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1st year chemistry n0tes new
CHAPTER 8
CHEMICAL EQUILIBRIUM
What is weak electrolyte?
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A compound which is only partially ionized in aqueous solution
is called as weak electrolyte
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g CH3COOH(Acetic aci)
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The state of reversible reaction, in which forward and reverse
rates are equal
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What are reversible reaction?
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When an acid is dissolved in water it will form H3O+ ions and
an anion the anion of an acid is called conjugate base and H3O+ is
called conjugate acid e
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CH3OOH + H2O H3O+ + CH3COO–
Acid
Base
Conjugate acid
Conjugate base
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Buffers can resist the charge of its PH value therefore they are
required in chemical analysis, pharmaceuticals, electroplating,
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photography, beverage industry, microbiology molecular biology,
soil science and in quantitative analysis
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(i)
Pka or ka value of an acid
(ii)
Concentration of salt and acid taken for the buffer
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What is buffer capacity?
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Buffer capacity
is the ability of buffer to resist the change in its PH value
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How can we calculate the PH of buffer?
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10 How Kc can be applied to calculate direction of chemical
reaction?
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(ii)
If > Kc
Then the reaction will proceed in the backward direction until the
equilibrium is established
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The extent of reaction depends upon the magnitude of Kc
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Kc is very large:
When Kc is very large the reverse reaction will not occur to an
appreciable extent and the forward reaction is almost complete
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46 kJ/m
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By applying pressure, more product is obtained
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Continuous withdrawl of NH3 will also increase the yield
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Why?
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According to Le–chatlier’s principle, by increasing pressure the
reaction will move toward less number of moles
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These four parameters are related as
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16 Prove that Kw is ionic product of water and its value is 1 x 10–14
at 25o
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Water undergoes self ionization as
2H2O H3O+ + OH–
or H2O H+ + OH–
Kc [H2O] = [H+] [OH–]
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Its
value is 1 x 10–14
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17 How can you purify NaCl by common ion effect?
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These impurities can be removed by common Ion
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Then HCl gas is passed through it
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19 How can you co–relate Ka with Kc?
Ka is dissociation constant of an acid while Kc is the equilibrium
constant suppose an acid HA Ionize as
HA + H2O H3O+ + A–
Kc =
concentration of [H2O] almost remains constant so we can write
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20 How can you calculate % Ionization of an acid?
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% Ionization = x 100
initially available
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21 N2(g) + 3H2(g) 2NH3(g) H = -92
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It is represented
by Ksp
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