Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN: 9781285869759
Author: Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher: Cengage Learning
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Chapter 8, Problem 8.113P
Interpretation Introduction

(a)

Interpretation:

The molarity of the hydrofluoric acid in the solution is to be calculated.

Concept Introduction:

The molarity of a solution is defined as number of moles of solute in 1L of solution. This is mathematically represented as follows:

M=nV(inl)

Here, n is number of moles and v is volume of solution.

The pressure, volume, moles and temperature of a gas are related to each other according to an equation,

PV=nRT

Here, p is pressure, v is volume, n is number of moles, r is gas constant and t is temperature of the gas.

Expert Solution
Check Mark

Answer to Problem 8.113P

Thus, the molarity of the HF solution is 0.02498 M.

Explanation of Solution

The pressure, volume, moles and temperature of a gas are related to each other according to an equation,

PV=nRT

Here,

P = Pressure of HF gas = 0.601 atm.

V = Volume of HF gas = 1.00 L.

n = Moles of HF gas = it is to be found.

R = Gas constant = 0.0821 L.atm/mol.K.

T = Temperature in K = 20.0 CO = 20.0 + 273 = 293.0 K.

Putting the given values in the ideal gas equation, we get.

PV=nRT(0.601atm)(1.00L)=n(0.0821L.atmmol.K)(293.0K)n=0.601×1.000.0821×293.0n=0.02498 mol

Thus, the number of moles of HF = 0.02498 mol.

Now, the molarity of this solution is to be calculated.

M=nV(inl)=0.02498mol1.00L=0.02498 M

Thus, the molarity of the HF solution is 0.02498 M.

Interpretation Introduction

(b)

Interpretation:

The acid ionization constant, Ka is to be calculated.

Concept Introduction:

Weak acids do not dissociate completely. Let HA be a weak acid. The dissociation of the weak acid can be represented by the chemical equation,

HA(aq)H+(aq)+A(aq)

The equation for acid dissociation constant can be written from this chemical equation.

Ka=[H+][A][HA].

Expert Solution
Check Mark

Answer to Problem 8.113P

The acid dissociation constant of hydrofluoric acid is Ka=0.01472.

Explanation of Solution

Hydrofluoric acid is a weak acid. Hence, it does not dissociate completely. The dissociation of the given weak acid can be represented by the chemical equation,

HF(aq)H+(aq)+F(aq)

The equation for acid dissociation constant can be written from this chemical equation.

Ka=[H+][F][HF]

The concentrations of each of the ions at equilibrium can be obtained from the ICE table, where ICE represents the Initial, Change and Equilibrium concentrations of the weak acid.

                                            HF(aq)H+(aq)+F(aq)                              [HF]                   [H+]                       [F]i                      0.02498                         0                            0 C                         X                              +X                          +X e                     0.02498X                     +X                           +X

The hydrogen ion concentration can be obtained from the given pH. The pH is defined as the negative logarithm of the hydrogen ion concentration.

pH=log[H+]

The pH of the weak acid solution at equilibrium is 1.88. Thus, we can calculate the concentration of the hydrogen ion.

pH=log[H+][H+]=101.88=0.01318molL1X=[H+]=0.01318molL1

We calculated the “x” which is the concentration of hydrogen ion. The concentration of the anion is also “x”. Thus,

X=[F]=0.01318molL1

Now, we need to calculate the concentration of [HF]

[HF]=0.02498X=0.024980.01318=0.0118M

Thus, the concentration of hydrofluoric acid is [HF] = 0.0118.

The concentrations of the anion, hydrogen ion and hydrofluoric acid are used in the equation used for acid dissociation constant.

Ka=[H+][F][HF]=[0.01318][0.01318]0.0118Ka=0.01472

Thus, the acid dissociation constant of hydrofluoric acid is Ka=0.01472.

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Chapter 8 Solutions

Introduction to General, Organic and Biochemistry

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