Now predict what will happen if you add AgNO3 (aq) to the solution that is at eq
ID: 587403 • Letter: N
Question
Now predict what will happen if you add AgNO3 (aq) to the solution that is at equilibrium instead of NaCI (aq) Remember that AgNO3 (aq) consists of Ag (aq) and NO3 (aq) ions, and that Ag (aq) ions react with Cl (aq) ions to form the insoluble solid AgCl(s). This effectively removes CI (aq) ions from solution. Part E The equilibrium will shift toward Please Choose, upon addition of AgNO3 (aq). Submit My Answers Give Up Part F The concentration of Co(H2O (aa) will Please Choose 4 upon addition of AgN03(aa) equilibrium mixture. Submit My Answers Give Up Part G The concentration of [CoCla2 (a) will Please Choose upon addition of AgNOs(aq) equilibrium mixture. Submit My Answers Give Up Part H The color of the solution will become more Please Choose Submit My Answers Give UpExplanation / Answer
At equilibrium
Co(H2O)6 + 4Cl- ========= Co(Cl)42- + (H2O)6
Equilibrium expresion is
Kc = [CoCl4][H2O] / [Co(H2O)62+][Cl-]
(E) AgNO3 is ionic so it is soluble and dissciate in Ag+ and NO3 then the Ag+ ions and Cl- ions will mix together in the reactants side means decrease the concentration of Cl- in reactant
AgNO3(aq) --> Ag+ + NO3-
Ag+ + Cl- --> AgCl(s)
AgNO3(aq) + Cl- --> AgCl(s) + NO3-
According to Lechatelier's Princilple "A dynamic equilibrium tends to respond as to remove the effect of any change in the conditions that affect the equilibrium." (From any text book)
So adding on AgNO3 in the reactant Equilibrium shift will shift towards the Reactant side means left side.
(F) concentraion of Co(H2O)6 increase because equilibrium shift left side with same reason.
(G) AgNO3 does not affect the concentration of Co(Cl)42- because of no reaction between them. It will be same.
(H) The colour become more like Co(H2O)6 ... because it has high concentration in the reaction with same reason as given in the E part.
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.