1. It is found that 16.34 mL of a solution containing Ni* is required to titrate a sample of pure KCNweighing 0.5024 g. The reaction is Ni* + 4 CN" → Ni(CN),“ . Calculate the molarity of the nickelsolution.From the following data calculate the normalities of the acid and base solutions:weight of pure Na2CO3 = 0.2448 g; volume of acid = 43.65 mL ; volume of base used in backtitration =%3D0.84 mL ; 1.000 mL of base = 0.982 mL of acid.Reaction: CO, + 2H* → H2CO3

1.) To calculate the molarity of nickel solution , we would use stoichiometry relation. Note :…

. It is found that 16.34 mL of a solution containing Ni+ is required to titrate a sample of pure KCN weighing 0.5024 g. The reaction is Ni* + 4 CN" → Ni(CN)4" . Calculate the molarity of the nickel solution.

. It is found that 16.34 mL of a solution containing Ni+ is required to titrate a sample of pure KCN weighing 0.5024 g. The reaction is Ni* + 4 CN" → Ni(CN)4" . Calculate the molarity of the nickel solution.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section12.3: Determining Equilibrium Constants

Problem 12.3PSP

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

1. It is found that 16.34 mL of a solution containing Ni* is required to titrate a sample of pure KCN
weighing 0.5024 g. The reaction is Ni* + 4 CN" → Ni(CN),“ . Calculate the molarity of the nickel
solution.
From the following data calculate the normalities of the acid and base solutions:
weight of pure Na2CO3 = 0.2448 g; volume of acid = 43.65 mL ; volume of base used in back
titration =
%3D
0.84 mL ; 1.000 mL of base = 0.982 mL of acid.
Reaction: CO, + 2H* → H2CO3

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