Question

Calculate the concentration of all species in a 0.180 M solution of H2CO3 find : [H2CO3] , [HCO3^-] , [CO3^-2] , [H3O^+] , [OH-] Please explain steps, thank you.

Answer #1

CO2(g) + H2O <==> H+ + HCO3- .............. Ka = 4.5 x
10^-7

HCO3^- is a weaker acid, dissociating to a slight extent to produce
H+ and CO3^2-

HCO3^- <==> H+ + CO3^2- ....................... Ka = 4.7 x
10^-11

Ka = [H+] [HCO3-] / [CO2]

4.5x10^-7 = x&2up2 / 0.180

x = 2.85x10^-4

Ka2 = [H+] [CO3^^2-] / [HCO3-]

4.7x10^-11 = [CO3^2-

[CO2] = 0.180

[H+] = 2.85x10^-4 M

[HCO3^-] = 2.85x10^-4 M

[CO3^2-] = 4.7x10^11

[OH-] = 1.00x10^-14 / 2.85x10^-4 = 3.5x10^-11

Calculate the concentration of all species in a 0.145 M solution
of H2CO3. The answers are the following: [H2CO3], [HCO−3], [CO2−3],
[H3O+], [OH−] = 0.145,2.5×10−4,5.6×10−11,2.5×10−4,4.0×10−11; I am
just having the hardest time figuring out how [CO3^2-] was
calculated. I keep getting 4.69 x 10^-11M instead of 5.6x10^-11

Calculate the concentration of [H2CO3], [HCO3(-)], [CO3 (2-)],
[H3O(+)], and [OH(-)] in a 0.140M solution of H2CO3. In
paranthesis, are the charges of the ions.

Calculate the concentration of all species in a 0.145 M solution
of H2CO3. Enter your answers numerically separated by commas.
Express your answer using two significant figures.
[H2CO3]=
[HCO−3]=
[CO2−3]=
[H3O+]=
[OH−]=
Please show work!

Calculate the concentration of all species in a 0.165 M solution
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Express your answer using two significant figures. [H2CO3],
[HCO−3], [CO2−3], [H3O+], [OH−] =

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couple of wrong answers posted to this question...
thanks
Calculate the concentration of all species in a 0.140 M solution
of H2CO3.
[H2CO3], [HCO−3], [CO2−3], [H3O+], [OH−] =

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[K+], [F−], [HF], [OH−], [H3O+]

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[H2SO3], [HSO−3], [SO2−3], [H3O+], [OH−]

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Calculate the concentrations of all species in a 0.180-M
solution of H2X if K1 = 5.01E-05 and
K2 = 2.82E-08
[H2X] =
M
[H3O1+] =
M
[HX1-] =
M
[X2-] =
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