   Chapter 4, Problem 127IL

Chapter
Section
Textbook Problem

Chromium(III) chloride forms many compounds with ammonia. To find the formula of one of these compounds, you titrate the NH3 in the compound with standardized acid.Cr(NH3)xCl3(aq) + x HCl(aq) → x NH4+(aq) + Cr3+(aq) + (x + 3) Cl−(aq)Assume that 24.26 mL of 1.500 M HCl is used to titrate 1.580 g of Cr(NH3)xCl3. What is the value of x?

Interpretation Introduction

Interpretation:

The value of x in the compound Cr(NH3)xCl3 involved in the given reaction has to be determined.

Concept introduction:

• For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.

Concentrationofsubstance=Amountof substancevolumeofthesubstance

Explanation

Balanced chemical equation for the given reaction is,

Cr(NH3)xCl3(aq)+xHCl(aq)xNH4+(aq)+Cr(aq)3++(x+3)Cl(aq)

Amount of HCl can be calculated from its volume and concentration as follows,

AmountofHCl =CHCl×VHCl =1.500molL×0.02426L =0.3639molHCl

Molar mass of Cr(NH3)xCl3 can be calculated as,

58.93+(14.01+1.008×3)x+35.45×3=17.034x+165.28

Cr(NH3)xCl3 And  HCl are in stoichiometric ratio

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