20.0 mL of aqueous solution of 0.0500mol/L barium hydroxide is titrated with 0.1

Question

20.0 mL of aqueous solution of 0.0500mol/L barium hydroxide is titrated with 0.100mol/L of hydroiodic acid. Calculate the number of moles of all ions in the erlenmeyer after 5.50mL of hydroiodic acid solution was added. Use the net ionic equation and and IRF table. Here is how I solved this problem but is the solution right? DO NOT SOLVE THE PROBLEM AGAIN, please just confirm if the solution below is right or wrong (if wrong why).

Logic behind my reasoning: This is an acid base reaction, the point of interest isnt the formation of BaCl2, this is just a spectator ion that does not participate in the acid base reaction. The reaction of interest here, since it is an acid base titration, is represented by the following Net Ionic Equation: H + OH- = H2O(l) . See all work on the picture.

Explanation / Answer

Your process looks good to me.

Al last you just need to calculate numberof moles of each ions and you have done that too.

Also calculate the amount of other ions like I- and Ba2+ . They will not chage. So there initial number of moles will be same as final number of moles.

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