10. As you saw in Model 1, all Arthenius bases in Model I have an OH^- ion in their chemical formulas. Write a balanced chemical reaction for the reaction of HCl(aq) with OH^-(aq) to illustrate that the hydroxide ion is also a Bronsted -Lowry base. 11. If you reverse Reaction 1 in Model 2, the following reaction is obtained. H_(3)O^-(aq)+Cl^-(aq)leftharpoons HCl(aq)+H_(2)O(l) a. For the reaction above, which reactant is acting like a Brensted-Lowry acid? How can you tell? b. For the reaction above, which reactant is acting like a Bronsted-Lowry base?How can you tell? 12. Write the reverse reactions for Reactions 2 and 3 in Model 2. Label the Bronsted-Lowry acid and base reactants for each reaction. Reaction 2 Reaction 3

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10. As you saw in Model 1, all Arthenius bases in Model I have an OH^- ion in their chemical formulas. Write a balanced chemical reaction for the reaction of HCl(aq) with OH^-(aq) to illustrate that the hydroxide ion is also a Bronsted -Lowry base. 11. If you reverse Reaction 1 in Model 2, the following reaction is obtained. H_(3)O^-(aq)+Cl^-(aq)leftharpoons HCl(aq)+H_(2)O(l) a. For the reaction above, which reactant is acting like a Brensted-Lowry acid? How can you tell? b. For the reaction above, which reactant is acting like a Bronsted-Lowry base?How can you tell? 12. Write the reverse reactions for Reactions 2 and 3 in Model 2. Label the Bronsted-Lowry acid and base reactants for each reaction. Reaction 2 Reaction 3

Answer 1

10. The balanced chemical reaction for the reaction of \( HCl(aq) \) with \( OH^{-}(aq) \) is: \[ HCl(aq) + OH^{-}(aq) \rightarrow H_{2}O(l) + Cl^{-}(aq) \] 11. a. In the reaction \( H_{3}O^{+}(aq) + Cl^{-}(aq) \rightleftharpoons HCl(aq) + H_{2}O(l) \), the reactant acting as a Bronsted-Lowry acid is \( H_{3}O^{+}(aq) \) because it donates a proton to form \( HCl(aq) \). b. The reactant acting as a Bronsted-Lowry base is \( Cl^{-}(aq) \) because it accepts a proton to form \( HCl(aq) \). 12. The reverse reactions for Reactions 2 and 3 in Model 2 are not provided in the question. To label the Bronsted-Lowry acid and base reactants for each reaction, the original reactions would be needed. Without the details of Reactions 2 and 3, it is not possible to write the reverse reactions or identify the Bronsted-Lowry acid and base.

Answer 2

## Step 1: Identify the reactants for the balanced chemical reaction between \( HCl(aq) \) and \( OH^{-}(aq) \). ## Step 2: Combine the \( H^{+} \) ion from \( HCl \) with the \( OH^{-} \) ion to form water (\( H_{2}O \)). ## Step 3: Write the remaining ion (\( Cl^{-} \)) as the other product, which will be part of the salt. ## Step 4: Balance the chemical equation to ensure the number of atoms of each element is the same on both sides. ### \( HCl(aq) + OH^{-}(aq) \rightarrow H_{2}O(l) + Cl^{-}(aq) \) ## Step 5: For question 11a, identify the reactant that donates a proton in the given reaction. ## Step 6: For question 11b, identify the reactant that accepts a proton in the given reaction. ## Step 7: For question 12, write the reverse reactions for Reactions 2 and 3 and identify the Bronsted-Lowry acid and base for each.

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