Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH.
(a) nitric acid (HNO3)
pH =
(b) acetic acid (HC2H3O2),
Ka = 1.8e-05
pH =
(c) benzoic acid (HC7H5O2),
Ka = 6.3e-05
pH =
1)
Concentration of HNO3 = 0.047M
concentration of NaOH = 0.055M
HNO3 and NaOH are strong acids and strong bases
Hence, PH=7
2)
Concentration of acetic acid= ( HC2H3O2) = 0.047M
Concentration of NaOH = 0.055M
Ka = 1.8 x10^-5
at equivalent point
HC2H3O2 ------------- H+ + C2H3O2-
at equivalent point
Concentration of C2H3O2- = [HC2H3O2][NaOH] / [HC2H2O2]+[NaOH]
[ C2H3O2- ] = 0.047 x 0.055 / 0.047+0.055 = 0.0253M
[ C2H3O2- ] = 0.0253M
C2H3O2- + H2O ------------------- HC2H3O2 + OH-
0.0253 0 0
-x +x +x
(0.0253-x) +x +x
Ka = 1.8 x10^-5
Ka xKb = Kw where Kw = ionic product of water = 1.0x10^-14
Kb = Kw / Ka = 1.0x10^-14 / 1.8x10^-5 = 5.55 x10^-10
Kb = 5.55 x10^-10
Kb = [ HC2H3O2] [ OH-] / [C2H3O2-]
5.55 x10^-2 = x*x /( 0.0253 -x )
for solving the equation
x= 3.75 x10^-6
[OH-] = 3.75x10^-6
-log[OH-] = -log( 3.75 x10^-6)
POH = 5.42
PH + POH = 14
PH = 14 - POH
PH = 14 - 5.42
PH = 8.58
c) Benzoic acid = ( HC7H5O2) = 6.3x10^-5
Concentration of acid = 0.047M
Concetration of base = 0.055
Ka = 6.3x10^-5
HC7H5O2 ------------------- H+ + C7H5O2-
at equivalent point
[ C7H5O2- ] = Mbase x Macid / Mbase + Macid
[ C7H5O2- ] = 0.047 x 0.055 / 0.047+0.055
[ C7H5O2- ] = 0.0253M
C7H5O2- + H2O ------------------------- HC7H5O2 + OH-
0.0253 0 0
-x +x +x
0.0253-x +x +x
Kb = Kw/ka = 1.0x10^-14 / 6.3x10^-5 = 1.59 x10^-10
Kb = 1.59 x10^-10
Kb = [ HC7H5O2] [ OH-]/[ C7H5O2- ]
1.59x10^-10 = x*x/(0.0253-x)
for solving the equation
x= 2.00 x10^-6
[OH-] = 2.00x10^-6
-log[OH-] = -log(2.00 x10^-6)
POH = 5.70
PH = 14 - 5.70
PH = 8.3
Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the...
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