Sulfurous acid, H2SO3, is a diprotic acid with Ka1= 1.3*10^-2
and Ka2= 6.3*10^-8. What is the pH of 0.200M solution of the
sulfurous acid? What is the concentration of the sulfite ion,
SO3^2-, in the solution? What is the percent ionization of
H2SO3?
Please include a brief explanation of your reasoning if you can;
I'd really like to understand this. Thank you!
Sulfurous acid (H2SO3) has
Ka1 = 1.500 × 10-2 and
Ka2 = 1.000 × 10-7. Consider the
titration of 60.0 mL of 1 M sulfurous acid by 1 M NaOH and answer
the following questions.
What is the maximum number of protons that can sulfurous acid
ionize (per molecule)?
b) Calculate the pH after the following total
volumes of NaOH have been added. (Correct to 2
decimal places.) No marks will be given if
the number of decimal places is wrong....
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
Ka1 = 1.5 ✕ 10-2 Ka2 = 2.6 ✕ 10-7
A 50.0 mL sample of 0.15 M of maleic acid is titrated with 0.13
M NaOH. Calculate the pH at the following points in the titration
curve. (a) the first half-equivalence point (b) the first
equivalence point (c) the second half-equivalence point (d) the
second equivalence point
Part A
Calculate the pH and the concentrations of all species present
in 0.16 M H2SO3. (Ka1 = 1.5×10−2, Ka2 =
6.3×10−8)
Express your answer to three significant figures and include the
appropriate units.
pH =
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Up
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Part B
Calculate the concentration of H2SO3 in solution.
Express your answer to two significant figures and include the
appropriate units.
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Part C
Calculate the concentration...
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 ( 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...