6G.5
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ayushibanerjee06
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6G.5
For the question: What is the concentration of hydronium ions in a solution that is 0.20 m NH2NH2(aq) and 0.30 m NaCl(aq), do we assume that [OH-] is 0.30 M and not [NH2NH3+]?
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Justin Vayakone 1C
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Re: 6G.5
NaCl doesn't affect the pH of the solution because the Na+ and Cl- ions don't react with anything. This means we completely ignore NaCl. We are given 0.20 M of NH2NH2, which is a weak base. Create an ICE table and look up the Kb for NH2NH2 in one of the tables in the textbook (6C.1 , 6C.2 and 6E.1). Then solve for x which equals [OH-]. Then use Kw value to convert [OH-] into [H3O+].
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