Adapted by Nelson Nuñez-Rodriguez
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By David W. Ball
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| QUESTION | ANSWER |
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1. Define Brønsted-Lowry acid. How does it differ from an Arrhenius acid? |
1. A Brønsted-Lowry acid is a proton donor. It does not necessarily increase the H+ concentration in water. |
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3. Write the dissociation of hydrogen bromide in water as a Brønsted-Lowry acid-base reaction and identify the proton donor and proton acceptor. |
3. HBr + H2O → H3O+ + Br−; PD: HBr; PA: H2O |
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5. Pyridine (C5H5N) acts as a Brønsted-Lowry base in water. Write the hydrolysis reaction for pyridine and identify the Brønsted-Lowry acid and Brønsted-Lowry base. |
5. C5H5N + H2O → C5H5NH+ + OH−; PD: H2O; PA: C5H5N |
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7. Identify the Brønsted-Lowry acid and Brønsted-Lowry base in this chemical equation. H3PO4 + OH− → H2PO4− + H2O |
7. BL acid: H3PO4; BL base: OH− |
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9. Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. HC2H3O2 + C5H5N → ? |
9. C2H3O2− and C5H5NH+ |
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11. What is the conjugate acid of H2O? of NH3? |
11. H3O+; NH4+ |
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13. What is the conjugate base of HSO4−? of H2O? |
13. SO42−; OH− |
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15. Identify the conjugate acid-base pairs in this reaction. HSO4− + PO43− → SO42− + HPO42− |
15. HSO4− and SO42−; PO43− and HPO42− |
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17. Identify the conjugate acid-base pairs in this reaction. NH3 + C6H5O− → C6H5OH + NH2− |
17. NH3 and NH2−; C6H5O− and C6H5OH |