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) acetic acid + ammonia hydrochloric acid + sodium hydroxide formic acid (HCHO2) + sodium nitrite KHCO3 + KCN H2SO3 + K2SO4

Explanation / Answer

q1.

CH3COOH(aq) + NH3(aq) --> NH4+(aq) + CH3COO-(aq)

Ka and Kb are involved s

Knet = Ka*Kb

q2.

HCl + NaNO2(aq) --> H+ and NO2- are present

so

H+(aq) + NO2-2(aq) --< HNO2(aq), which is the inverse of a Ka of HNO2

so

K = 1/Ka

q3.

HCOOH + NaNO2 --> HCOOH + NO2-

so

HCOOH + NO2- --> formic acid is stornger acid so

HCOO- + HNO2 will be the solution

Ka f HCOO and 1/Ka for HNO2

Ktotal = Ka(formic) / Ka(nitrite)

Q4

KHCO3 --> K+ + HCO3-

KCN --> K+ + CN-

so

HCO3- and CN- are present

HCN is weaker acid so:

HCN and CO3-2

HCN Ka = 9.21

HCO3- Ka = 10.32

H2CO3 = 6.37

clearly, H2CO3 > HCN > HCO3-

so HCN is nt likely to form

CN- + HCO3- remais constant

Finally

H2SO3 + K2SO4

H2SO3 + 2K+ + SO4-2

this is simply Ka for H2SO3

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