Although the aciddissociation constant for phenol C 6 H 5 OH is listed in your book the dissociation constant for the phenolate ion C 6 H 5 O is not Explain why it is not necessary to list both ID: 1036067
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1. Tuesday, February 14thAlthough 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 10-10. 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. 6Given that Ka for acetic acid is 1.8 x 10-8 and the Ka for hypochlorous acid is 3.0 x 10-8Which 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.
3. pKa and pKbpKa = -log(Ka)pKb = -log(Kb)pKa + pKb = 14We will use these a lot more in chapter 16!
4. Is that salt acidic, basic, or neutral?Separate the salt into its anions and cationsTurn 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?CationAnionResultStrong baseStrong acidNeutralWeak baseStrong acidAcidicStrong baseWeak acidBasicWeak baseWeak acid??? (depends on relative strength)
5. Will each of the following salt solutions be acidic, basic or neutral?NaClNH4NO3NH4Br FeCl3 Na2CO3 KClO4 NaHC2O4
6. HomeworkFinish MasteringChem 15.7-15.8Ch 15 ReviewYour chapter 15 quiz is tomorrow!!