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Electrolytic Dissociation

identify the ...

Question

identify the following compounds are ions as acids /bases CL- NH4 +,HSO4-

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Solution

When chlorine (in any form) is added to water, a weak acid called Hypochlorousacid is produced. It is this acid, not the chlorine, which gives water its ability to oxidize and disinfect.

NH4+, aka ammonium ion, is for all practical purposes an acid. It readily "gives off" a proton in the form of h+. NH4+ is the conjugate acid of the base, NH3, aka ammonia.

H2SO4 is a strong acid. When it looses a hydrogen, it becomes HSO4-, and gains a negative charge. HSO4- is the conjugate base of H2SO4 but it can still give its Hydrogen away, and thus it is a weak acid as well

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Q. Identify the following compounds/ ions as acids or bases: Cl^-^-, NH_4+^,^HSO₄^_-

Q. Identify the conjugate acids and bases in the following equation:

N H_{3} + H_{2} O ⇌ N H_{4}^{+} + O H^{-}

Q. Which of the following are Bronsted acids as well as Bronsted bases?

{N H}_{3}, {H S O}_{4}^{-}, H_{2} {S O}_{4}, {H C O}_{3}^{-}, H_{3} O

Q. The hydrogen sulfate or bisulfate ion,

H {S O}_{4}^{-}

, can act as either an acid or a base in water solution. In which of the following equations does

H {S O}_{4}^{-}

act as an acid?

Q. From the following reactions identify each of an Arrhenius acid or base, Bronsted-Lowry acid or base, or Lewis acid or base.
(A)

N a O H

N a O H \to {N a}^{+} + {O H}^{-}

H C l

H C l \to H^{+} + {C l}^{-}

N H_{3}

N H_{3} + H^{+} \to N H_{4}^{+}

N H_{4}^{+}

N H_{4}^{+} \to N H_{3} + H^{+}

{(C H_{3})}_{3} N :

{(C H_{3})}_{3} N : + B F_{3} \to {(C H_{3})}_{3} N : B F_{3}

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