Write net Bronsted equations and determine the equilibrium constants for the aci

Question

Write net Bronsted equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed.

Instructions:

Reactants Rxn: Acid(1) + Base(2) = Base(1) + Acid(2) K (three sig figs) hydrocyanic acid + sodium nitrite
hydrochloric acid + sodium hydroxide

hydrazoic acid + sodium hypochlorite

KHSO4 + NH3

H2CO3 + KHS

Write net Bronsted equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed. Instructions: Enter all substances in the order listed at the top of the column. Use a carot to indicate a superscript, but do nothing for subscripts. Use a hyphen + greater than (rightarrow) for yields. Click on the eye symbol to check your formatting. Report K to three sig figs even though it is good to only two. Group 1A and 7A ions (except fluoride) are spectator ions

Explanation / Answer

HF + CN- --> HCN + F-
HF is the proton donor, CN- is the proton acceptor, the base. That's because HCN is a much weaker acid than is HF.

K = [HCN] [F-] / [HF] [CN-]

Start with the Ka of HF, and the Kb of CN-

HF <==> H+ + F-
Ka = [H+] [F-] / [HF]
CN- + HOH <==> HCN + OH-
Kb = [HCN] [OH-] / [CN-]

Multiply Ka x Kb
[HCN] [F-] [H+] / [HF] [CN-] [OH-]

Therefore K equals Ka x Kb / Kw

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