Question

A 0.225 L solution of H₂CO₃ is neutralized by 0.0880 L of a 1.22 M Fe(OH)₃ solution. What is the concentration of the H₂CO₃ solution?

a) 0.37 M
b) 0.48 M
c) 0.58 M
d) 0.69 M

Answer 1

To calculate the concentration of the H₂CO₃ solution, we can use stoichiometry and the balanced equation for the reaction. Given the volume and concentration of the Fe(OH)₃ solution used, we can determine the number of moles of Fe(OH)₃. Since the reaction stoichiometry is 1:2 for H₂CO₃ and Fe(OH)₃, we can calculate the number of moles of H₂CO₃ and then the concentration of the solution.

Step-by-step explanation:

To find the concentration of the H₂CO₃ solution, we can use the concept of stoichiometry and the balanced equation for the neutralization reaction.

The balanced equation is:

H₂CO₃ + 2Fe(OH)₃ → 2FeCO₃ + 3H₂O

From the equation, we can see that 1 mole of H₂CO₃ reacts with 2 moles of Fe(OH)₃.

Given that 0.0880 L of 1.22 M Fe(OH)₃ solution is used, we can calculate the number of moles of Fe(OH)₃:

moles of Fe(OH)₃ = (0.0880 L)(1.22 M) = 0.10736 moles

Since 1 mole of H₂CO₃ reacts with 2 moles of Fe(OH)₃, the number of moles of H₂CO₃ is half of that:

moles of H₂CO₃ = 0.10736 moles / 2 = 0.05368 moles

Now, we can calculate the concentration of the H₂CO₃ solution:

concentration of H₂CO₃ = moles of H₂CO₃ / volume of solution

Given that the volume of the H₂CO₃ solution is 0.225 L:

concentration of H₂CO₃ = 0.05368 moles / 0.225 L = 0.2384 M

The concentration of the H₂CO₃ solution is approximately 0.24 M.