Showing posts with label Acid-base titration. Show all posts
Showing posts with label Acid-base titration. Show all posts

Tuesday, August 23, 2022

Why acid-base titration is important in food industry

The analysis of food products by titration ensures that the foods have a balanced composition.

In the last few years, the food industry's quality standards have grown a lot and sometimes reached the level of the pharmaceutical industry. Because of this, more and more modern piston burettes and automatic titrators are being used in the food lab because they meet the requirements for accuracy, reliability, and being ability to keep records.

What is titration?

Titration is an analytical technique in chemistry used to determine the concentration of an unknown component in a sample. It is a type of quantitative chemical analysis utilized in a variety of industries, such as pharmaceutical, food processing, water, textile, dairy, petroleum, chemical manufacturing, and agriculture sector.

The principle behind titration is that we add a solution, called a titrant, to the sample (analyte) we want to analyze. A known chemical in the titrant will react with the sample. A burette is used to add the titrant. Using this tool; we can exactly know the volume of the titrant. 

As soon as we do this, a chemical reaction will happen in the sample, which will change its characteristics. At the endpoint or equivalence point of the reaction, the substance reacts with the titrant and the color of the indicator changes.

According to the nature of the chemical reaction occurring between the titrant and sample, there are four types of titrations, including acid-base, redox, complexometric, and precipitation titration. They make it possible for food manufacturers to determine the amount of a reactant present in a sample. 

For example, it can be used to determine the amount of salt or sugar present in a product, as well as the concentration of vitamin C or vitamin E, both of which affect the color of the product.

Importance of acid-base titration:

The purpose of a titration is to determine the concentration of the sample solution by titrating the acid solution with a basic solution whose concentration is already known, or vice versa, until the solution is neutralized.

In food processing, the acidity of fruit juice is determined using acid-base titration. Redox titration can be used to determine the concentration of vitamin C in orange juice. The salt content of various foods can be determined using the precipitation titration method.

For salt testing, several food manufacturers employ manual titration techniques. To measure the concentration of salt the Mohr's method one of the oldest titration methods, this uses a silver nitrate solution. The potentiometric titration method is one option that can be performed automatically. This sample measures the change in the membrane potential of the substance.

Three industries in the industrial sector that depends on titration techniques are food processing, pharmaceutical production, and chemical manufacturing. They are used in many significant fields including product research and development, quality control, and large-scale production. In these fields, raw materials need to be calibrated at a high level, and titration can help with this.

Titration is essential to ensure the consistency of products sold, even when advanced processes such as gas chromatography (GC) or liquid chromatography (HPLC) are unavailable to most wineries for practical reasons.


Here are some of the reasons why titration is still used so often today.
  • It is one of the most accurate quantitative analysis techniques.
  • It is simple to perform and is economical, requiring little in the way of equipment.
  • Methods can use for concentrations of the ppm up to 100%.
  • It does not require a high level of skill.
  • The results are readily available right away.


People also ask

How are acid base titrations used in the food industry?
Where is acid base titration used in industry?
Why are acid base titrations important?
Why is titration important in real life?
Where is acid base titration used in industry?
What is the importance and application of acid base titration?
Why is titration important in a laboratory?
What are the applications of acid base titration?
What is the real life application of acid base titration?
How is titration used in the pharmaceutical industry?
Posted by No comments:
Labels: ,

Determination of acetic acid in vinegar

Learn about the assay of acetic acid in a given sample of vinegar using 0.1 n sodium hydroxide through a laboratory experiment or practical.

To determine the percentage purity of acetic acid in a given sample of vinegar using 0.1 n NaOH


Requirements:

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

Chemicals: LR grade sodium hydroxide (NaOH), acetic acid (CH3COOH), phenolphthalein indicator, etc.

Apparatus: Digital/analytical balance

The determination of acetic acid in vinegar by direct titration:

The major components in vinegar are acetic acid and water. It is a carbon-based compound with a –COOH functional moiety with a single ionizable proton. Vinegar derives its acidity from acetic acid (CH3COOH or HC2H2O2). Acetic acid, (Ethanoic acid), is a weak acid that is a type of organic acid (carboxylic acid).

CH3COOH(aq) + NaOH(aq) -> CH3COONa(aq) + H2O(l)

Phenolphthalein or thymol blue are ideal indicators for this titration since the pH at the equivalence point will be larger than 07 when weak acids like acetic acid are titrated with strong bases like NaOH solution.

By titrating an appropriate sample of commercial vinegar with the standardized NaOH solution, it is simple to determine the amount of acetic acid (CH3COOH) present in the vinegar. This experiment requires two steps; first, we must standardize the sodium hydroxide standard solution, followed by the acetic acid test.

Click here to get the procedure for standardization of the sodium hydroxide solution:

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 commercial vinegar sample and pour it into a 250 ml conical flask.
  • Add 5 ml of distilled water using a pipette.
  • Add 2-4 drops of phenolphthalein indicator and thoroughly mix the mixture.
  • Titrate this solution with NaOH solution until the endpoint is reached.
  • The actual endpoint is indicated by the appearance of a pale pink color.
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.
  • Take their mean and calculate the % acetic acid in vinegar.

Observation table:

Sr. No.

Content in conical flask

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Calculations:

Calculate the solution's molarity using the following formula.
Moles of acetic acid = (MNaOH)(VNaOH) 

Grams of acetic acid = (moles of acetic acid)(MW)

Grams of vinegar =(volume of vinegar)(density of vinegar)

% acetic acid = (grams of acetic acid / grams of vinegar) x 100


Result:

The concentration of acetic acid in the vinegar solution: _________ %.



People also ask:

Assay of acetic acid by titration
Assay of acetic acid using sodium hydroxide
How will you determine acetic acid in vinegar?
What is the acid content in vinegar lab?
What is the amount of acetic acid in vinegar?
Determination of the concentration of acetic acid in vinegar lab report
Determination of acetic acid in vinegar using naoh
Determination of acetic acid concentration in vinegar using titration lab report
Determination of acetic acid in vinegar pdf
Determination of acetic acid in vinegar conclusion
Molarity of acetic acid in vinegar
Determine the concentration of acetic acid in vinegar



Posted by No comments:
Labels: ,

Monday, August 22, 2022

Prepare and standardize 0.1 n NaOH using succinic acid

Learn about the preparation and standardization of 0.1 n NaOH solution using succinic acid through a laboratory experiment or practical.

To prepare and standardize 0.1 n NaOH using succinic acid as a primary standard


Requirements:

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

Chemicals: LR grade sodium hydroxide (NaOH), succinic acid (C4H6O4), phenolphthalein indicator, etc.

Apparatus: Digital/analytical balance

Theory:

Solid NaOH can't be used as a primary standard as it can't be available in a pure form. This is because it absorbs moisture and carbon dioxide from the air when it is stored and also when it is weighed. 

This reaction consumes hydroxide ions, changing the concentration of a standard sodium hydroxide solution. Thus, sodium hydroxide solutions must be standardized before any analytical use.

For standardizing NaOH, we can use various primary standards such as potassium hydrogen phthalate (PHP), succinic acid, benzoic acid, sulfamic acid, etc.

In this experiment, a standard solution of succinic acid is used as a primary standard to determine the exact concentration of sodium hydroxide. Succinic acid, which dissolves in water to form H+ and succinate ions, is a pure and stable substance that contains two titrable acidic hydrogens. 

In this reaction, we use phenolphthalein as an indicator that changes color from colorless to faint pink at the endpoint/equivalence point.

Preparation of 0.1 M NaOH solution:

To make 0.1 M NaOH solution, weigh accurately 02.00 gm of NaOH and dissolve in 200 ml of distilled water in a volumetric flask, and properly mix it. Once it has completely dissolved, make up the volume to 500 ml.

Preparation of 0.1 M standard succinic acid solution:

To make 0.1 M standard succinic acid solution, weigh accurately 0.59 gm of succinic acid and dissolve in 70 ml of distilled water in a volumetric flask, and properly mix it. Once it has completely dissolved, make up the volume to 100 ml.

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 succinic acid solution and pour it into a 250 ml conical flask.
  • Add 2-4 drops of phenolphthalein indicator and mixed thoroughly the mixture.
  • Titrate this solution with NaOH solution until the endpoint is reached.
  • The actual endpoint is indicated by the appearance of a faint 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 sodium hydroxide solution.

Observation table:

Sr. No.

Content in conical flask

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Calculations:

Calculate the solution's molarity using given formula.
NNaOH  x   VNaOH   =     N(succ. acid.)   x V(succ.acid.)  

Volume of succinic acid solution in each titration = 10 m
Normality of succinic acid = 0.1 M

Result:

The strength of the prepared sodium hydroxide (NaOH), solution was found to be_____M.


People also ask:

How do you prepare and standardize 0.1 N NaOH solution?
What are the steps involved in standardization of approx 0.1 N NaOH?
Which of the following compound is used for the standardization of 0.1 N NaOH?
What is the reaction between succinic acid and NaOH?
What is the type of titration between succinic acid and sodium hydroxide?
What is the standardization of NaOH?
Standardization of NaOH solution lab report
Posted by No comments:
Labels: ,

Saturday, August 20, 2022

Preparation and standardization of 1N HCl

Learn about the preparation and standardization of 1N hydrochloric acid solution through a laboratory experiment or practical.

To prepare and standardize 1 N HCl using sodium carbonate as a primary standard.

Requirements:

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

Chemicals: LR grade concentrated hydrochloric acid (HCl), sodium carbonate, (Na2CO3), methyl red indicator, etc.

Apparatus: Digital/analytical balance

Principle of standardization of HCl:

In the titration of hydrochloric acid against the solution of sodium carbonate, methyl red (a weak base) which is yellow in the unionized form is used as an indicator.

When a weak base is used to titrate a solution that is just slightly acidic the endpoint is also slightly acidic. The solution is slightly alkaline when a weak acid is titrated with a strong base because the salt formed is partially hydrolyzed.

The reaction of sodium carbonate with hydrochloric acid is given below:

Na2CO3 + 2HCl → 2NaCl + H2O + CO2

In the process of acid-base titration, the portion of acid becomes chemically equivalent to the quantity of base present. When a strong acid and a strong base are tested at the same time, the solution turns out to be neutral.

Preparation of 1 N HCl solution:

Pipette out accurately 08.50 ml of concentrated hydrochloric acid (HCl) and dilute to 100 ml of distilled water in a volumetric flask, and properly mix it.

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 primary standard anhydrous sodium carbonate (Na2CO3) and dry it at 150°C for 1 hour in a Petri dish or crucible.
  • Once it is cool, weigh accurately 01.50 g sodium carbonate and pour it into a conical flask.
  • Pour in 100 ml of water and stir the mixture to dissolve.
  • Add 2-3 drops of methyl red indicator.
  • Titrate the sample solution with the prepared HCl solution until the light pink color appears.
  • Heat the solution to boiling until the color returns to yellow, then cool and titrate again until the light pink color is no longer affected by boiling.
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.

Observation table:

Sr. No.

Content in conical flask

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Calculations:

Each ml of 1M HCl is equivalent to 0.05299g of Na2CO3.
Calculate the solution's molarity using the following formula.
Molarity = Wt. X 1 / volu. X 0.05299
Where,
Wt. is weight of Na2CO3 used,
Volu. is volume of HCl solution used in titration

Result:

The strength of the prepared hydrochloric acid (HCl) solution was found to be_____N.


People also ask

How do you prepare 1N HCl solution?
What is the procedure for standardization of hydrochloric acid?
How do you make 1N HCl from HCl?
How can we prepare 0.1 N HCl in 100 ml?
Standardization of hcl with na2co3 lab report
Standardization of hcl with na2co3 calculations


You may also like this
Posted by No comments:
Labels: ,

Thursday, August 18, 2022

Standardization of HCl solution

Learn about the preparation and standardization of hydrochloric acid solution through a laboratory experiment or practical.

To prepare and standardize 0.1 N HCl using sodium carbonate as a primary standard.


Requirements:

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

Chemicals: LR grade concentrated hydrochloric acid (HCl), sodium carbonate, (Na2CO3), methyl orange indicator, etc.

Apparatus: Digital/analytical balance

Principle of standardization of HCl:

In the titration of hydrochloric acid against the solution of sodium carbonate, methyl orange (a weak base) which is yellow in the unionized form is used as an indicator.

Standardization of HClWhen a weak base is used to titrate a solution that is just slightly acidic the endpoint is also slightly acidic. The solution is slightly alkaline when a weak acid is titrated with a strong base because the salt formed is partially hydrolyzed.

The reaction of sodium carbonate with hydrochloric acid is given below:

Na2CO3(aq) + 2HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l)
CO32-(aq) + 2H+(aq) → CO2(g) + H2O(l)

In the process of acid-base titration, the portion of acid becomes chemically equivalent to the quantity of base present. When a strong acid and a strong base are tested at the same time, the solution turns out to be neutral.

Preparation of 0.1 N HCl solution:

Pipette out accurately 08.50 ml of concentrated hydrochloric acid (HCl) and dilute in 500 ml of distilled water in a volumetric flask, and properly mix it. Once it has completely dissolved, make up the volume to 1000 ml with distilled water.

Preparation of sodium carbonate standard solution:

The molecular weight of sodium carbonate is 106. Therefore, weigh accurately 0.53 gm of Na2CO3 and dissolve in 50 ml of distilled water in a volumetric flask, once it has completely dissolved, make up the volume to 100 ml.

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 primary standard anhydrous sodium carbonate (Na2CO3) and dry it at 250°C for 4 hours in a Petri dish or crucible.
  • Once it is cool, weigh accurately 0.22 g sodium carbonate and pour it into a conical flask.
  • Pour in 50 ml of water and stir the mixture to dissolve.
  • Add 2-3 drops of methyl orange indicator.
  • Titrate the sample solution with the prepared HCl solution until the light pink color appears.
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.

Observation table:

Sr. No.

Content in conical flask

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Calculations:

Calculate the normality of the HCl solution (N),

As follows:

N = A /0.053*B

Where
A - gram of Na2CO3 used,
B - used ml of HCl solution in titration.

Result:

The strength of the prepared hydrochloric acid (HCl) solution was found to be_____N.


Frequently Asked Question (FAQ):

Why methyl orange is used in the standardization of HCl with Na2CO3?

Methyl orange is a better indicator for the titration of hydrochloric acid with sodium carbonate since the endpoint of the reaction falls in the pH range of 3.0 to 4.4 which is the pH range of Methyl orange.

What is the purpose of standardizing HCl acid solution?

To determine the concentration of a prepared solution of HCl we perform the standardization. Standardization is the process of determining a solution's exact concentration (Molarity/Normality). We can also use standard NaOH to measure the molarity of a hydrochloric acid solution.

What primary standard is taken in HCl standardization?

Usually, sodium carbonate (Na2CO3) is used as the primary standard in the standardization of HCl, as it complies with all the requirements (properties) of the primary standard. It has a high molecular weight, high purity, is non-toxic, is easy to weigh, and is non-hygroscopic.



People also ask

How to calculate the molarity of standardized HCl
How to prepare a standard solution of HCl
How do you prepare and standardize 0.1 N HCl?
How do you make a standard solution of HCl?
How do you standardize HCl with Na2CO3?
Which primary standard is used for the standardization of HCl?
Posted by No comments:
Labels: ,

Wednesday, August 17, 2022

Standardization of NaOH with KHP

Learn about the preparation and standardization of NaOH solution through a laboratory experiment or practical.

To prepare and standardize 0.1N sodium hydroxide solution with potassium hydrogen phthalate by acid-base titration.


Requirements:

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

Chemicals: LR grade potassium hydrogen phthalate (C8H5KO4), sodium hydroxide (NaOH), phenolphthalein indicator, etc.

Apparatus: Digital/analytical balance

Theory for standardization of NaOH:


When sodium hydroxide is weighed, it takes moisture from the air because it is hygroscopic. Because of this water, we will not be able to find out the exact mass of NaOH. Therefore to determine the exact concentration of prepared sodium hydroxide solution, titration with a solid acid that is not hygroscopic is required.

KHP, also known as potassium hydrogen phthalate, is an acidic salt compound. It is used as the primary standard because it has high purity, is non-toxic, has a high molecular weight, is non-hygroscopic, and is easy to weigh. For the purpose of determining the concentration of a solution containing sodium hydroxide, we will use this primary standard.

It is an acid-base titration in which sodium hydroxide is a strong base and potassium hydrogen phthalate is a weak acid. By direct titration, we standardize the 0.1 N NaOH solution (the titrant) with potassium hydrogen phthalate (KHP, KC8H4O4H) using phenolphthalein as an indicator.

KHP is a weak acid, and its reactions with bases are as follows:

Standardization of NaOH

Preparation of 0.1N NaOH solution:

Weigh accurately 0.2 gm of sodium hydroxide and dissolve in 40 ml of distilled water in a volumetric flask, and properly mix it. Once it has completely dissolved, make up the volume to 50 ml with distilled water.

Preparation of 0.1N KHP solution:

Weigh accurately 1.02 gm of potassium hydrogen phthalate and dissolve in 40 ml of distilled water in a volumetric flask, and properly mix it. Once it has completely dissolved, make up the volume to 50 ml with 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 05.00 ml of prepared KHP solution and pour it into a conical flask.
  • Add 2-3 drops of phenolphthalein indicator.
  • Titrate the sample solution with the sodium hydroxide (NaOH) solution until the color of the solution is discharged.
  • To get accurate results, repeat the titration three times.
  • Properly record the readings of the burette.

Observation table:

Sr. No.

Content in conical flask

Burette reading

Volume of titrant used (ml)

Initial

Final

1

 

 

 

 

2

 

 

 

3

 

 

 

 

Mean:

Calculations:

Calculate the normality and % of NaOH.

meq. NaOH = meq KHP

(N * V)NaOH = (N * V)KHP

Wt./ Eq.Wt * 1000 = ( N * V) KHP

Wt./40*1000 = 0.1 x V1 X V2 X V3/3

% NaOH = Wt./Wt. of sample X 100


Result:

The strength of the prepared NaOH solution was found to be_____M.




People also ask

Why is KHP used as a primary standard?
How do you standardize NaOH with KHP?
How do you calculate standardized NaOH?
Why is phenolphthalein used for KHP and NaOH?
What is the purpose of standardization of NaOH?
Give 3 reasons why NaOH is not used as a primary standard?
Why NaOH percentage less than 100%?
Standardization of naoh with khp lab report
Posted by No comments:
Labels: ,
Subscribe to: Posts (Atom)