Determine the poh of 0.01 molar solution of carbonic acid

Hello!

Data:

Molar Mass of H2CO3 (carbonic acid)

H = 2*1 = 2 amu

C = 1*12 = 12 amu

O = 3*16 = 48 amu

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Molar Mass of H2CO3 = 2 + 12 + 48 = 62 g/mol

Now, since the Molarity and ionization constant has been supplied, we will find the degree of ionization, let us see:

M (molarity) = 0.01 M (Mol/L) →

Use: Ka (ionization constant) = 

Now, we will calculate the amount of Hydronium [H3O+] in carbonic acid (H2CO3), multiply the acid molarity by the degree of ionization, we will have:

And finally, we will use the data found and put in the logarithmic equation of the PH, thus:

Data:

apply the data to formula

Note:. The pH <7, then we have an acidic solution (weak acid).

Now, let's find pOH by the following formula:

I Hope this helps, greetings ... DexteR! =)

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

the answer is 0.8m.

by: nicholas