Using Le Chatelier's principle, at equilibrium, how would ion concentrations change for the following balanced reactions after adding more of something (given below)? Fe+3 + SCN-1 ↔ Fe(SCN)+2 a. add Fe(NO3)3 b. add KSCN c. add NaOH Ni+2 + 6NH3 ↔ Ni(NH3)6+2 d. add HCl e. add NH4OH HInaq + H2O ↔ H3O+ + Inaq-1 f. add HCl g. add NaOH
Using Le Chatelier's principle, at equilibrium, how would ion concentrations change for the following balanced reactions after adding more of something (given below)?
Fe+3 + SCN-1 ↔ Fe(SCN)+2
a. add Fe(NO3)3
b. add KSCN
c. add NaOH
Ni+2 + 6NH3 ↔ Ni(NH3)6+2
d. add HCl
e. add NH4OH
HInaq + H2O ↔ H3O+ + Inaq-1
f. add HCl
g. add NaOH
We konw that as per Le Chatelier's Principle, the system will react to minimize the stress , and attend equillibrium state.
As per given reaction
Fe+3 + SCN-1 ↔ Fe(SCN)+2
A) Add Fe(NO3)3
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- Fe(NO3)3 Fe +3 + 3(NO3)-1
Here in above reaction concentration of Fe +3 increases when we add Fe(NO3)3 in main reaction.
Acoording to Le Chatelier's Principle equilibrium shifts right hand side. So in reaction product will be formed more that is Fe(SCN)+2
B. Add KSCN
- KSCN K+ + SCN -1 Here in above reaction concentration of SCN -1 also increases when we add kscn in mailn reaction As SCN -1 increases reactant will be increases equilibrium shift towards right hand side and product will be more formed.
C. Add NaOH
Adittion of NaOH it will form Fe(OH)3 as precipitates and intesity of that Fe(SCN)+2 complex will decreased so and equilibrium of the reaction will shif left hand side means towords reactant.
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