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Write a balanced net ionic equation for each of the following acid- base reactions in water.  a. acetic acid with strontium hydroxide  b. diethylamine , with sulfuric acid  c. aqueous hydrogen cyanide with sodium hydroxide

Write a balanced net ionic equation for each of the following acid- base reactions in water.  a. acetic acid with strontium hydroxide  b. diethylamine , with sulfuric acid  c. aqueous hydrogen cyanide with sodium hydroxide

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Write a balanced net ionic equation for each of the following acid- base reactions in water.

 a. acetic acid with strontium hydroxide

 b. diethylamine , with sulfuric acid

 c. aqueous hydrogen cyanide with sodium hydroxide

Please refer to the picture. Thank you.

 

 

Equations for Acid-Base Reactions When an acidic water solution is mixed with a basic water solution, an acid-base reaction takes place. The nature of the reaction and hence the equation written for it depend on whether the acid and base involved are strong or weak. 1. Strong acid- strong base. Consider what happens when a solution of a strong acid such as HNO3 is added to a solution of a strong base such as NaOH. Because HNO3 is a strong acid, it is completely converted to H* and NO3 ions in solution. Similarly, with the strong base NaOH, the solution species are the Nat and OH ions. When the solutions are mixed, the H* and OH ions react with each other to form H20 molecules. This reaction, referred to as neutralization, is represented by the net ionic equation H*(aq) OH (aq) → H2O The Na* and NO; ions take no part in the reaction and so do not appear in the equation. It follows that the neutralization equation written above applies to any strong acid- strong base reaction. 2. Weak acid-strong base. when a strong base such as NaOH is added to a solution of weak acid, HB, a two -step reaction occurs. The first step is the ionization of the HB molecule to H* and B ions; the second is the neutralization of the H* ions produced in the first step by the OH ions of the NaOH solution. (1) HB(aq) → H*(aq) The equation for the overall reaction is obtained by adding the two equations and cancelling H* ions: HB(aq) B'(aq) (2) H*(aq) + OH(aq) → H2O OH (aq) → B'(aq) H2O 3. Strong acid-weak base. consider what happens when an aqueous solution of a strong acid like HCl is added to an aqueous solution of ammonia, NH3. We consider the reaction to take place in two steps. The first step is the reaction of NH3 with H20 to form NH4* and OH ions. Then, in the second step, the H* ions of the strong acid neutralize the OH ions formed in the first step. OH (aq) (2) H* (ag) + OH (aq) The overall equation is H20 + NH4*(aq) → NH4*(aq) (1) NH3(aq) H*(aq) NH3(aq) Example: Write a net ionic equation for each of the following reactions in dilute water solution. b. ammonia with perchloric acid (HCIO4) a. hypochlorous acid ( HCIO) and calcium hydroxide c. hydroiodic acid (HI) with sodium hydroxide Solution: CIO (aq) a. HCIO(aq) b. H*(aq) OH'(aq) NH3(aq) → H20 → NH4*(aq) + c. H*(aq) OH (aq) H2O
Transcribed Image Text:Equations for Acid-Base Reactions When an acidic water solution is mixed with a basic water solution, an acid-base reaction takes place. The nature of the reaction and hence the equation written for it depend on whether the acid and base involved are strong or weak. 1. Strong acid- strong base. Consider what happens when a solution of a strong acid such as HNO3 is added to a solution of a strong base such as NaOH. Because HNO3 is a strong acid, it is completely converted to H* and NO3 ions in solution. Similarly, with the strong base NaOH, the solution species are the Nat and OH ions. When the solutions are mixed, the H* and OH ions react with each other to form H20 molecules. This reaction, referred to as neutralization, is represented by the net ionic equation H*(aq) OH (aq) → H2O The Na* and NO; ions take no part in the reaction and so do not appear in the equation. It follows that the neutralization equation written above applies to any strong acid- strong base reaction. 2. Weak acid-strong base. when a strong base such as NaOH is added to a solution of weak acid, HB, a two -step reaction occurs. The first step is the ionization of the HB molecule to H* and B ions; the second is the neutralization of the H* ions produced in the first step by the OH ions of the NaOH solution. (1) HB(aq) → H*(aq) The equation for the overall reaction is obtained by adding the two equations and cancelling H* ions: HB(aq) B'(aq) (2) H*(aq) + OH(aq) → H2O OH (aq) → B'(aq) H2O 3. Strong acid-weak base. consider what happens when an aqueous solution of a strong acid like HCl is added to an aqueous solution of ammonia, NH3. We consider the reaction to take place in two steps. The first step is the reaction of NH3 with H20 to form NH4* and OH ions. Then, in the second step, the H* ions of the strong acid neutralize the OH ions formed in the first step. OH (aq) (2) H* (ag) + OH (aq) The overall equation is H20 + NH4*(aq) → NH4*(aq) (1) NH3(aq) H*(aq) NH3(aq) Example: Write a net ionic equation for each of the following reactions in dilute water solution. b. ammonia with perchloric acid (HCIO4) a. hypochlorous acid ( HCIO) and calcium hydroxide c. hydroiodic acid (HI) with sodium hydroxide Solution: CIO (aq) a. HCIO(aq) b. H*(aq) OH'(aq) NH3(aq) → H20 → NH4*(aq) + c. H*(aq) OH (aq) H2O
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