How do I figure out the [I-], [BrO3-], and the [H+] for a solution with flask 1

Question

How do I figure out the [I-], [BrO3-], and the [H+] for a solution with flask 1 and 2 mixed together, stiring for 630 seconds until it turned a dark blue with a temperature of 24 degrees Celsius after mixing.

Here are the contents of flask 1 and 2

The chemical equation is as follows.

I'm trying to fill out this table.

Table 1 Contents: Flask #1 always contains 10.0 mL Trial ! of 0.001 M Na2S203, and imL ofstarch |contents. Flask#2 solution, AND: 10 mL 0.010 M KI 10 mL 0.040 M KBrO 10 mL 0.10 M HCl 10 mL H20

Explanation / Answer

Concentration= moles/Volume of solution in L

When the two solution are mixed for the reaction then the total volume = 10 ml of Na2S2O3 + 1ml of starch solution + 10 ml KI + 10 ml H2O + 10 ml KBrO3 + 10 ml HCl

= 51 ml = 0.051 L

FOR MOLES OF DIFFERENT SPECIES

Moles of I-

Volume of KI used = 10 ml

Concentration of KI = 0.010 M . Now,0.010 M solution means

1000 ml of solution contain KI = 0.010 mol

10 ml solution contain KI = 0.010×10/1000 mol = 0.0001 mol

Now 1 KI has 1 K+ and 1 I-

So moles of I- =0.0001 mol

Concentration = [I-] = 0.0001 mol/0.051 L

=0.0020 mol/L =0.0020 M

Similarly,

Moles of KBrO3 = 0.040×10/1000 mol = 0.0004 mol

Moles of BrO3^-1 = 0.0004 mol

Concentration =[BrO3^-1]= 0.0004 mol/0.051 L = 0.0078 M

Moles of H+ (from 10 ml of 0.10M HCl)

=0.10×10/1000 mol =.0010 mol

concentration = [H+] = 0.0010 mol/ 0.051 L =0.0196 M

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