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georgiabrown
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Homework Statement
In a lab, 40.3 mL Mn2+ is mixed with 5 mL H3PO4. 0.4g of potassium periodate is added. The flask is heated and then diluted to 100mL. The final solution prepared is a permanganate solution. Calculate the final molarity of the solution.
C Mn2+ = 0.06061 M (60.61 micrograms/ mL)
C H3PO4 = 15 M
V Mn2+ = 40.3 mL
V H3PO4 = 5 mL
M (Mn2+) = 54.94 g/mol
V final = 100mL
Homework Equations
C1V1=C2V2
2Mn2+ + 5IO4- + 3H2O ---> 2MnO4- + 5IO3- + 6H+
The Attempt at a Solution
(60.62 * 40.3 *10^-6) / (54.94 *0.100) = 4.45 *10^-4 M
The 10^-6 was used as a conversion factor from micrograms to grams.
I'm not sure if this is right, as it is not taking into account the H3PO4 added.
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