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The concentration of Cu+ in a solution is determined by titrating it with a 0.1621 M...

The concentration of Cu+ in a solution is determined by titrating it with a 0.1621 M permanganate solution. The balanced net ionic equation for the reaction is:

MnO4-(aq) + 5Cu+(aq) + 8H3O+(aq) Mn2+(aq) + 5Cu2+(aq) + 12H2O(l)

In one experiment, 18.21 mL of the 0.1621-M permanganate solution is required to react completely with 25.00 mL of the Cu+ solution. Calculate the concentration of the Cu+ solution.

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Answer #1

Equation MnO^(aq) +5Cu(a) 8H No of moles of MnO-18.21 mLx Mn2 (aq) + 5Cu2 (aq)+ 12H20() 1し 1000 mL .. 0.1621 mo! MnOǐ 1L = 0.002952 mol MnO 5 mol Cu 1 mol MnO No of moles of Cu+ required 0.002952 mol MnO、< = 0.01476 mol Cu 1L Volume of Cu+ solution 25.00 mL×- . 1000 mL = 0.02500 L 0.01476 mol Cu 0.02500 L Concentrati on of Cu- = 0.5904 M

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