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Chapter 16, Problem 16.166QP

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CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933

Solutions

Chapter
Section
FindFindarrow_forward

CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933

(a)

Interpretation Introduction

Interpretation:

The overall and net ionic equations for the reaction between iron(III) oxide, which represents the rust layer over iron, and HCl has to be written; the Brønsted acid and base has to identified

Concept Information:

A chemical substance that gives hydrogen ions when dissolved in water is called as acid. A chemical substance that gives hydroxide ions in solution is called as base.

Bronsted's definitions of acid and base:

 Bronsted's definition is based on the  chemical reaction that occur when both acids and bases are added with each other. In Bronsted's theory acid donates proton , while base accepts proton from acid.

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid. Ammonia accepts a proton, and hence it is a Bronsted base.

pH definition:

The concentration of hydrogen ion is measured using pH scale.  The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H3O+]

To Give: The overall and net ionic equations for the reaction between iron(III) oxide, which represents the rust layer over iron, and HCl ; the Brønsted acid and base in the reaction

(b)

Interpretation Introduction

Interpretation:

Hydrochloric acid reacts with calcium carbonate in two stages. Equations for these two stages and for the overall reaction has to be written

Concept Information:

A chemical substance that gives hydrogen ions when dissolved in water is called as acid. A chemical substance that gives hydroxide ions in solution is called as base.

Bronsted's definitions of acid and base:

 Bronsted's definition is based on the  chemical reaction that occur when both acids and bases are added with each other. In Bronsted's theory acid donates proton , while base accepts proton from acid.

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid. Ammonia accepts a proton, and hence it is a Bronsted base.

pH definition:

The concentration of hydrogen ion is measured using pH scale.  The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H3O+]

To Write: Equations for these two stages and for the overall reaction

(c)

Interpretation Introduction

Interpretation:

Hydrochloric acid is used to recover oil from the ground. If the density of the acid    solution is 1.073 g/mL , the pH of the acid solution has to be calculated

Concept Information:

A chemical substance that gives hydrogen ions when dissolved in water is called as acid. A chemical substance that gives hydroxide ions in solution is called as base.

Bronsted's definitions of acid and base:

 Bronsted's definition is based on the  chemical reaction that occur when both acids and bases are added with each other. In Bronsted's theory acid donates proton , while base accepts proton from acid.

Example: Consider the following reaction.

HCl+NH3NH4++Cl-

Hydrogen chloride donates a proton, and hence it is a Bronsted acid. Ammonia accepts a proton, and hence it is a Bronsted base.

pH definition:

The concentration of hydrogen ion is measured using pH scale.  The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H3O+]

To calculate: The pH of the given acid solution

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