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Chapter 17

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Chapter 17. 2). a) HCl and CH3COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH2PO4 and Na2HPO4 are an acid/base conjugate pair. They will make an excellent buffer. c) H2CO3 and NaHCO3 are also an acid/base conjugate pair and they will make an excellent buffer. The carbonic acid/bicarbonate buffer plays an important role in maintaining the pH of your blood at a constant value. 4) Solutions containing acid-base buffers are resistant to change in the pH of the solution when H3O+ or OH- is added or removed.

orders of magnitude in [H3O +]. Part 2. Calculate the pH change upon adding 10.0 mL 0.10 M NaOH to 90 mL buffer containing 1.0 M NH3 and 1.0 M NH4Cl. The key reaction with the buffer will be: NH4 + + OH-Æ H 2O + NH3 The strong base will react with the ammonium cation in the buffer and completely convert it to ammonia. The number of moles of ...

  Order, Reactions

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