Fill in the table below for the salts listed below. Follow similar formatting to

Question

Fill in the table below for the salts listed below. Follow similar formatting to the example 0 Pick out one of the conjugate acids that you identified from the table above and write out the equilibrium reaction with water. Write the K_a expression for this reaction. Pick out one of the conjugate bases that you identified from the table above and write out the equilibrium reaction with water. Write the K_b expression for this reaction. For the last example in the table (Ammonium Fluoride: NH_4 F), assume this compound completely ionizes in water. If you dissolve 1 mol of in 1 L of water, will the resulting solution be acidic or basic? NH_4^+ has a K_a of 5.8 Times 10^-10 F^- has a K_b of 1.5 Times 10^-11 Explain how you got to your conclusion or show calculations. Additional assumptions for calculations: x is small (no quadratic), all H^+ formed will react with OH^-.

Explanation / Answer

7)  NaNO2 dissociates almost completely:
NaNO2 (aq) --> Na+ (aq) + NO2- (aq)

The resulting ions could react with water:
Na+ + 2 H2O <--> NaOH (aq) + H3O+ (aq)
Since NaOH is a strong base, this reaction doesn't occur appreciably.

NO2- (aq) + H2O <--> HNO2 (aq) + OH- (aq)
The results of this reaction do appear because HNO2 is a weak acid. So the solution is basic (OH- in products)

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