A mixture is made by combining 14 mL of 1.9×10−3 M KSCN, 7.8 mL of 9.1×10−2...

A mixture is made by combining 14 mL of 1.9×10−3 M KSCN, 7.8 mL of 9.1×10−2 M Fe(NO3)3, and 11.7 mL of 0.475 M HNO3. Calculate the concentraion of Fe3+ in the solution.

Expert Solution

number of moles of KSCN = 1.9 * 10^-3 * 14 /1000 = 2.66 * 10^-5

number of moles of Fe(NO3)3 = 9.1*10^-2 * 7.8 /1000 = 7.098*10^-4

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

1mole of Fe(NO3)3 requirea 3 moles of KSCN

2.66 * 10^-5 moles of KSCN requires (1/3)*2.66 * 10^-5

= 8.867 * 10^-6

remaining moles of Fe(NO3)3 = 7.098*10^-4 - 8.867 * 10^-6 = 7.093 * 10^-4

concentration of Fe+3 = (7.093 * 10^-4) * 1000 / (14+7.8+11.7)

= 0.02117 M

queen_honey_blossom answered 2 years ago

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