# Problem: Calculate the pH and equilibrium concentration of all species present in a 0.150 M carbonic acid solution. For carbonic acid (H2CO3: Ka1 = 4.3 x 10-7 and Ka2 = 4.8 x 10-11 ).

###### FREE Expert Solution

We are being asked to calculate the pH of the solution and equilibrium concentration of each species if the concentration of H2COis 0.15 M

We're going to calculate the pH of the solution using the following steps:

Step 1: Construct an ICE chart for the equilibrium reaction.
Step 2: Write the Ka expression.
Step 3: Calculate for the equilibrium concentration.
Step 4: Calculate pH.

Step 1: Construct an ICE chart for the equilibrium reaction.

Since we’re dealing with a weak acid and Ka is an equilibrium expression, we will have to create an ICE chart to determine the equilibrium concentration of each species:

H2COweak acidproton donor
H2O → will act as the weak baseproton acceptor

We will use the first equilibrium reaction given:

H2CO3  +  H2O (l) ⇋ HCO (aq) + H3O(aq)               Ka1 = 4.3 x 10–7

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###### Problem Details

Calculate the pH and equilibrium concentration of all species present in a 0.150 M carbonic acid solution. For carbonic acid (H2CO3: Ka1 = 4.3 x 10-7 and Ka2 = 4.8 x 10-11 ).

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Diprotic Acid concept. You can view video lessons to learn Diprotic Acid. Or if you need more Diprotic Acid practice, you can also practice Diprotic Acid practice problems.

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