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Problem- The conjugate acid of ammonia is NH4+, a weak acid. If a 0.2 M NH4Cl solution has a pH of 5.0, what is the Ka of NH4+?
Hi, I'm trying to understand this problem: "The conjugate acid of ammonia is NH4+, a weak acid. If a 0.2 M NH4Cl solution has a pH of 5.0, what's the Ka of NH4+? " The NH4Cl is throwing me off, I don't know where it's coming from. I wrote the EQ equation as: NH4+ + H2O <-> NH3 + H3O+, so Ka = [NH3][H3O+]/[NH4+]... I used the given pH to get [H3O+]=1x10^-5 M, same as [NH3]

Please explicate as simply and as clearly as you can thank in advance for assistance.

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