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Please help! Calculate the % hydrolysis for 1 M Na2CO3 if [OH-] = 5.4x10^-(4).

  • Thread starter imconfused
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  • #1
Calculate the % hydrolysis for 1 M Na2CO3 if [OH-] = 5.4x10^-(4)
 

Answers and Replies

  • #2
Borek
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Done.

Ignoring template and not showing any effort will lead you nowhere.
 
  • #3
Done.

Ignoring template and not showing any effort will lead you nowhere.
Huh? But I asked my question. This is the only information I was given.

No effort? But I'm stuck! I'm showing some effort by asking for some help here on ONE problem!
 
  • #4

Homework Statement



Calculate the % hydrolysis for 1 M Na2CO3 if [OH-] = 5.4x10^-(4).

Not sure what to put for the other fields.
 
  • #5
Borek
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Do you know any reaction equations? What is hydrolysis?
 
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  • #6
Calculate the theoretical % hydrolysis for 1 M solution of Na2CO3

Homework Statement


Calculate the theoretical % hydrolysis for 1 M solution of Na2CO3


Homework Equations


CO3^(2-) + 2H2O -> H2CO3 + 2OH^(-1)

or

CO3^(2-) + H2O -> HCO3^(-1) + OH^(-1)
HCO3^(-1) + H2O -> H2CO3 + OH^(-1)

Chart values for the Ka1 and Ka2 of H2CO3:
Ka1 = 4.3x10^(-7)
Ka2 = 5.6x10^(-11)

The Attempt at a Solution



Kb1 = {[HCO3^(-1)][OH^(-1)]}/[CO3^(-2)] = Kw/Ka2 = [10^(-14)]/[5.6x10^(-11) = 1.78x10^(-4)

Kb2 = {[H2CO3][OH^(-1)]}/[HCO3^(-1)] = Kw/Ka1 = [10^(-14)]/[4.3x10^(-7)] = 2.32x10^(-8)
 
  • #7
Redbelly98
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Moderator's note: merged two threads.
 
  • #8
Borek
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CO3^(2-) + H2O -> HCO3^(-1) + OH^(-1)
You know equilibrium concentration of OH- - can you use it to calculate concentration of HCO3-?

How is hydrolysis percentage defined?
 
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