EBK FOUNDATIONS OF COLLEGE CHEMISTRY
EBK FOUNDATIONS OF COLLEGE CHEMISTRY
15th Edition
ISBN: 9781118930144
Author: Willard
Publisher: JOHN WILEY+SONS INC.
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Chapter 13, Problem 24PE
Interpretation Introduction

Interpretation:

Empirical formula of hydrated nickel chloride has to be determined.

Concept Introduction:

The steps required for calculation of empirical formula is as follows:

1 Convert the data provided of each element in grams if not given in grams. If data is provided in percentage than total mass of compound is taken as 100 g.

2 Mass of each element is changed into moles by division of given mass of each element with its atomic mass respectively.

3 The value of mole of each element is divided by the smallest mole value and round off the resultant value to positive integer.

4 If resultant value is in fraction then multiply with smallest number to make it integer.

5 The final value of mole is used as a subscript for empirical formula.

Expert Solution & Answer
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Explanation of Solution

The hydrated nickel chloride contain 24.69 %  Ni, 29.83 % Cl and 45.48 % H2O. Therefore the empirical formula is calculated as follows:

Step 1: The percentage "%" is replaced by "g". Thus, 100 g hydrated iron chloride contain 24.69 g  Ni, 29.83 g Cl and 45.48 g H2O.

Step 2: The expression to calculate moles of elements is as follows:

   Moles=given massatomic mass

The formula to calculate moles of Ni is as follows:

   Moles(Ni)=mass of Nimolar mass of Ni        (1)

Substitute 24.69 g for mass of Ni and 58.69 g/mol for molar mass of Ni in equation (1).

   Moles(Ni)=24.69 g58.69 g/mol= 0.42 mol

The formula to calculate moles of Cl is as follows:

   Moles(Cl)=mass of Clmolar mass of Cl        (2)

Substitute 29.83 g for mass of Cl and 35.5 g/mol for molar mass of Cl in equation (2).

   Moles(Cl)=29.83 g35.5 g/mol=0.84 mol

The formula to calculate moles of H2O is as follows:

   Moles(H2O)=mass of H2Omolar mass of H2O        (3)

Substitute 45.48 g for mass of H2O and 18.02 g/mol for molar mass of H2O in equation (3).

   Moles(H2O)=45.48 g18.02 g/mol=2.52 mol

Step 3: The positive integer for Ni is calculated as follows:

  Subscript for Ni=moles of Ni smallest mole value         (4)

Substitute 0.42 mol for moles of Ni and 0.42 mol for smallest mole value in equation (4).

  Subscript for Ni=0.42 mol 0.42 mol1.0 

The positive integer for Cl is calculated as follows:

  Subscript for Cl=moles of Cl smallest mole value         (5)

Substitute 0.84 mol for moles of Cl and 0.42 mol for smallest mole value in equation (5).

  Subscript for Cl=0.84 mol 0.42 mol2.0 

The positive integer for H2O is calculated as follows:

  Subscript for H2O=moles of H2smallest mole value         (6)

Substitute 2.52 mol for moles of H2O and 0.42 mol for smallest mole value in equation (6).

  Subscript for H2O=2.52 mol 0.42 mol6.0 

Therefore, the empirical formula for hydrated iron chloride is NiCl26H2O.

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Chapter 13 Solutions

EBK FOUNDATIONS OF COLLEGE CHEMISTRY

Ch. 13 - Prob. 1RQCh. 13 - Prob. 2RQCh. 13 - Prob. 3RQCh. 13 - Prob. 4RQCh. 13 - Prob. 5RQCh. 13 - Prob. 6RQCh. 13 - Prob. 7RQCh. 13 - Prob. 8RQCh. 13 - Prob. 9RQCh. 13 - Prob. 10RQCh. 13 - Prob. 11RQCh. 13 - Prob. 12RQCh. 13 - Prob. 13RQCh. 13 - Prob. 14RQCh. 13 - Prob. 15RQCh. 13 - Prob. 16RQCh. 13 - Prob. 17RQCh. 13 - Prob. 19RQCh. 13 - Prob. 20RQCh. 13 - Prob. 21RQCh. 13 - Prob. 22RQCh. 13 - Prob. 23RQCh. 13 - Prob. 24RQCh. 13 - Prob. 25RQCh. 13 - Prob. 26RQCh. 13 - Prob. 27RQCh. 13 - Prob. 28RQCh. 13 - Prob. 29RQCh. 13 - Prob. 30RQCh. 13 - Prob. 31RQCh. 13 - Prob. 32RQCh. 13 - Prob. 33RQCh. 13 - Prob. 34RQCh. 13 - Prob. 35RQCh. 13 - Prob. 36RQCh. 13 - Prob. 37RQCh. 13 - Prob. 38RQCh. 13 - Prob. 39RQCh. 13 - Prob. 40RQCh. 13 - Prob. 41RQCh. 13 - Prob. 42RQCh. 13 - Prob. 43RQCh. 13 - Prob. 1PECh. 13 - Prob. 2PECh. 13 - Prob. 3PECh. 13 - Prob. 4PECh. 13 - Prob. 5PECh. 13 - Prob. 6PECh. 13 - Prob. 7PECh. 13 - Prob. 8PECh. 13 - Prob. 9PECh. 13 - Prob. 10PECh. 13 - Prob. 11PECh. 13 - Prob. 12PECh. 13 - Prob. 13PECh. 13 - Prob. 14PECh. 13 - Prob. 15PECh. 13 - Prob. 16PECh. 13 - Prob. 17PECh. 13 - Prob. 18PECh. 13 - Prob. 19PECh. 13 - Prob. 20PECh. 13 - Prob. 21PECh. 13 - Prob. 22PECh. 13 - Prob. 23PECh. 13 - Prob. 24PECh. 13 - Prob. 25PECh. 13 - Prob. 26PECh. 13 - Prob. 27PECh. 13 - Prob. 28PECh. 13 - Prob. 29PECh. 13 - Prob. 30PECh. 13 - Prob. 31PECh. 13 - Prob. 32PECh. 13 - Prob. 33AECh. 13 - Prob. 34AECh. 13 - Prob. 35AECh. 13 - Prob. 36AECh. 13 - Prob. 38AECh. 13 - Prob. 39AECh. 13 - Prob. 40AECh. 13 - Prob. 41AECh. 13 - Prob. 42AECh. 13 - Prob. 43AECh. 13 - Prob. 44AECh. 13 - Prob. 45AECh. 13 - Prob. 46AECh. 13 - Prob. 47AECh. 13 - Prob. 48AECh. 13 - Prob. 49AECh. 13 - Prob. 50AECh. 13 - Prob. 51AECh. 13 - Prob. 52AECh. 13 - Prob. 53AECh. 13 - Prob. 54AECh. 13 - Prob. 55AECh. 13 - Prob. 56AECh. 13 - Prob. 57AECh. 13 - Prob. 58AECh. 13 - Prob. 59AECh. 13 - Prob. 60AECh. 13 - Prob. 61AECh. 13 - Prob. 62AECh. 13 - Prob. 63AECh. 13 - Prob. 64AECh. 13 - Prob. 65AECh. 13 - Prob. 66AECh. 13 - Prob. 67AECh. 13 - Prob. 69CECh. 13 - Prob. 70CECh. 13 - Prob. 71CECh. 13 - Prob. 72CE
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Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY