A mixture is made by combining 11.5 mL of 8.5×10−3 M KSCN, 6.3 mL of 3.7×10−2...

A mixture is made by combining 11.5 mL of 8.5×10−3 M KSCN, 6.3 mL of 3.7×10−2 M Fe(NO3)3, and 10.4 mL of 0.397 M HNO3. Calculate the concentraion of Fe3+ in the solution.

Expert Solution

number of moles of KSCN = ((8.5 * 10^-3) * 11.5) / 1000 = 9.775 * 10^-5

number of moles of Fe(NO3)3 = ((3.7*10^-2)*10.4) / 1000 = 3.848 * 10^-4

3 KSCN (aq) + Fe(NO3)3 (aq) ---------> Fe(SCN)3 (s) + 3 KNO3 (aq)

3 mole of KSCN requires 1 mole of Fe(NO3)3

9.775 * 10^-5 moles of KSCN requires (1/3) * 9.775 * 10^-5

= 3.2583 * 10^-5 moles

remaining moles of Fe(NO3)3 = (3.848 * 10^-4) - (3.2583 * 10^-5) = 3.5222 * 10^-4

concentration of Fe+3 = (3.5222 * 10^-4) * (1000 / (11.5 + 6.3 + 10.4))

= 0.01249 M

queen_honey_blossom answered 2 years ago

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