equilibrium constant for this reaction:--
Fe^3+ (aq) + SCN- (aq) ---> Fe(SCN)^2+ (aq)
moles Fe(NO3)3 = 0.00300 M x 5.00 x 10^-3 L=1.50 x 10^-5
moles KSCN = 0.00300 M x 4.00 x 10^-3 L=1.2 x 10^-5
total volume = 5 + 4 + 3 = 12 mL = 0.012 L
[SCN-]= 1.2 x 10^-5 / 0.012 =0.00100 M
[Fe3+]= 1.50 x 10^-5 / 0.012 L=0.00125
at equilibrium
[Fe3+]= 0.00125 - 2.72 x 10^-4
[SCN-]= 0.00100 - 2.72 x 10^-4
so
[Fe3+]= 0.000978 M
[SCN-] = 0.000728 M
K = 2.72 x 10^-4 / ( 0.000978)( 0.000728)= 382
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