SOLUTION: Acids and bases worksheet - Studypool - Free Printable
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Step-by-step solution for: SOLUTION: Acids and bases worksheet - Studypool
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Show Answer Key & Explanations
Step-by-step solution for: SOLUTION: Acids and bases worksheet - Studypool
You're absolutely correct in your labeling! Let's go through each reaction step-by-step to explain *why* each species is labeled as an acid or a base according to the Brønsted-Lowry theory.
Recap of Brønsted-Lowry Theory:
* An acid is a proton (H⁺) donor.
* A base is a proton (H⁺) acceptor.
* In any reversible reaction, the species on the left that donates H⁺ becomes its conjugate base on the right. The species on the left that accepts H⁺ becomes its conjugate acid on the right.
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* Left Side: One water molecule (`H₂O`) acts as an acid because it *donates* a proton (H⁺) to the other water molecule.
* Left Side: The other water molecule (`H₂O`) acts as a base because it *accepts* the proton (H⁺).
* Result: The donating `H₂O` becomes `OH⁻` (its conjugate base). The accepting `H₂O` becomes `H₃O⁺` (its conjugate acid).
* Your Labeling: You correctly labeled the first `H₂O` as "base" and the second `H₂O` as "acid". *(Note: The order written is `H₂O + H₂O`, so the first one shown is acting as the base, accepting the proton from the second one, which is acting as the acid. Your arrow shows H⁺ moving from the second `H₂O` to the first `H₂O`, which matches this interpretation.)*
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* Left Side: Sulfuric acid (`H₂SO₄`) acts as an acid because it *donates* a proton (H⁺) to the hydroxide ion (`OH⁻`).
* Left Side: Hydroxide ion (`OH⁻`) acts as a base because it *accepts* the proton (H⁺).
* Result: `H₂SO₄` loses a proton to become `HSO₄⁻` (its conjugate base). `OH⁻` gains a proton to become `H₂O` (its conjugate acid).
* Your Labeling: You correctly labeled `H₂SO₄` as "acid" and `OH⁻` as "base". Your arrow shows H⁺ moving from `H₂SO₄` to `OH⁻`.
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* Left Side: Hydrogen sulfate ion (`HSO₄⁻`) acts as an acid because it *donates* a proton (H⁺) to water (`H₂O`).
* Left Side: Water (`H₂O`) acts as a base because it *accepts* the proton (H⁺).
* Result: `HSO₄⁻` loses a proton to become `SO₄²⁻` (its conjugate base). `H₂O` gains a proton to become `H₃O⁺` (its conjugate acid).
* Your Labeling: You correctly labeled `HSO₄⁻` as "acid" and `H₂O` as "base". Your arrow shows H⁺ moving from `HSO₄⁻` to `H₂O`.
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* Left Side: Hydronium ion (`H₃O⁺`) acts as an acid because it *donates* a proton (H⁺) to the hydroxide ion (`OH⁻`).
* Left Side: Hydroxide ion (`OH⁻`) acts as a base because it *accepts* the proton (H⁺).
* Result: `H₃O⁺` loses a proton to become `H₂O` (its conjugate base). `OH⁻` gains a proton to become `H₂O` (its conjugate acid). Both products are water molecules.
* Your Labeling: You correctly labeled `OH⁻` as "base" and `H₃O⁺` as "acid". Your arrow shows H⁺ moving from `H₃O⁺` to `OH⁻`.
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* Left Side: Ammonia (`NH₃`) acts as a base because it *accepts* a proton (H⁺) from water (`H₂O`).
* Left Side: Water (`H₂O`) acts as an acid because it *donates* a proton (H⁺) to ammonia.
* Result: `NH₃` gains a proton to become `NH₄⁺` (its conjugate acid). `H₂O` loses a proton to become `OH⁻` (its conjugate base).
* Your Labeling: You correctly labeled `NH₃` as "base" and `H₂O` as "acid". Your arrow shows H⁺ moving from `H₂O` to `NH₃`.
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Conclusion:
Your answers for all five reactions are perfectly correct according to the Brønsted-Lowry definition. You accurately identified the proton donor (acid) and proton acceptor (base) in each case and correctly indicated the direction of proton transfer with your arrows. Great job!
Recap of Brønsted-Lowry Theory:
* An acid is a proton (H⁺) donor.
* A base is a proton (H⁺) acceptor.
* In any reversible reaction, the species on the left that donates H⁺ becomes its conjugate base on the right. The species on the left that accepts H⁺ becomes its conjugate acid on the right.
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Reaction 1: `H₂O + H₂O ⇌ H₃O⁺ + OH⁻`
* Left Side: One water molecule (`H₂O`) acts as an acid because it *donates* a proton (H⁺) to the other water molecule.
* Left Side: The other water molecule (`H₂O`) acts as a base because it *accepts* the proton (H⁺).
* Result: The donating `H₂O` becomes `OH⁻` (its conjugate base). The accepting `H₂O` becomes `H₃O⁺` (its conjugate acid).
* Your Labeling: You correctly labeled the first `H₂O` as "base" and the second `H₂O` as "acid". *(Note: The order written is `H₂O + H₂O`, so the first one shown is acting as the base, accepting the proton from the second one, which is acting as the acid. Your arrow shows H⁺ moving from the second `H₂O` to the first `H₂O`, which matches this interpretation.)*
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Reaction 2: `H₂SO₄ + OH⁻ ⇌ HSO₄⁻ + H₂O`
* Left Side: Sulfuric acid (`H₂SO₄`) acts as an acid because it *donates* a proton (H⁺) to the hydroxide ion (`OH⁻`).
* Left Side: Hydroxide ion (`OH⁻`) acts as a base because it *accepts* the proton (H⁺).
* Result: `H₂SO₄` loses a proton to become `HSO₄⁻` (its conjugate base). `OH⁻` gains a proton to become `H₂O` (its conjugate acid).
* Your Labeling: You correctly labeled `H₂SO₄` as "acid" and `OH⁻` as "base". Your arrow shows H⁺ moving from `H₂SO₄` to `OH⁻`.
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Reaction 3: `HSO₄⁻ + H₂O ⇌ SO₄²⁻ + H₃O⁺`
* Left Side: Hydrogen sulfate ion (`HSO₄⁻`) acts as an acid because it *donates* a proton (H⁺) to water (`H₂O`).
* Left Side: Water (`H₂O`) acts as a base because it *accepts* the proton (H⁺).
* Result: `HSO₄⁻` loses a proton to become `SO₄²⁻` (its conjugate base). `H₂O` gains a proton to become `H₃O⁺` (its conjugate acid).
* Your Labeling: You correctly labeled `HSO₄⁻` as "acid" and `H₂O` as "base". Your arrow shows H⁺ moving from `HSO₄⁻` to `H₂O`.
---
Reaction 4: `OH⁻ + H₃O⁺ ⇌ H₂O + H₂O`
* Left Side: Hydronium ion (`H₃O⁺`) acts as an acid because it *donates* a proton (H⁺) to the hydroxide ion (`OH⁻`).
* Left Side: Hydroxide ion (`OH⁻`) acts as a base because it *accepts* the proton (H⁺).
* Result: `H₃O⁺` loses a proton to become `H₂O` (its conjugate base). `OH⁻` gains a proton to become `H₂O` (its conjugate acid). Both products are water molecules.
* Your Labeling: You correctly labeled `OH⁻` as "base" and `H₃O⁺` as "acid". Your arrow shows H⁺ moving from `H₃O⁺` to `OH⁻`.
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Reaction 5: `NH₃ + H₂O ⇌ NH₄⁺ + OH⁻`
* Left Side: Ammonia (`NH₃`) acts as a base because it *accepts* a proton (H⁺) from water (`H₂O`).
* Left Side: Water (`H₂O`) acts as an acid because it *donates* a proton (H⁺) to ammonia.
* Result: `NH₃` gains a proton to become `NH₄⁺` (its conjugate acid). `H₂O` loses a proton to become `OH⁻` (its conjugate base).
* Your Labeling: You correctly labeled `NH₃` as "base" and `H₂O` as "acid". Your arrow shows H⁺ moving from `H₂O` to `NH₃`.
---
Conclusion:
Your answers for all five reactions are perfectly correct according to the Brønsted-Lowry definition. You accurately identified the proton donor (acid) and proton acceptor (base) in each case and correctly indicated the direction of proton transfer with your arrows. Great job!
Parent Tip: Review the logic above to help your child master the concept of lewis acid and base worksheet.
