Each mix has a total volume of 50.0 ml. This is purposely done to ease the calcu

Question

Each mix has a total volume of 50.0 ml. This is purposely done to ease the calculations. When the reagents are poured together, each one dilutes the other. In the 2nd table depicted the concentrations given at the head of each column are the pre-mix concentrations. To calculate concentrations after a dilution, use the following equation: final concentration = original conc x original volume divided by final volume. The 1st table is what I

Each mix has a total volume of 50.0 ml. This is purposely done to ease the calculations. When the reagents are poured together, each one dilutes the other. In the 2nd table depicted the concentrations given at the head of each column are the pre-mix concentrations. To calculate concentrations after a dilution, use the following equation: final concentration = original conc x original volume divided by final volume. The 1st table is what I??ve calculated so far the highlighted column marked H+ is what I can??t figure out. The calculations below the tables are how I calculated the I- and BrO3- I know how to calculate the final molarity, I just don??t know If I use H2O or HCl to calculate H+

Explanation / Answer

[H+] is only from HCl => H+ + Cl- (reaction is complete, HCl is a strong acid)

In 0.1 M HCl you have [H+] = 0.1 M and by dilution in 50 mL, the final concentration will be

[H+] = 0.1 M/5 = 0.02M. (as you have calculated for I- and BrO3-).

You are on the right way.

N.B. Ignore any dissociatiation of water. A strong (stronger) acid regresses the dissociation of a weak acid.

If you still have something not clear, write a comment to my answer.

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