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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

A Boric acid and glycerin form a complex

B(OH)3(aq) + glycerin(aq) ⇄ B(OH)3 · glycerin(aq)

with an equilibrium constant of 0.90. If the concentration of boric acid is 0.10 M, how much glycerin should be added, per liter, so that 60.% of the boric acid is in the form of the complex?

Interpretation Introduction

Interpretation:

The amount of glycerine that has added so that 60% of boric acid will be in the form of complex in the reaction B(OH)3(aq)+glycerinB(OH)3.glycerin(aq) has to be calculated.

Concept Introduction:

Equilibrium constantKC for a general reaction is:

aA(g)+bB(g)cC(g)+dD(g)KC=[C]c×[D]d[A]a×[B]b

Equilibrium constant in terms of pressure[Kp]: Equilibrium constant can be expressed in terms of partial pressures in atmospheres.

aA(g)+bB(g)cC(g)+dD(g)KP=PCc×PDdPAa×PBb

Explanation

Given:

B(OH)3(aq)+glycerinB(OH)3.glycerin(aq)KC=0.90ConcentrationofB(OH)3=0.10M

Given that 60% of the given boric acid will be in the form of complex

60×0.1100=0.06M

At equilibrium [B(OH)3]=0.1-0.06=0.04M

B(OH)3(aq)+glycerinB(OH)3.glycerin(aq)Initial0.10Mx0Equilibrium0

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