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:

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 (->) 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.

Reactants Rxn: Acid(1) + Base(2) = Base(1) + Acid(2) K (three sig figs) hydrofluoric acid + potassium cyanide perchloric acid + sodium cyanide nitrous acid + sodium fluoride KHCO3 + KCN H2S + KClO

Explanation / Answer

HF + KCN = KF + HCN

acid     base base(1) acid (2)

K = Ka(HF)/Ka(HCN) = (6.8*10^-4)/ (6.2*10^-10) = 1.096*10^6

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HClO4 + NaCN <==> HCN + NaClO4

acid        base            acid      base

K = K(HClO4)/K(HCN) = 1*10^7/ 6.2*10^-10 =0.16 *10^17

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KHCO3 + KCN <==> HCN + K2CO3

K = Ka (KHCO3)/Ka(HCN) = 5.6*10^-11/6.2*10^-10 = 0.09

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H2S + KClO <==> HClO + KHS

K = K(H2S)/K(HCLO) = 5.7*10^-8/ 3*10^-8 = 1.9

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