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11 Dec 2019

You could add HCl(aq) to the solution to precipitate out AgCl(s). What volume of a 0.200 M HCl(aq) solution is needed to precipitate the silver ions from 13.0 mL of a 0.180 M AgNO3 solution

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Jamar Ferry
Jamar FerryLv2
13 Dec 2019

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Related questions

(a) What volume of 0.115 M HClO4 solution is needed to neutralize 50.00 mL of 0.0875 M NaOH? (b) What volume of 0.128 M HCl is needed to neutralize 2.87 g of Mg(OH)2? (c) If 25.8 mL of an AgNO3 solution is needed to precipitate all the Cl- ions in a 785-mg sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution? (d) If 45.3 mL of a 0.108 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution?

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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?

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