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Please help me with this part of problem/ Pb2+(aq) + EDTA2-(aq) -> PbEDTA(aq) A 10.00 mL sample of the water from the holding tank requires 35.47 mL of 8.193 x 10-4 M EDTA to reach the end point. (A) What will be the molar concentration of lead(II) ions if you added a 10% excess...
A 10.00 mL sample of the water from the holding tank requires 35.47 mL of 8.193 x 10-4 M EDTA to reach the end point. (A) Based on this titration, what is the concentration of lead(II) ions in the holding tank? here, I try to start the problem by writing following equation: Pb2+(aq) + ...
have to find the molarity of an Unknown acid, but I was wondering how. I used this equation Cr2O7+14H+ + 6S2O3 = 2Cr + 3S4O6 + 7h2O We had to find the molarity of sodium thiosulphate which was 0.1M and K2Cr2O7 which was 0.02M for part A Part B This was an idometric titration the volumes used...
How would I find the RMM of the unknown metal if the molarity of HCl = 0.1 M , NaOH = 0.1 The Metal was dissolved in 80 cm3 of HCL and titrated against 22. 74 cm3 of NaOH. The mass of the metal was 0.0686 g.
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