When solutions of yellow Fe+3(aq) and Fe+3(aq) and colorless SCN (aq) are mixed, a red complex ion forms
Fe^3+(aq) + SCN^- (aq) = Fe(SCN)^2+ (aq)

a) What change would be observed when a solution of Fe+3(aq) is added to this equilibrium
containing an excess of SCN-(aq)?

b) What change to the solution color would be observed when a solution of Ag+ (aq) is added to
equilibrium containing an excess of SCN (aq)? (Hint Agt forms a precipitate with SCN)

c) Explain how these observations are consistent with Le Chatlier's Principle.

Answer and explanantion:

PART A

If you add Fe+3 ions, the shift goes toward products, since there is excess of reactants . So, the solutoin gets more RED . It is consistent, since more reagent will favour more produciton of FeSCN, therefore, the red color must increase

PART B

If you add Ag+ ions, then you will have AgSCN production

SCN- decreases, so the reagents decrease . The reaction stops productino of FeSCN complex, and the complex starts formid reactants , so the color goes more YELLOW .

PART C

This is consistent, since Q = [products] / [reactants] constant must be kept.

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.  

solute : a solute is a substance that is dissolved in another substance is known as a solvent. it is mixed with a special mixture know as homogeneous mixture.

solvent: a solvent is a substance that dissolved a solute, which results in a solution is known as solvent.