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The Acid Dissociation Constant K_a Equals 1 $\times$ 10^-2 for HSO₄^- and Is 5

Question 60

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The acid dissociation constant K_a equals 1.26 $\times$ 10^-2 for HSO₄^- and is 5.6 $\times$ 10^-10 for NH₄⁺.Which statement about the following equilibrium is correct?
HSO₄^-(aq) + NH₃(aq) $The acid dissociation constant Ka equals 1.26 \times 10-2 for HSO4- and is 5.6 \times 10-10 for NH4+.Which statement about the following equilibrium is correct? HSO4-(aq) + NH3(aq) SO42-(aq) + NH4+(aq) A) The reactants will be favored because ammonia is a stronger base than the sulfate anion. B) The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion. C) Neither reactants or products will be favored because all of the species are weak acids or bases. D) The initial concentrations of the hydrogen sulfate ion and ammonia must be known before any prediction can be made. E) This reaction is impossible to predict,since the strong acid and the weak base appear on the same side of the equation.$
SO₄^2-(aq) + NH₄⁺(aq)

A) The reactants will be favored because ammonia is a stronger base than the sulfate anion.
B) The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion.
C) Neither reactants or products will be favored because all of the species are weak acids or bases.
D) The initial concentrations of the hydrogen sulfate ion and ammonia must be known before any prediction can be made.
E) This reaction is impossible to predict,since the strong acid and the weak base appear on the same side of the equation.

The Acid Dissociation Constant Ka Equals 1 ×\times× 10-2 for HSO4- and Is 5

Multiple Choice

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The Acid Dissociation Constant K_a Equals 1 $\times$ 10^-2 for HSO₄^- and Is 5

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