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IntroductionIn this section Mohr method will be discussed in details
Mohr Method
An excellent method to determine the chloride ion titrimetrically is Mohr method.Mohr is very sensitive to pH; thus, this method should be occurred at neutral medium.Therefore, AgCl is formed first and after all
Clis consumed, the first drop of Ag+
in excess will react with the chromate indicator giving a reddish
precipitate(Ag2CrO4), however, this precipitate has a greater solubility than that of AgCl
Ag+ + Cl- -> AgCl(s) (Titration reaction) Ksp = 1.82 * 10-10
2Ag+ + CrO4
-2 -> Ag2CrO4
(End point reaction) Red -Brown Ksp=1.2 * 10-12
Titration added the equivalence point causes local excesses of Ag+
that result in flashes of red
color, but the correct end point is the first permanent darkening of the yellow chromate color.Ag+ + OH- -> AgOH(s) Ksp = 2.0 * 10-8
Moreover, in acidic solutions, the indicator if this experiment chromate will be converted to
dichromate.Since, in
alkaline solutions, silver will react with the hydroxide ions (OH-
) forming insoluble silver
hydroxide(AgOH).This method undergoes
direct titration; it utilizes chromate as an indicator.Chloride is titrated with a standard silver nitrate
solution; a soluble chromate salt is added as the indicator.The Mohr method
for chloride was published more than a hundred years ago and is still used.Some excess silver nitrate must be added to form
enough silver chromate to be seen over the heavy white precipitate and yellow chromate solution.Moreover, a
dilute chromate solution should be used due to the intense color of the indicator.
IntroductionIn this section Mohr method will be discussed in details
Mohr Method
An excellent method to determine the chloride ion titrimetrically is Mohr method. The Mohr method
for chloride was published more than a hundred years ago and is still used. This method undergoes
direct titration; it utilizes chromate as an indicator. Chloride is titrated with a standard silver nitrate
solution; a soluble chromate salt is added as the indicator. Therefore, AgCl is formed first and after all
Clis consumed, the first drop of Ag+
in excess will react with the chromate indicator giving a reddish
precipitate(Ag2CrO4), however, this precipitate has a greater solubility than that of AgCl
𝐴𝑔+ + 𝐶𝑙− → 𝐴𝑔𝐶𝑙(𝑠) (𝑇𝑖𝑡𝑟𝑎𝑡𝑖𝑜𝑛 𝑟𝑒𝑎𝑐𝑡𝑖𝑜𝑛) 𝐾𝑠𝑝 = 1.82 ∗ 10−10
2𝐴𝑔+ + 𝐶𝑟𝑂4
−2 → 𝐴𝑔2𝐶𝑟𝑂4
(𝐸𝑛𝑑 𝑝𝑜𝑖𝑛𝑡 𝑟𝑒𝑎𝑐𝑡𝑖𝑜𝑛) Red –Brown 𝐾𝑠𝑝=1.2 ∗ 10−12
Titration added the equivalence point causes local excesses of Ag+
that result in flashes of red
color, but the correct end point is the first permanent darkening of the yellow chromate color. The
end point is not sharp as might be desired. Some excess silver nitrate must be added to form
enough silver chromate to be seen over the heavy white precipitate and yellow chromate solution.
The concentration of chromate indicator is important. If too much chromate is added, the end
point appears before the equivalence point, if not enough, the end point comes late. Moreover, a
dilute chromate solution should be used due to the intense color of the indicator. This will require
additional amount of Ag+
for the Ag2CrO4 to form.
Mohr is very sensitive to pH; thus, this method should be occurred at neutral medium. Since, in
alkaline solutions, silver will react with the hydroxide ions (OH-
) forming insoluble silver
hydroxide(AgOH).
𝐴𝑔+ + 𝑂𝐻− → 𝐴𝑔𝑂𝐻(s) 𝐾𝑠𝑝 = 2.0 ∗ 10−8
Moreover, in acidic solutions, the indicator if this experiment chromate will be converted to
dichromate.
2𝐶𝑟𝑂4
2− + 2𝐻+ → 𝐶𝑟2𝑂7
2− +H2O
Therefore, the pH of solution should be kept at about 7.
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