We are being asked to calculate the Kb for a 0.100 M solution of ethylamine (C2H5NH2).
Sodium phenolate (C6H5ONa) is a sodium salt of phenol, therefore we know that it is a weak base.
Since we’re dealing with a weak base and Kb is an equilibrium expression, we will have to create an ICE chart to determine the equilibrium concentration of each species:
• C6H5O- → weak base → proton acceptor
• H2O → will act as the weak acid → proton donor
Equilibrium reaction: C6H5O-(aq) + H2O(l) ⇌ C6H5OH(aq) + OH-(aq)
(a) What is the pH of 0.100 M sodium phenolate, C6H5ONa, the sodium salt of phenol?
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Our tutors have indicated that to solve this problem you will need to apply the Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems.
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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.