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Tuesday, February 14th Although the acid-dissociation constant for phenol (C6H5OH) is listed in your book, the dissociation constant for the phenolate.

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Presentation on theme: "Tuesday, February 14th Although the acid-dissociation constant for phenol (C6H5OH) is listed in your book, the dissociation constant for the phenolate."— Presentation transcript:

1 Tuesday, February 14th Although the acid-dissociation constant for phenol (C6H5OH) is listed in your book, the dissociation constant for the phenolate ion (C6H5O-) is not. Explain why it is not necessary to list both. The Ka for phenol is 1.3 x Calculate the Kb for the phenolate ion. Is the phenolate ion a weaker or stronger base than ammonia? (Kb for ammonia = 1.8 x 10-8) Which is more likely to occur – the acid-dissociation of phenol or base- dissociation of phenolate? Explain.

2 Given that Ka for acetic acid is 1
Given that Ka for acetic acid is 1.8 x 10-8 and the Ka for hypochlorous acid is 3.0 x 10-8 Which is the stronger acid? Why? Which is the stronger base – the acetate ion or the hypochlorite ion? Why? Calculate the Kb values for the acetate ion and the hypochlorite ion. 6

3 pKa and pKb pKa = -log(Ka) pKb = -log(Kb) pKa + pKb = 14
We will use these a lot more in chapter 16!

4 Is that salt acidic, basic, or neutral?
Separate the salt into its anions and cations Turn the anion into an acid (add a hydrogen ion) Is it a strong acid or a weak acid? Turn the cation into a base (add hydroxide OR remove a hydrogen ion) Is it a strong base or weak base? Cation Anion Result Strong base Strong acid Neutral Weak base Acidic Weak acid Basic ??? (depends on relative strength)

5 Will each of the following salt solutions be acidic, basic or neutral?
NaCl NH4NO3 NH4Br  FeCl3  Na2CO3  KClO4  NaHC2O4

6 Homework Finish MasteringChem 15.7-15.8 Ch 15 Review
Your chapter 15 quiz is tomorrow!!

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