2. Consider each of the following: 1.0 M hydroxide will form a precipitate with
ID: 1042887 • Letter: 2
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2. Consider each of the following: 1.0 M hydroxide will form a precipitate with copper(II) cation but 6.0 M hydroxide will dissolve the solid. Explain using equations and Ksp and Kr arguments a. b. In the preliminary test with chloride (Section 1.1) there is a note stating that excess chloride ion must be avoided. Explain. 3. Consider the following situation involving aqueous ammonia and Cu+ a. List all species present in a 1.0 M ammonia solution. b. Is the pH of the ammonia solution acidic or basic? c. Looking at both the Ksp and Kr data given in Section 4.2, what reactions might occur when a 1.0 M ammonia is added to a Cu2 solution? d. If a solid precipitate is formed when 1.0 M ammonia is added to Cu2t, what has happened? What is the most likely product? Further addition of 1.0 M ammonia to the solution and precipitate from part d. does not dissolve the precipitate but addition of 15.0 M ammonia does. Explain. e. Lab 10 (Metal Cations) - Page 13 of 20Explanation / Answer
Cation NaCl Na2SO4 NaOH NH3(aq) Al3+ soluble Al3+, Cl- soluble Al3+, SO42- solid Al(OH)3 solid Al(OH)3 Ba2+ soluble Ba2+, Cl- solid BaSO4 soluble, Ba2+, OH- soluble, Ba2+, OH- Cu2+ soluble Cu2+, Cl- soluble Cu2+, SO42- solid Cu(OH)2 solid Cu(OH)2 Fe3+ soluble Fe3+, Cl- solid Fe2(SO4)3 soluble, Fe3+, SO42- solid Fe(OH)3 solid Fe(OH)3 Mn2+ soluble Mn2+, Cl- soluble Mn2+, SO42- solid Mn(OH)2 solid Mn(OH)2 Ni2+ soluble Ni2+, Cl- soluble Ni2+, SO42- solid Ni(OH)2 solid Ni(OH)2 Ag+ solid AgCl soluble [AgCl2-] solid Ag2SO4 solid AgOH solid AgOH soluble [Ag(NH3)2+]
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