Preparation of dithizone indicator solution

Learn the procedure for making a dithizone indicator solution.

The compound that changes color when exposed to acidic or basic solutions is called an indicator. Most of the time, color indicators are used to measure pH. To find the endpoint or equivalence point of the titration, they are added to the reaction mixture.

Dithizone (C13H12N4S) is a sulfur-containing organic compound chemically described as 1,5-diphenylthiocarbazone, which is used as a complexometry/metal indicator. It comes in the form of crystalline black powder which is soluble in ethanol but insoluble in water.

It is a good ligand and can form complexes with several toxic metals, including lead, thallium, and mercury. Additionally, it acts as a chelating agent for toxic metals including lead and mercury.

How to prepare dithizone indicator for titration:

• Accurately weigh 25 mg of dithizone and pour it into a 100 mL volumetric flask with 50 ml of ethanol.
• Once it is dissolved, dilute it to 100.00 mL with ethanol.
• The concentration of the prepared solution is about 01 g/L.

Dithizone has a pKa of 1:4.50;pK2:15 (25°C), When used as an indicator, it produces a pink color in a pH range of 4 to 5 when zinc ions are present, and a green color when these ions are absent.

References:

Wikipedia contributors. (2022, August 9). Dithizone. In Wikipedia, The Free Encyclopedia. Available Here:

Law.resource.org. 2022. [online] Available Here:

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Preparation of pyridylazo naphthol indicator solution

Learn the procedure for making pyridylazo naphthol indicator solution.

The compound that changes color when exposed to acidic or basic solutions is called an indicator. Most of the time, color indicators are used to measure pH. To find the endpoint or equivalence point of the titration, they are added to the reaction mixture.

Pyridylazonaphthol (C15H11N3O) is an orange-colored dye chemically described as 1-(2-Pyridylazo)-2-naphthol (PAN) which is used as an acid-base/complexometry/metal indicator. It comes in the form of orange powder which is soluble in ethanol but insoluble in water.

When copper ions are present in an acidic solution, it produces a yellow color. However, when these ions are absent, the solution becomes red. It is a useful indicator in complexometric titrations because it may form chelates with metal ions.

How to prepare pyridylazo naphthol indicator for titration:

• Accurately weigh 100 mg of pyridylazo naphthol and pour it into a 100 mL volumetric flask with 50 ml of methyl alcohol.
• Once it is dissolved, dilute it to 100.00 mL with methyl alcohol.
• The concentration of the prepared solution is about 01 g/L.

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Preparation of sodium alizarin sulfonate indicator solution

Learn the procedure for making sodium alizarin sulfonate indicator solution.

The compound that changes color when exposed to acidic or basic solutions is called an indicator. Most of the time, color indicators are used to measure pH. To find the endpoint or equivalence point of the titration, they are added to the reaction mixture.

Sodium alizarin sulfonate is a chemical compound, chemically described as sodium 1,2-dihydroxy-9, 10 anthraquinone-3-sulphonate, used as a metal indicator. It comes in the form of yellow-orange powder which is soluble in water and ethanol.

At a pH of about 4.0, it produces a bluish-red lake with thorium and aluminum ions, However, the solution turns yellow when these ions are absent.

How to prepare sodium alizarin sulfonate indicator for titration:

• Accurately weigh 100 mg of sodium alizarin sulfonate and pour it into a 100 ml volumetric flask with 50 ml of distilled water.
• Once it is dissolved, dilute it to 100.00 mL with distilled water.
• The concentration of the prepared solution is about 01 g/L.

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Preparation of alkali blue 6B indicator solution

Learn the procedure for making an alkali blue 6B indicator solution.

The compound that changes color when exposed to acidic or basic solutions is called an indicator. Most of the time, color indicators are used to measure pH. They are added to the reaction mixture to find the endpoint or equivalence point of the titration.

Alkali blue 6B (C37H29N3O3S) is a chemical compound, chemically described as sodium para-rosaline mono sulphonate.

Alkali blue 6B has been used as a pH indicator for the non-aqueous titration method, which changes color from blue to greenish-red and its pH range is 9.4 (Blue) to pH 14.0 (Red). Alkali Blue 6B is a solid that is a dark blue powder. It is soluble in ethanol, but not in water.

How to prepare dichlorofluorescein indicator for titration:

• Accurately weigh 2 g of Alkali blue 6B and pour it into a 100 ml volumetric flask with 50 ml of rectified spirit.
• Once it is dissolved, dilute it to 100.00 mL with rectified spirit.
• The concentration of the prepared solution is about 20.0g/L.

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Preparation of α-Naphtholbenzein indicator solution

Learn the procedure for making 1-Naphtholbenzein indicator solution.

The compound that changes color when exposed to acidic or basic solutions is called an indicator. Most of the time, color indicators are used to measure pH. They are added to the reaction mixture to find the endpoint or equivalence point of the titration.

α-Naphtholphthalein (C28H18O4) is a dye, chemically describes as 4, 4′-(α-Hydroxybenzylidene)di-1-naphthol, p-naphtholbenzein

α-Naphtholbenzein has been used as a pH indicator during the acid-base titration method which changes color from colorless/reddish to greenish blue at pH 7.3–8.7. It changes from green (basic) to orange (neutral) to yellow (acidic) when used as an indicator for non-aqueous titrations.

Naphtholbenzein is a solid that is colorless to slightly reddish or blue-green. It dissolves in ethanol, acetic acid, and acetone, but not in water.

How to prepare dichlorofluorescein indicator for titration?

• Accurately weigh 0.2 g of 1-Naphtholbenzene and pour it into a 100 ml volumetric flask with 50 ml of acetic acid.
• Once it is dissolved, dilute it to 100.00 mL with acetic acid.
• The concentration of the prepared solution is about 2.0 g/L.

References:

1. Wikipedia contributors. (2022, April 3). Naphtholphthalein. In Wikipedia, The Free Encyclopedia. Available Here:
2. Law.resource.org. 2022. [online] Available Here:

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Preparation of dichlorofluorescein indicator solution

Learn the procedure for making dichlorofluorescein indicator solution.

The compound that changes color when exposed to acidic or basic solutions is called an indicator. Color indicators are commonly used to measure pH and are added to the reaction mixture to identify the titration endpoint or equivalence point.

Dichlorofluorescein (C20H10Cl2O5) is an organic dye of the fluorescein family, which is chemically described as 2′, 7′-Dichloro-3, 6-fluorandiol.

In Fajan’s method, it is used as an indicator for argentometric titration and as adsoprtion indicator. The color of the titration reaction changes from colorless to pale pink on reaching the equivalence point.

Dichlorofluorescein usually comes in the form of crystalline powder, in the color of orange to red-brown powder, which is soluble in ethanol and methanol but insoluble in water.

How to prepare dichlorofluorescein indicator for titration:

• Weigh 0.1 gm of dichlorofluorescein accurately and pour it into a 100.00 ml volumetric flask containing 50.00 ml of rectified spirit.
• Once it is dissolved, dilute it to 100.00 ml with rectified spirit.
• The concentration of the prepared solution is about 1.0 g/L.

References:

1. Wikipedia contributors. (2022, June 30). Dichlorofluorescein. In Wikipedia, The Free Encyclopedia. Available Here:
2. Law.resource.org. 2022. [online] Available Here:

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Preparation of phenosafranine indicator solution

Learn the procedure for making phenosafranine indicator solution.

The compound that changes color when exposed to acidic or basic solutions is called an indicator. Color indicators are commonly used to measure pH and are added to the reaction mixture to identify the titration endpoint/equivalence point.

Phenosafranine (C18H15ClN4) is a compound or dye, chemically described as 3,7-Diamino-5-phenylphenazinium chloride.

Phenosafranine is a phenylphenazinium bacterial stain for microscopy that is used as an indicator in adsorption and redox titration.

It turns the precipitate red when used in the titration of chloride or bromide with silver nitrate in an acid solution. Once the precipitate is complete, the color of the precipitate changes to blue color.

Phenosafranine usually comes in the form of powder, crystals, or flakes, and its appearance of dark green powder which is soluble in water.

How to prepare phenosafranine indicator for titration:

• Weigh accurately 0.25 gm of phenosafranine and pour it into a 100.00 ml volumetric flask containing 50.00 ml of distilled water and mix it.
• Once it is dissolved, dilute it to 100.00 ml with distilled water.
• The concentration of the prepared solution is about 2.5 g/L.

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Why KCl is used for the calibration of conductivity meter

Potassium chloride, often known as KCl, is the most commonly used solution for calibrating conductivity meters due to its high stability and solubility.

If you want reliable and repeatable results from the conductivity meter, calibration using pre-prepared standard solutions is essential. The most common calibration solution is potassium chloride (KCl). Calibration of a conductivity meter is an important maintenance task. Regular calibration produces consistent and reliable readings.

Electrical conductivity (EC) is the measure of the ion concentration present in the sample. The ability of a substance to transmit electric current in a certain area is known as conductivity. Siemens (S) is the unit of measurement for electrical conductivity, and scientific instruments commonly show measured units as MilliSiemens per centimeter mS/cm or MicroSiemens per cm μS/cm.

Because of its solubility and stability, KCl is the solution most often used in the process of calibrating the conductivity meter. Conductivity standard solutions are made up of a KCl: Water ratio. The mixing ratio is determined by the desired ion concentration level of the standard solution.

Molarity/Concentration of KCl	Standard conductivity
0.001 M	147 µS/cm ±10% at 25°C
0.01 M	1.413 mS/cm ±10% at 25°C
0.1 M	12.88 mS/cm ±10% at 25°C

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