Studying the Equilibrium of a slightly soluble Salt, Mg (OH)_2 What is the initi
ID: 488791 • Letter: S
Question
Studying the Equilibrium of a slightly soluble Salt, Mg (OH)_2 What is the initial, color and appearance of the introduces in wells B-1 and B-2? If a precipitate is press note that fact as well as the color of the precipitate what color change do you observe after adding concentrated HCL to well B-1? What color change do you observe adding Na _4 EDTA solution to well B-2? What is the initial color and appearance is present note that fact and the color of the precipitate what color change do you observe when you heat the from well B-3? What color change do you observe when you cool the pipet containing the heated from well B-4? What color change do you observe when you cool the pipet containing the heated from well B-3? What color change do you observe when you cool the pipet containing the heated from well B-4? Write the net ionic equation for the equilibrium involving Mg(OH) _2 in this experiment predict the direction in which the equilibrium should shift when you add concentrated HCL to the mixture in well B-1 briefly explain Briefly explain how your observation do or do not support your prediction in (24) predict the direction in which the equilibrium should shift when you add Na _4EDTA solution to the mixture in well B-2 breifly explain Briefly explain how your observation do or do not support your prediction in (26) Based on your observation of heating the mixture from well B-3, is the forward reaction endothermic or exothermic? Briefly explain Write the net ionic equation for the equilibrium again, but include heat in the equation this timeExplanation / Answer
IV solubility of Mg(OH)2
(15) the intial color of wells is white
(16) When HCl is added, the color changes to colorless
(17) blue color is formed when reacted with EDTA
(18) The initial color of wells would be white for precipitate presence
(19) colorless, precipitate dissolved
(20) cooling the mixture gives Mg(OH)2 precipitate back.
(23) color changes to white
(22) Color changes to transparent
(23) Net reaction,
Mg(OH)2 <==> Mg2+ + 2OH-
(24) Adding concentrated HCl, neutralize OH- and more of Mg(OH)2 dissolved.
(25) the solution becomes more tubid
(26) When Na4EDTA added, the Mg(OH)2 dissolves as Mg2+ complexes with EDTA
(27) The solution becomes more turbid
(28) The reaction is endothermic
(29) net ionic equation,
Mg2+ + EDTA <==> [MgEDTA]2-