the following equilibrium reaction occurs in aqueous solutionswhen 0.1 M KSCN is mixed with 0.1 M
Fe(NO3)3. Fe(SCN)2+(aq) <----> Fe3+(aq) + SCN-(aq)
Predict whether the following statements (in relation to theabove equilibrium reaction in aqueous solution) are \"True\" or\"False\".
1.Addition of 0.1 M NaNO3 does not have as much influence on theposition of the equilibrium.
2.Addition of 0.1 M KSCN does not affect the position of theequilibrium.
3.Addition of 0.1 M KNO3 causes the equilibrium to shift to theleft (reactant side).
4.Addition of 0.1 M Fe(NO3)3 causes the equilibrium to shift tothe right (product side).
5.In the addition of 6 M NaOH, OH- reacts with Fe3+ to formslightly soluble Fe(OH)3.
6.Addition of 0.1 M LiSCN will have a similar effect on theposition of the equilibrium as the addition of 0.1 M KSCN.
7.Addition of 6 M NaOH causes the equilibrium to shift to theleft because NaOH is a strong base and breaks the bonds inFe(SCN)2+
