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2. Write the net ionic equation for each Bronsted-Lowry acid-base reaction. Remember, this type of reaction is a single-proton transfer reaction. a. HF(aq) + NH3(aq) b. NaHSO,(aq) + NaOH(aq) с. НС-Н,О-(aq) + NaCN(aq) d. H3PO4(aq) + NażCO3(aq) е. NH,CI(aq) + КоН(ад)

2. Write the net ionic equation for each Bronsted-Lowry acid-base reaction. Remember, this type of reaction is a single-proton transfer reaction. a. HF(aq) + NH3(aq) b. NaHSO,(aq) + NaOH(aq) с. НС-Н,О-(aq) + NaCN(aq) d. H3PO4(aq) + NażCO3(aq) е. NH,CI(aq) + КоН(ад)

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Help with 2d and 2e please

**Exercise 2: Writing Net Ionic Equations for Bronsted-Lowry Acid-Base Reactions** **Objective:** Write the net ionic equation for each Bronsted-Lowry acid-base reaction. Remember, this type of reaction involves a single-proton transfer. a. \( \text{HF(aq)} + \text{NH}_3\text{(aq)} \) b. \( \text{NaHSO}_4\text{(aq)} + \text{NaOH(aq)} \) c. \( \text{HC}_2\text{H}_3\text{O}_2\text{(aq)} + \text{NaCN(aq)} \) d. \( \text{H}_3\text{PO}_4\text{(aq)} + \text{Na}_2\text{CO}_3\text{(aq)} \) e. \( \text{NH}_4\text{Cl(aq)} + \text{KOH(aq)} \) These equations involve identifying the acids and bases according to Bronsted-Lowry theory and determining the products formed as a result of proton transfer.
Transcribed Image Text:**Exercise 2: Writing Net Ionic Equations for Bronsted-Lowry Acid-Base Reactions** **Objective:** Write the net ionic equation for each Bronsted-Lowry acid-base reaction. Remember, this type of reaction involves a single-proton transfer. a. \( \text{HF(aq)} + \text{NH}_3\text{(aq)} \) b. \( \text{NaHSO}_4\text{(aq)} + \text{NaOH(aq)} \) c. \( \text{HC}_2\text{H}_3\text{O}_2\text{(aq)} + \text{NaCN(aq)} \) d. \( \text{H}_3\text{PO}_4\text{(aq)} + \text{Na}_2\text{CO}_3\text{(aq)} \) e. \( \text{NH}_4\text{Cl(aq)} + \text{KOH(aq)} \) These equations involve identifying the acids and bases according to Bronsted-Lowry theory and determining the products formed as a result of proton transfer.
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Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a substance that gives H+ ions and the base is a substance that accepts the H+ ions. 

The species which are differing by the H+ are called conjugate acid-base pairs.

Conjugate base = Conjugate acid - H+Conjugate acid = Conjugate base + H+

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