Suppose 1.01 g of FeCl_3 is placed in a 10.0 ml volumetric flask, water is added

Question

Suppose 1.01 g of FeCl_3 is placed in a 10.0 ml volumetric flask, water is added, the mixture is shaken to dissolve the solid, and then water is added to the calibration mark of the flask. Calculate the molarity of each ion present in the solution. Calculate the new molarity that results when each of the following solution is diluted to a final total volume of 1.00 L? For convenience, one form of sodium hydroxide that is sold commercially is the saturated solution. This solution is 19.4 M, which is approximately 50% by m ass sodium hydroxide. What volume of this solution would be needed to prepare 3.5 L of 3.00 M NaOH solution?

Explanation / Answer

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7)
Mass of FeCl3 = 1.01 g
Molar Mass of FeCl3 = 162.2 g/mol
Number of moles of FeCl3 = mass / molar mass
                                                       = 1.01 / 162.2
                                                       = 6.23*10^-3 mol

V = 10 mL = 0.01 L

M = number of moles / volume
      = (6.23*10^-3 ) / 0.01
      = 0.623 M

This is concentration of FeCl3

FeCl3 ----> Fe3+   +   3Cl-
[Fe3+] = [FeCl3] = 0.623 M
[Cl-] = 3*[FeCl3] = 3*0.623 = 1.87 M

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