1 indicators the indicator is usually a weaker chelate forming ligand. the indicator has a color...

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Indicators

The indicator is usually a weaker chelate forming ligand. The indicator has a color

when free in solution and has a clearly different color in the chelate. The following

equilibrium describes the function of an indicator (H3In) in a Mg2+ reaction with

EDTA:

MgIn- (Color 1) + Y4- MgY2- + In3- (Color 2)

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Problems Associated with Complexometric Indicators

There could be some complications which may render some complexometric titrations useless or have great uncertainties. Some of these problems are discussed

below:

1. Slow reaction rates

In some EDTA titrations, the reaction is not fast enough to allow acceptable and successful determination of a metal

ion. An example is the titration of Cr3+ where direct titration is not possible. The best way to overcome this

problem is to perform a back titration. However, we are faced with the problem of finding a suitable indicator that

is weaker than the chelate but is not extremely weak to be displaced at the first drop of the titrant.

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2. Lack of a suitable indicator

This is the most sever problem in EDTA titrations and one should be critical about

this issue and pay attention to the best method which may be used to overcome

this problem. First let us take a note of the fact that Mg2+-EDTA titration has excellent indicators that show very good change in

color at the end point. Look at the following situations:

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a. A little of a known standard Mg2+ is added to the metal ion of interest. Now the indicator will form a clear cut color with magnesium ions. Titration of the metal ion follows and after it is over, added EDTA will react with Mg-In chelate to release the free indicator, thus changing color. This procedure requires performing the same titration on a blank containing the same amount of Mg2+.

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b. A blank experiment will not be necessary if we add a little of Mg-EDTA complex to the metal ion of interest. The metal ion will replace the Mg2+ in the Mg-EDTA complex thus releasing Mg2+ which immediately forms a good color with the indicator in solution. No need to do any corrections since the amount of EDTA in the added complex is exactly equal to the Mg2+ in the complex.

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c. If it is not easy to get a Mg-EDTA complex, just add a little Mg2+ to the EDTA titrant. Standardize the EDTA and start titration. At the very first point of EDTA added, some Mg2+ is released forming a chelate with the indicator and thus giving a clear color.

It is wise to consult the literature for suitable indicators of a specific titration. There are a lot of data and information on titrations of all metals you may think of. Therefore, use this wealth of information to conduct successful EDTA titrations.

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Example

Find the concentrations of all species in solution at equilibrium resulting from mixing 50 mL of 0.200 M Ca2+

with 50 mL of 0.100 M EDTA adjusted to pH 10. 4 at pH

10 is 0.35. kf = 5.0x1010

Solution

Ca2+ + Y4- CaY2-

mmol Ca2+ added = 0.200 x 50 = 10.0

mmol EDTA added = 0.100 x 50 = 5.00

mmol Ca2+ excess = 10.0 – 5.00 = 5.00

[Ca2+]excess = 5.00/100 = 0.050 M

mmol CaY2- formed = 5.00

[CaY2-] = 5.00/100 = 0.050

CaY2- Ca2+ + Y4-

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CT = [H4Y] + [H3Y-] + [H2Y

2-] + [HY3-] + [Y4-]

Kf = [CaY2-]/[Ca2+]4CT

[Ca2+] = CT

Using the same type of calculation we are used to perform, one can write the following:

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Kf = [CaY2-]/[Ca2+][Y4-]

5.0x1010 = (0.05 – x)/((0.050 + x)*4 x)

assume that 0.05>>x

x = 5.6x10-11

Relative error will be very small value

The assumption is valid

[Ca2+] = 0.050 + x = 0.050 M

[CaY2-] = 0.050 – x = 0.050 M

[Y4-] = 0.35 * 5.6x10-11 = 1.9x10-11 M

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Example

Calculate the pCa of a solution at pH 10 after addition of 100 mL of 0.10 M Ca2+ to 100 mL of 0.10 M EDTA. 4 at pH 10 is 0.35. kf = 5.0x1010

Solution

Ca2+ + Y4- = CaY2-

mmol Ca2+ = 0.10 x 100 = 10

mmol EDTA = 0.10 x 100 = 10

mmol CaY2- = 10

[CaY2-] = 10/200 = 0.05 M

Therefore, Ca2+ will be produced from partial dissociation of the complex

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CaY2- Ca2+ + Y4-

CT = [H4Y] + [H3Y-] + [H2Y

2-] + [HY3-] + [Y4-]

Kf = [CaY2-]/[Ca2+]4CT

[Ca2+] = CT

5.0x1010 = 0.05/([Ca2+]2 x 0.35)

[Ca2+] = 1.7x10-6 M

pCa = 5.77

Using the same type of calculation we are used to perform, one can write the following:

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Kf = [CaY2-]/[Ca2+][Y4-]

5.0x1010 = (0.05 – x)/(x*4 x)

assume that 0.05>>x

x = 1.7x10-6

Relative error = (1.7x10-6/0.05) x 100 = 3.4x10-3%

[Ca2+] = 1.7x10-6 M

pCa = 5.77

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Example

Calculate the titer of a 0.100 M EDTA solution in terms of mg CaCO3 (FW = 100.0) per mL EDTA

Solution

The EDTA concentration is 0.100 mmol/mL, therefore, the point here is to calculate the mg CaCO3 reacting

with 0.100 mmol EDTA. We know that EDTA reacts with metal ions in a 1:1 ratio. Therefore 0.100 mmol

EDTA will react with 0.100 mmol CaCO3.

Mg CaCO3 = 0.100 mmol x 100.0 mg/mmol = 10.0

Therefore, the titer og EDTA in terms of CaCO3 is

10.0 mg CaCO3/mL EDTA

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Example

An EDTA solution is standardized against high purity CaCO3 by dissolving 0.3982 g of CaCO3 in HCL

and adjusting the pH to 10. The solution is then titrated with EDTA requiring 38.26 mL. Find the

molarity of EDTA.

Solution

EDTA reacts with metal ions in a 1:1 ratio. Therefore,

mmol CaCO3 = mmol EDTA

mg/FW = Molarity x VmL

398.2/100.0 = M x 38.26

MEDTA = 0.1041

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Example

Find the concentration of Ca2+ in a 20 mL of 0.20 M solution at pH 10 after addition of 100 mL of 0.10 M

EDTA. 4 at pH 10 is 0.35. kf = 5x1010

Solution

Initial mmol Ca2+ = 0.20 x 20 = 4.0

mmol EDTA added = 0.10 x 100 = 10

mmol EDTA excess = 10 – 4.0 = 6.0

CT = 6.0/120 = 0.050 M

mmol CaY2- = 4.0

[CaY2-] = 4.0/120 = 0.033 M

Ca2+ + Y4- CaY2- kf = 5.0x1010

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Kf = [CaY2-]/[Ca2+][Y4-]

5x1010 = (0.033 – x)/(x*4(0.050 + x) )

assume that 0.033>>x

x = 3.9x10-11

The assumption is valid by inspection of the values and no need to calculate the relative error. [Ca2+] = 3.9x10-11 M

pCa = 10.41

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Example

Find pCa in a 100 mL solution of 0.10 M Ca2+ at pH 10 after addition of 0, 25, 50, 100, 150, and 200 mL of

0.10 M EDTA. 4 at pH 10 is 0.35. kf = 5x1010

Solution

Again, we should remember that EDTA reactions with metal ions are 1:1 reactions. Therefore, we have:

Ca2+ + Y4- CaY2- kf = 5.0x1010

1. After addition of 0 mL EDTA

[Ca2+] = 0.10

pCa = 1.00

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Initial mmol Ca2+ = 0.10 x 100 = 10


mmol Ca2+ left = 10 – 2.5 = 7.5

[Ca2+]left = 7.5/125 = 0.06 M

In fact, this calcium concentration is the major source of calcium in solution since the amount of calcium

coming from dissociation of the chelate is very small. However, let us calculate the amount of

calcium released from the chelate:

mmol CaY2- formed = 2.5

[CaY2-] = 2.5/125 = 0.02 M

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Kf = [CaY2-]/[Ca2+][Y4-]

5x1010 = (0.02 – x)/((0.06 + x)*4 x)

assume that 0.02>>x

x = 1.9x10-11

The assumption is valid even without verification.

[Ca2+] = 0.06 + 1.9x10-11 = 0.06 M

pCa = 1.22

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mmol Ca2+ left = 10 – 5.0 = 5.0

[Ca2+]left = 5.0/150 = 0.033 M

We will see by similar calculation as in step above that the amount of Ca2+ coming from dissociation of the chelate is exceedingly small as compared to amount left. However, for the sake of practice

let us perform the calculation:

Mmol CaY2- formed = 5.0

[CaY2-] = 5.0/150 = 0.033 M

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Kf = [CaY2-]/[Ca2+][Y4-]

5x1010 = (0.033 – x)/((0.033 + x)*4 x)


x = 5.7x10-11

The assumption is valid even without verification.

[Ca2+] = 0.033+ 5.7x10-11 = 0.033 M

pCa = 1.48

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mmol Ca2+ left = 10 – 10 = ??

This is the equivalence point. The only source for Ca2+ is the dissociation of the Chelate

mmol CaY2- formed = 10

[CaY2-] = 10/200 = 0.05 M

Ca2+ + Y4- CaY2- kf = 5.0x1010

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Kf = [CaY2-]/[Ca2+][Y4-]

5x105 = (0.05 – x)/(x*4 x)

assume that 0.05>>x, x = 1.7x10-6

Relative error = (1.7x10-6/0.05) x 100 = 3.4x10-3%

[Ca2+] = 1.7x10-6 M, pCa = 5.77



mmol EDTA excess = 15 – 10 = 5.0

CT = 5.0/250 = 0.02 M

Mmol CaY2- = 10

[CaY2-] = 10/250 = 0.04 M

Ca2+ + Y4- CaY2- kf = 5.0x1010

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Kf = [CaY2-]/[Ca2+][Y4-]

5x1010 = (0.04 – x)/(x*4(0.02 + x) )

assume that 0.02>>x

x = 1.1x10-10

The assumption is valid

[Ca2+] = 1.1x10-10 M

pCa = 9.95

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mmol EDTA excess = 20 – 10 = 10

CT = 10/300 = 0.033 M

mmol CaY2- = 10

[CaY2-] = 10/300 = 0.033 M

Ca2+ + Y4- CaY2- kf = 5.0x1010

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Kf = [CaY2-]/[Ca2+][Y4-]

5x1010 = (0.033 – x)/(x*4(0.033 + x) )


x = 5.7x10-11

The assumption is undoubtedly valid

[Ca2+] = 5.7 x10-11 M

pCa = 10.24

1 indicators the indicator is usually a weaker chelate forming ligand. the indicator has a color...

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