. A 100.0 mL solution containing HCl and HBr was titrated with 0.1235 M NaOH. The volume of the base required to neutralize the acid was 47.14 mL. Aqueous silver nitrate was then added to precipitate the Cl- and Br- ions as AgCl and AgBr. The mass of silver halides obtained was 0.9974 g. What are the molarities of HCl and HBr in the original solution?

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Sixta KovacekLv2

28 Sep 2019

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A 100.0 mL solution containing aqueous HCl andHBr was titratedwith 0.1215M NaOH. The volume of base required to neutralize theacid was 47.72mL . Aqueous AgNO3 was then added to precipitate theCl? and Br? ions as AgCl and AgBr. The mass of the silver halidesobtained was 0.9941g

1) What is the molarity of the HBr in the original solution?

2) What is the molarity of the HCl in the original solution?

It is desired to neutralize a solution X that contains a mixture of potassium chloride and hydrobromic acid. Titration of 13.6 mL X with 0.107 M silver nitrate required 56.6 mL of the latter. The resulting precipitate, containing a mixture of AgCl and AgBr, was dried and found to weigh 1.090 g. How much 0.131 M sodium hydroxide should be used to neutralize 13.6 mL solution X?

When sodium chloride, NaCl, is added to a solution of silver nitrate, AgNO₃, a white precipitate of silver chloride, AgCl, forms. If concentrated ammonia, NH₃, is added to this precipitate, a clear colorless solution forms containing diamminesilver(I) ions, [Ag(NH₃)₂]⁺. Potassium iodide, KBr, solution added to this colorless solution will cause pale yellow silver bromide, AgBr, to precipitate. List the species, Cl^-, NH₃, or Br^- in order of decreasing stability of the compounds or complexes that they can form with silver and explain your reasons.

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