption: 0.242581636 Also at wavelegnth of: 418.9806824 and Absorpotion: 0.096807577. With 17ml of DI water at 60psi.

CO2 (g)---> CO2(aq)

CO2 (aq) + H2O --> H2CO3 (aq)

H2CO3 (aq) + H2O (liq) --> H3O+ + HCO3-

HCO3- + H2O (liq) --> H3O+ + CO32-

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