A 327- ML sample of unknown HCI solution reacts completely with Na2CO3 to form 20.1 g CO2 What was the concentration of the HCI solution?
Na2CO3 + 2HCl ==> 2NaCl + H2O + CO2
Convert 20.1 g CO2 to moles. moles = grams/molar mass.
Using the coefficients in the balanced equation, convert moles CO2 to moles HCl.
Now convert moles HCl to M. M = moles/L of solution.
To determine the concentration of the HCl solution, we need to use a balanced chemical equation and stoichiometry.
The balanced chemical equation for the reaction between HCl and Na2CO3 is:
2HCl + Na2CO3 → H2O + CO2 + 2NaCl
From the balanced equation, we can see that 2 moles of HCl react with 1 mole of Na2CO3 to produce 1 mole of CO2.
First, let's convert the mass of CO2 (20.1 g) to moles using the molar mass of CO2 (44.01 g/mol):
moles of CO2 = mass of CO2 / molar mass of CO2 = 20.1 g / 44.01 g/mol ≈ 0.457 mol
Since 1 mole of CO2 is produced from 2 moles of HCl, we can determine the moles of HCl present in the reaction:
moles of HCl = 0.457 mol CO2 × (2 mol HCl / 1 mol CO2) ≈ 0.914 mol
Finally, we can calculate the concentration (molarity) of the HCl solution, given that we have a 327 mL (or 0.327 L) sample:
concentration of HCl = moles of HCl / volume of solution (in L)
= 0.914 mol / 0.327 L ≈ 2.8 M
Therefore, the concentration of the HCl solution is approximately 2.8 M.