I have to do an identity lab on these tomorrow and I'm trying to look up certain properties of these solutions. I was just wondering if any of these would be considered acids.
Barium chloride,
copper (II) sulfate
lead (II) nitrate
magnesium nitrate
nickel (II) sulfate
zinc (II) chloride
2006-10-17 11:26:50 · 3 answers · asked by Cree 2 in Education & Reference ➔ Homework Help
No, none are acids.
Barium chloride is neutral because one all +1 and +2 metals are neutral, as well as conjugate bases of strong acids (Cl- is the CB of HCl)
Same goes for the Pb(NO3)2, MgNO3, and ZnCl2.
Your sulfates will be weakly basic, because sulfate is the conjugate base of HSO4-, a weak acid. (Strictly speaking, this doesn't exist, but it is helpful in explaining the equilibrium of the sulfate, where it has a tendency to donate electrons)
2006-10-17 11:37:42 · answer #1 · answered by kickapookidonthefritz 2 · 0⤊ 0⤋
What you have to look for is the ionic charge carried by these compounds. If the ion charge is negative, then they are acidic. If the ion charge is positive, then they are basic. That doesn't mean that we would necessarily call them an acid but that the compounds are acidic in nature.
2006-10-17 18:37:33 · answer #2 · answered by rac 7 · 1⤊ 0⤋
considering none of them contain the world ACID, no none are acids
2006-10-17 18:30:40 · answer #3 · answered by Anonymous · 1⤊ 0⤋