Wednesday, December 29, 2021

Preparation and standardization of 0.02 M mercuric nitrate

Learn about the preparation and standardization of 0.02 M mercuric nitrate solution through a laboratory experiment or practical.

Aim:

To prepare and standardize 0.02 M mercuric nitrate solution using standard sodium chloride (volumetric solution).

Requirements:

Glasswares: Burette, burette stand, conical flask, volumetric pipette, beaker, volumetric flask, funnel, glass rod, and wash bottle, etc.
Chemicals: Mercuric nitrate (Hg(NO3)2), sodium chloride (NaCl), and nitric acid (HNO3), etc.

Preparation of 0.02 M mercuric nitrate solution:

Take properly weighed 06.80 gm of mercuric nitrate and add in 20 ml of 1M nitric acid, Once it has completely dissolved, make up the volume to 1000 ml with water.

Titration procedure:

  • All glassware should be cleaned and dried according to standard laboratory procedures.
  • Before filling the burette for the titration, rinse it with distilled water and then pre-rinse it with a portion of the titrant solution. Pre-rinsing is required to make sure that all solution in the burette is the desired solution, not a contaminated or diluted solution.
  • Take the unknown stock solution of titrant in a clean and dry beaker then fill the burette using the funnel.
  • Remove air bubbles from the burette and adjust the reading to zero.
  • Take 15.00 mg of sodium chloride and add 50 ml of water.
  • Titrate it with mercuric nitrate solution until the endpoint, which is to be determined potentiometrically.
  • Titration can be done with a platinum or mercury indicator electrode and a mercury-mercurous sulfate reference electrode
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.
  • Take their mean and calculate the molarity of the mercuric nitrate solution.
  • 1 ml of 0.02 M mercuric nitrate is equivalent to 0.002338 g of sodium chloride.

Observation table:

Sr. No.

Content in conical flask

 

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Result:

The strength of the prepared mercuric nitrate solution was found to be_____M.


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Preparation and standardization of 0.1 M lead nitrate

Learn about the preparation and standardization of 0.1 M lead nitrate solution through a laboratory experiment or practical.

Aim:

To prepare and standardize 0.1 M lead nitrate solution using standard 0.1M EDTA (volumetric solution).

Requirements:

Glasswares: Burette, burette stand, conical flask, volumetric pipette, beaker, volumetric flask, funnel, glass rod, and wash bottle, etc.

Chemicals: Lead nitrate (Pb(NO3)2) disodium edetate (EDTA), hexamine (C6H12N4), and Xylenol Orange mixture, etc.

Preparation of 0.1M lead nitrate solution:

Take properly weighed 33.12 gm of lead nitrate and add in 500 ml of distilled water, Once it has completely dissolved, make up the volume to 1000 ml with water.

Titration procedure:

  • All glassware should be cleaned and dried according to standard laboratory procedures.
  • Before filling the burette for the titration, rinse it with distilled water and then pre-rinse it with a portion of the titrant solution. Pre-rinsing is required to make sure that all solution in the burette is the desired solution, not a contaminated or diluted solution.
  • Take the unknown stock solution of titrant in a clean and dry beaker then fill the burette using the funnel.
  • Remove air bubbles from the burette and adjust the reading to zero.
  • Take 50.00 ml of a prepared solution of lead nitrate and pour it into a conical flask.
  • Then, as an indication, add 50 mg of xylenol orange mixture and enough hexamine to make a violet-pink color.
  • Titrate it with 0.1 M disodium edetate solution with constant stirring until the endpoint.
  • The actual endpoint is indicated by the appearance of a lemon yellow color.
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.
  • Take their mean and calculate the molarity of the lead nitrate solution.

Observation table:

Sr. No.

Content in conical flask

 

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Calculations:

1 ml of 0.1 M disodium edetate is equivalent to 0.03312 g of lead (II) nitrate.

M = Molarity of EDTA x reading of the burette / 33

Result:

The strength of the prepared lead nitrate solution was found to be_____M.


Frequently Asked Questions (FAQ):

What is the molecular mass of lead (II) nitrate?

Lead (II) nitrate is an inorganic compound with the chemical formula Pb(NO3)2 and its molecular weight is 331.2 g/mol.

Which primary standard is used in the standardization of 0.1 normal AgNO3?

Sodium chloride is used as the primary standard in the standardization of 0.1 normal AgNO3.
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Tuesday, December 28, 2021

Preparation and standardization of 0.05 M magnesium sulphate

  Learn about the preparation and standardization of 0.05 m magnesium sulphate solution through a laboratory experiment or practical.


Aim:

To prepare and standardize 0.05 m magnesium sulphate solution using standard 0.1M EDTA (volumetric solution).

Requirements:

Glasswares: Burette, burette stand, conical flask, volumetric pipette, beaker, volumetric flask, funnel, glass rod, and wash bottle, etc.

Chemicals: Magnesium sulfate (MgSO4), disodium edetate (EDTA), ammonia-ammonium chloride solution, and mordant back II, etc.

Preparation of 0.05 M magnesium sulphate solution:

Take properly weighed 12.50 gm of magnesium sulfate and add in 500 ml of distilled water, Once it has completely dissolved, make up the volume to 1000 ml with water.

Titration procedure:

  • All glassware should be cleaned and dried according to standard laboratory procedures.
  • Before filling the burette for the titration, rinse it with distilled water and then pre-rinse it with a portion of the titrant solution. Pre-rinsing is required to make sure that all solution in the burette is the desired solution, not a contaminated or diluted solution.
  • Take the unknown stock solution of titrant in a clean and dry beaker then fill the burette using the funnel.
  • Remove air bubbles from the burette and adjust the reading to zero.
  • Take 30.00 ml of a prepared 0.05 m magnesium sulphate solution and pour it into a conical flask.
  • Then add 20.00 ml of distilled water and 10.00 ml of ammonia-ammonium chloride solution and shake well.
  • Add 50 mg mordant back II as an indicator.
  • Titrate it with 0.1 M disodium edetate solution with constant stirring until the endpoint.
  • The actual endpoint is indicated by the appearance of a violet color to blue.
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.
  • Take their mean and calculate the molarity of the magnesium sulphate solution.

Observation table:

Sr. No.

Content in conical flask

 

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Calculations:

1 ml of 0.1 M EDTA is equivalent to 0.02465 g of magnesium sulphate.

M = Molarity of EDTA x reading of the burette / 25

Result:

The strength of the prepared magnesium sulphate solution was found to be_____M.


Frequently Asked Questions (FAQ):

What is the molecular mass of MgSO4?

Magnesium sulphate, often known as magnesium sulphate, is a salt with the formula MgSO4 with a molecular weight of 120.366 g/mol.

Which indicator is used in the assay of magnesium sulphate?

Titration with 0.1 M MgSO4 solution is performed in the presence of an eriochrome black T solution as an indicator.
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Preparation and standardization of 0.1 M zinc chloride

Learn about the preparation and standardization of 0.1 M zinc chloride solution through a laboratory experiment or practical.

Aim:

To prepare and standardize 0.1 M zinc chloride solution using standard 0.1M EDTA (Complexometric titration).

Requirements:

Glasswares: Burette, burette stand, conical flask, volumetric pipette, beaker, volumetric flask, funnel, glass rod, and wash bottle, etc.

Chemicals: Zinc chloride (ZnCl2), disodium edetate (C10H16N2O8), ammonium acetate (C2H7NO2), hydrochloric acid (HCl), hexamine (C6H12N4) and xylenol orange indicator, etc.

Preparation of 0.1M zinc chloride solution:

Take properly weighed 13.63 gm of zinc chloride and dissolve in a minimum volume of 2M HCl, add 500 ml of distilled water and allow cooling and dissolving. Once it has completely dissolved, make up the volume to 1000 ml with water.

Preparation of 2M HCl:

Take 07.30 gm of concentrated hydrochloric acid in 1000 ml of distilled water.

Titration procedure:

  • All glassware should be cleaned and dried according to standard laboratory procedures.
  • Before filling the burette for the titration, rinse it with distilled water and then pre-rinse it with a portion of the titrant solution. Pre-rinsing is required to make sure that all solution in the burette is the desired solution, not a contaminated or diluted solution.
  • Take the unknown stock solution of titrant in a clean and dry beaker then fill the burette using the funnel.
  • Remove air bubbles from the burette and adjust the reading to zero.
  • Take 25.00 ml of a prepared 0.1 M zinc chloride solution and pour it into a conical flask.
  • Add 04.00 gm of ammonium acetate.
  • Then add 25.00 ml of distilled water and 50.00 mg xylenol orange mixture and shake well.
  • Add a sufficient amount of hexamethylenetetramine until the solution becomes violet-pink.
  • Titrate it with previously standardized 0.1 M Disodium edetate solution with constant stirring until the endpoint.
  • A solution becomes yellow when it reaches the endpoint.
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.
  • Take their mean and calculate the molarity of the zinc chloride solution.

Observation table:


Sr. No.

Content in conical flask

 

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Calculations:

1 ml of 0.1 M EDTA is equivalent to 0.013630 g of zinc chloride.

M = Molarity of EDTA x reading of the burette / 25

Result:

The strength of the prepared zinc chloride solution was found to be_____M.


Frequently Asked Questions (FAQ):

How to prepare 0.05 m zinc chloride solution?

Take properly weighed 6.82 gm of zinc chloride and pour in a 1-liter volumetric flask, add a minimum volume of 2M HCl to dissolve, and make up the volume to 1000 ml with water.

What is the molecular mass of zinc chloride?

Zinc chloride is a chemical compound with the formula ZnCl2 and its molecular mass is 136.286 g/mol.
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Preparation and standardization of 0.1 M zinc sulphate

 Learn about the preparation and standardization of 0.1 M zinc sulphate solution through a laboratory experiment or practical.


Aim:

To prepare and standardize 0.1 M zinc sulphate solution using standard 0.1M EDTA (Complexometric titration).

Requirements:

Glasswares: Burette, burette stand, conical flask, volumetric pipette, beaker, volumetric flask, funnel, glass rod, and wash bottle, etc.

Chemicals: Zinc sulphate (ZnSO4), disodium edetate (C10H16N2O8), ammonium acetate (C2H7NO2), acetic acid (CH3COOH), and dithizone (C13H12N4S), etc.

Preparation of 0.1 M zinc sulphate solution:

Take properly weighed 28.80 gm of zinc sulphate and dissolve in 800 ml of distilled water, once it has completely dissolved, make up the volume to 1000 ml.

Preparation of acetic acid-ammonium acetate buffer:

Take 07.70 gm of ammonium acetate in 50 ml of distilled water and add 05.70 ml of acetic acid, once it has completely dissolved, make up the volume to 100 ml with water.

Titration procedure:

  • All glassware should be cleaned and dried according to standard laboratory procedures.
  • Before filling the burette for the titration, rinse it with distilled water and then pre-rinse it with a portion of the titrant solution. Pre-rinsing is required to make sure that all solution in the burette is the desired solution, not a contaminated or diluted solution.
  • Take the unknown stock solution of titrant in a clean and dry beaker then fill the burette using the funnel.
  • Remove air bubbles from the burette and adjust the reading to zero.
  • Take 10.00 ml of a previously standardized solution of 0.1 M EDTA and pour into a conical flask.
  • Add 04.00 gm of ammonium acetate.
  • Then add 10.00 ml of acetate buffer and 50.00 ml alcohol.
  • Add 02.00 ml of dithizone TS as an indicator and shake well.
  • Titrate it with prepared 0.1 M zinc sulphate solution with constant stirring until the endpoint.
  • The actual endpoint is indicated by a rose pink color.
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.
  • Take their mean and calculate the molarity of the zinc sulphate solution.

Observation table:


Sr. No.

Content in conical flask

 

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:


Calculations:

1 ml of 0.1 M EDTA is equivalent to 0.02785 g of zinc sulphate.

M = Molarity of EDTA x 10 / reading of the burette

Result:

The strength of the prepared zinc sulphate solution was found to be_____M.
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