Question

Arsenic acid, H3AsO4 is a triprotic acid. The acid ionization constants are: Ka1 = 5.5×10-3 ....

Arsenic acid, H3AsO4 is a triprotic acid. The acid ionization constants are: Ka1 = 5.5×10-3 . Ka2 = 1.7×10-7 , Ka2 = 5.1×10-12

a) Write the stepwise ionization equilibria for arsenic acid.

b) Determine for a 0.350 M solution of arsenic acid the pH, and the equilibrium concentrations of all species (H3AsO4, H2AsO4 -, HAsO4 2-, AsO4 3-, H3O+, OH-)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Determine the pH of an aqueous solution of 0.0028 M Arsenic Acid. Ka1(H3AsO4) = 5.8x10-3, Ka2(H3AsO4)...
Determine the pH of an aqueous solution of 0.0028 M Arsenic Acid. Ka1(H3AsO4) = 5.8x10-3, Ka2(H3AsO4) = 1.1x10-7, Ka3(H3AsO4) = 3.2x10-17 Charge balance equation: [H+]=[H2AsO4-]+2[HAsO42-]+3[AsO43-]+[OH-] Mass Balance equation: 0.0028 M = [H3AsO4]+[H2AsO4-]+[HAsO42-]+[AsO43-]
Arsenic acid, H3AsO4 (MW= 141.94 g/mol), is a triprotic acid. The Ka values for arsenic acid...
Arsenic acid, H3AsO4 (MW= 141.94 g/mol), is a triprotic acid. The Ka values for arsenic acid are Ka1 = 5.0 x 10^ -4, Ka2 = 8.0 x 10^ -8, and Ka3 = 6.0 x 10 ^ -10. What volumes of 0.25 M H3AsO4, 0.25 M NaOH, and distilled water are required to make a buffer with a pH = 8? The total [AsO4] = 0.05M and the total volume is 1 L.
The triprotic acid H3A has ionization constants of Ka1 = 2.4× 10–3, Ka2 = 4.9× 10–7,...
The triprotic acid H3A has ionization constants of Ka1 = 2.4× 10–3, Ka2 = 4.9× 10–7, and Ka3 = 3.2× 10–11. Calculate the following values for a 0.0170 M solution of NaH2A. Calculate the following values for a 0.0170 M solution of Na2HA.
given a diprotic acid, H2A, with two ionization constants of Ka1 = 1.6×10^-4 and Ka2 =...
given a diprotic acid, H2A, with two ionization constants of Ka1 = 1.6×10^-4 and Ka2 = 5.2×10^-11, calculate the ph for a .206 M solution of NaHA
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1 10-3 and Ka2 =...
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1 10-3 and Ka2 = 2.5 10-6. In order to make up a buffer solution of pH 5.80, which combination would you choose, NaHA/H2A or Na2A/NaHA? NaHA/H2A Na2A/NaHA pKa of the acid component
Calculate the concentration of all species in a 0.490 M solution of H2SO3. The acid ionization...
Calculate the concentration of all species in a 0.490 M solution of H2SO3. The acid ionization constants for the acid are Ka1=1.6×10−2 and Ka2=6.4×10−8. Express your answer using two significant figures. Enter your answers numerically separated by commas. [H2SO3], [HSO−3], [SO2−3], [H3O+], [OH−] =
A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.48× 10–4 and Ka2 =...
A diprotic acid, H2A, has acid dissociation constants of Ka1 = 3.48× 10–4 and Ka2 = 3.21× 10–12. Calculate the pH and molar concentrations of H2A, HA–, and A2– at equilibrium for each of the solutions below.(a) a 0.153 M solution of H2A.(b) a 0.153 M solution of NaHA.(c) a 0.153 M solution of Na2A
For the diprotic weak acid H2A, Ka1= 3.5 x 10^-6 & Ka2= 5.5 x 10^-9 What...
For the diprotic weak acid H2A, Ka1= 3.5 x 10^-6 & Ka2= 5.5 x 10^-9 What is the pH of a 0.0450 M solution of H2A? & What are the equilibrium concentrations of H2A & A2- in this solution? Please explain
Given that the stepwise dissociation constants for phosphoric acid are: Ka1 = 7.5×10-3; Ka2 = 6.2×10-8;...
Given that the stepwise dissociation constants for phosphoric acid are: Ka1 = 7.5×10-3; Ka2 = 6.2×10-8; Ka3 = 4.8×10-13 To prepare 1.20 L of a buffer solution having an ionic strength of 0.150 and a pH of 7.50 would require: Answer to 3 sig figs. a) (mass) of Na2HPO4(anhydrous) and b) (mass) of NaH2PO4(anhydrous).
Given a diprotic acid, H2A, with two ionization constants of Ka1=1.3x10^-4 and Ka2=4.1x10^-12, calculate the pH...
Given a diprotic acid, H2A, with two ionization constants of Ka1=1.3x10^-4 and Ka2=4.1x10^-12, calculate the pH for a .114 M solution of NaHA.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT