Identify the Bronsted-Lowry acid, base, conjugate acid andconjugate base in the following reaction. HCl + NH3 NH4

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Identify the Bronsted-Lowry acid, base, conjugate acid andconjugate base in the following reaction.

HCl + NH3 <----> NH4 + Cl

b. If HCl is a strong acid how strong/weak is the conjugatebase?

c. Which side of the equation will preominate, the products orthe reactants at equilibrium given your answer to b?

d. If the Kb for NH3 is 1.80x10^-5 what is the Ka forNH4, the conjugat acid of NH3?

e. If ammonium chloride is added to ammonia in water whichdirection will the equilibrium move to( reactants or products)?

f. Is the ammonium chloride product in water solution acidic orbasic? Explain why.

Related Book For answer-question

Cambridge International AS And A Level Chemistry Coursebook

ISBN: 9781316637739

2nd Edition

Authors: Lawrie Ryan, Roger Norris

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Posted Date: Nov 30, 2022 04:20 PM

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Identify the Bronsted-Lowry acid, base, conjugate acid andconjugate base in the following reaction. HCl + NH3 NH4

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Answer BronsteLowry acid is HCl and base is NH3 conjugate acid base pair... View the full answer

Cambridge International AS And A Level Chemistry Coursebook

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