Question

Determine the total concentration of CO_{2} solution
whose pH 4.5. pKa of H_{2}CO_{3} = 3.6 and the
equilibrium constant of CO_{2} hydration (to produce
H_{2}CO_{3}) K = 0.0017. Show your work.

Answer #1

**H2CO3 (aq) <---> H (aq) + HCO3- (aq) , pka = 3.6 ,
Ka = 10^ -3.6 = 2.5 x 10^ -4**

**goven pH = 4.5 , [H+] = 10^ -4.5 = 3.16 x 10^ -5 M =
[HCO3-]**

**at equilibrium Ka = [H+] [HCO3-] /[H2CO3]**

**2.5 x 10^ -4 = (3.16 x 10^-5) ( 3.16 x 10^ -5) / (
[H2CO3]**

**[H2CO3] = 4 x 10^ -6**

**Initial [H2CO3] = equilibrium [H2CO3] +
[H+] ( since some part of H2CO3 is diddciated to
form H+)**

** = 4 x 10^ -6 + 3.16 x 10^
-5**

** = 3.56 x 10^ -5**

**We now have another equilibrium**

**CO2 (aq) + H2O (l) <--> H2CO3 (aq) , K =
0.0017**

**K = [H2CO3] /[CO2]**

**0.0017 = ( 3.56 x 10^ -5) /[CO2]**

**[CO2] =0.02094**

**Initial [CO2] = equi [CO2] + {H2CO3]**

**= 0.02094 + 3.56x10^-5**

**= 0.021 M**

Calculate the concentration of all species in a 0.145 M solution
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Express your answer using two significant figures.
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[CO2−3]=
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medicine, where understanding the Henderson-Hasselbalch equation is
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