Which of the following best explains why a semisoluble hydroxide salt like Zn(OH

Question

Which of the following best explains why a semisoluble hydroxide salt like Zn(OH)2 is more soluble in acidic or basic aqueous solutions than in pure water? O Because the Zn2+ ion can be both a Lewis acid and a Lewis base and can therefore react with both bases and acids. O Because hydroxide ion OH can accept a proton from an acid (to form H20) and donate a proton to a base (to form O2) and both of these processes are equally potential in aqueous solutions. O Because the actual chemical formula for zinc hydroxide is not merely Zn(OH2 but 2+ actually Zn(H20)2(OH)2 with acidic O-H bonds in the H20 molecules around the Zn ion, as well as the basic OH hydroxides. Hence the amphoteric nature of such hydroxide salts as "Zn(OH)2", which can therefore react with acids or with bases O I don't know the answer to this question because I was not in lecture that day...o. i was, I wasn't paying attention....nd I never got around to watching the lecture video either....

Explanation / Answer

Because the actual chemical formula for zinc hydroxide is not merely Zn (OH)2 but actually Zn(H2O)2(OH)2 with acidic O-H bonds in the H2O molecule around the Zn2+ , as well as the basic OH- hydroxides. Hene the amphoteric nature of such hydroxide salts as Zn(OH)2 which can therefore react with acids or with bases.

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