a titration experiment 20 mL solution of hydrochloric acid required 15.2mL of a .879 M barium hydroxide solution. What was the molar concentration of the HCl solution?
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To determine the molar concentration of the hydrochloric acid (HCl) solution, you can use the concept of stoichiometry. In this case, the balanced chemical equation for the reaction between HCl and barium hydroxide (Ba(OH)2) is:
2HCl + Ba(OH)2 -> 2H2O + BaCl2
From the equation, we can see that the ratio between HCl and Ba(OH)2 is 2:1. So, for every 2 moles of HCl, there will be 1 mole of Ba(OH)2.
First, let's calculate the number of moles of Ba(OH)2 used in the titration:
Moles of Ba(OH)2 = Molarity * Volume
= 0.879 M * 15.2 mL / 1000 mL/L
= 0.01337 moles
Since the stoichiometric ratio is 2:1, the number of moles of HCl is twice the number of moles of Ba(OH)2:
Moles of HCl = 2 * 0.01337 moles
= 0.02674 moles
Now, let's calculate the molar concentration of the HCl solution:
Molarity = Moles of solute / Volume of solution
= 0.02674 moles / 20 mL / 1000 mL/L
= 1.337 M
Therefore, the molar concentration of the hydrochloric acid (HCl) solution is approximately 1.337 M.