Thank you very much Make sure you show all work and report all answers with the

Question

Thank you very much Make sure you show all work and report all answers with the proper number of significant figures Your unknown G is a mixture of NaCl and a neutral salt. Suppose you weigh a 0.2134 grams sample of Unknown G, dissolve it, and want to precipitate ALL of its Cl with 0.20 M AgNO3. 1) The Cl in Unknown G is precipitated with the solution of AgNO3. Write the net ionic equation for the reaction between the silver ion and the chloride ion. 2) To make sure ALL the Cl in your Unk G is precipitated, assume that your sample is 100%NaCl. Calculate the moles of Naci in this supposedly 100% NaCl sample (the molar mass for Naci is 58.54 g/mol.) 3) How many mole of Ag do you need to precipitate the Cl in your "100% NaCl sample?" (Note that the moles of Cl is equal to the mole of NaCl. 4) Calculate the volume (in mL) of 0.20 M AgNO3 that you need to precipitate the CI in your "100% NaCl sample.

Explanation / Answer

Given

Net ionic equation

Ag+ (aq) + Cl- (aq) -----> AgCl (s) Answer 1

Mass of NaCl = 0.2134 g

Molar mass of NaCl = 58.44 g/mol

No. of moles of NaCl = mass / molar mass = 0.2134 g / 58.44 g/mol = 0.003652 moles Answer 2

No. moles of Cl- = 0.003652 moles

No. of moles of Ag+ required to nuetralize this many mole so Cl-

No. of moles of Ag+ = 0.003652 moles Answer 3

given molarity = 0.2 M = 0.2 mol/L

Volume = No. of moles / molarity = 0.003652 moles / 0.2 mol/L = 0.01826 L = 18.26 ml Answer 4

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