• imconfused
In summary, to calculate the theoretical % hydrolysis for 1 M Na2CO3, one must use the equilibrium concentrations of OH- and HCO3- to determine the equilibrium concentration of H2CO3. Then, using the equilibrium concentration of H2CO3 and the initial concentration of Na2CO3, the percentage of hydrolysis can be calculated.
imconfused
Calculate the % hydrolysis for 1 M Na2CO3 if [OH-] = 5.4x10^-(4)

Done.

Ignoring template and not showing any effort will lead you nowhere.

Borek said:
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!

## Homework Statement

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

Not sure what to put for the other fields.

Do you know any reaction equations? What is hydrolysis?

Last edited by a moderator:
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)

imconfused said:
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?

Last edited by a moderator:

## 1. What is the equation for calculating % hydrolysis?

The equation for calculating % hydrolysis is (% hydrolysis) = ([OH-]/[initial concentration]) x 100%.

## 2. What is the initial concentration of Na2CO3 in this problem?

The initial concentration of Na2CO3 is 1 M.

## 3. How do you calculate the concentration of hydroxide ions ([OH-]) in this problem?

The concentration of hydroxide ions can be calculated using the formula [OH-] = Kw/[H+] where Kw is the ion product constant for water and [H+] is the concentration of hydrogen ions.

## 4. Can you provide the numerical value for the ion product constant for water (Kw)?

The ion product constant for water (Kw) is 1 x 10^-14 at 25°C.

## 5. What is the % hydrolysis for 1 M Na2CO3 if [OH-] = 5.4x10^-(4)?

The % hydrolysis for 1 M Na2CO3 with [OH-] = 5.4x10^-(4) is 0.054%.

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