Question

In: Chemistry

The Ka's for H2CO3 are K1 = 4.5 x 10^-11. Calculate the pH of the solution...

The Ka's for H2CO3 are K1 = 4.5 x 10^-11. Calculate the pH of the solution when 45.9 ml of 0.25 M KHCO3 is mixed with a)35 mL 0.15 M HBr.     b) 50.0 mL of 0.15 M KOH

Solutions

Expert Solution

H2CO3 Ka1 = 4.3 x 10^-7

Ka2 = 5.6 x 10^-11

millimoles of HCO3- = 45.9 x 0.25 = 11.475

millimoles of HBr = 35 x 0.15 = 5.25

HCO3- +       H+   ----------------> H2CO3

11.475       5.25                            0

6.225            0                       5.25

pOH = pKb1 + log [HCO3- / H2CO3]

        = 7.63 + log [6.225 / 5.25]

        = 7.70

pH = 14 - 7.70 = 6.3

pH = 6.30

(b)

millimoles of KOH = 50 x 0.15 = 7.5

HCO3- +   OH-   -------------------> CO32- + H2O

11.475       7.5                                    0            0

3.975           0                                    7.5          7.5

pH = pKa2 + log [CO32- / HCO3-]

     = 10.25 + log [7.5 / 3.975]

     = 10.53

pH = 10.53

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

The solubility of CaCO3 is pH dependent. (Ka1(H2CO3)=4.3×10−7,Ka2(H2CO3)=5.6×10−11.) **Part A Calculate the molar solubility of CaCO3...
The solubility of CaCO3 is pH dependent. (Ka1(H2CO3)=4.3×10−7,Ka2(H2CO3)=5.6×10−11.) **Part A Calculate the molar solubility of CaCO3 ( Ksp = 4.5×10−9) neglecting the acid-base character of the carbonate ion. Express your answer using two significant figures. S = 6.71⋅10−5 M (****THIS HAS BEEN ANSWERED, PLACED HERE FOR REFERENCE ONLY****) Part B-- Use the Kb expression for the CO32− ion to determine the equilibrium constant for the reaction CaCO3(s)+H2O(l)⇌Ca2+(aq)+HCO3−(aq)+OH−(aq) Express your answer using two significant figures. K = ?????? Part C ---...
The solubility of CaCO3 is pH dependent. (Ka1(H2CO3)=4.3×10−7,Ka2(H2CO3)=5.6×10−11.) Part A Calculate the molar solubility of CaCO3...
The solubility of CaCO3 is pH dependent. (Ka1(H2CO3)=4.3×10−7,Ka2(H2CO3)=5.6×10−11.) Part A Calculate the molar solubility of CaCO3 ( Ksp = 4.5×10−9) neglecting the acid-base character of the carbonate ion. Part B Use the Kb expression for the CO32− ion to determine the equilibrium constant for the reaction CaCO3(s)+H2O(l)⇌Ca2+(aq)+HCO3−(aq)+OH−(aq) Part C If we assume that the only sources of Ca2+, HCO3−, and OH− ions are from the dissolution of CaCO3, what is the molar solubility of CaCO3using the preceding expression? Part D...
Calculate the pH of an aqueous solution that is 1.0 M Na2CO3. Ka2 for H2CO3 is...
Calculate the pH of an aqueous solution that is 1.0 M Na2CO3. Ka2 for H2CO3 is 4.7 × 10-11. Please post full work and explanation. Thank you.
Calculate the pH of a solution that is 1.5 x 10^-8 M NaOH. This is a...
Calculate the pH of a solution that is 1.5 x 10^-8 M NaOH. This is a very dilute solution
Part A Calculate the pH in 0.020 M H2CO3 (Ka1=4.3×10−7; Ka2=5.6×10−11). Express your answer using two...
Part A Calculate the pH in 0.020 M H2CO3 (Ka1=4.3×10−7; Ka2=5.6×10−11). Express your answer using two decimal places. pH = SubmitMy AnswersGive Up Part B Calculate the concentrations of all species present (H2CO3, HCO−3, CO2−3, H3O+ and OH−) in 0.020 M H2CO3. Express your answers using two significant figures. Enter your answers numerically separated by commas. [H2CO3], [HCO−3], [CO2−3], [H3O+] and [OH−] = M
Question: Calculate The PH Of A 0.080 M Carbonic Acid Solution, H2CO3(aq), That Has The Stepwise...
Question: Calculate The PH Of A 0.080 M Carbonic Acid Solution, H2CO3(aq), That Has The Stepwise Dissociation Constants Ka1=4.3x10^-7 And Ka2=5.6x10^-11.
Calculate the pH of a 0.080 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation...
Calculate the pH of a 0.080 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11. Group of answer choices 10.25 1.10
Calculate the pH of an aqueous solution containing 1.0 x 10^-2 M HCL, 1.0 x 10^-2...
Calculate the pH of an aqueous solution containing 1.0 x 10^-2 M HCL, 1.0 x 10^-2 M H2SO4 (Ka1 = Ka2 = 1.2 x 10^-2 M HCN (Ka = 6.2 x10^-10).
find the pH of an aqueous 0.050 M carbonic acid (H2CO3) solution. Ka1 = 4.3 x...
find the pH of an aqueous 0.050 M carbonic acid (H2CO3) solution. Ka1 = 4.3 x 10^-7, Ka2 = 5.2 x 10^-11.
a) Neglecting activity coefficients, calculate the pH of an aqueous solution of 5.0 x 10-7 M...
a) Neglecting activity coefficients, calculate the pH of an aqueous solution of 5.0 x 10-7 M KOH. b) What fraction of the total [H+] is derived from the autoionization of water?
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT