World’s first cloned buffalo gives birth to calf in Karnal

The cloned buffalo Garima II on Friday gave birth to a calf at the Karnal-based National Dairy Research Institute (NDRI) on Friday.

The calf, named Mahima, was born through ‘hand-guided cloning technique’.It weighs 32 kg and is reported to be normal and healthy.

The newborn “Mahima” is keeping good health and started suckling of milk within 30 minutes of birth, said A.K. Srivastava, Director, National Dairy Research Institute.

“It is a big success and a proud moment for India. It is the first calf born from a cloned buffalo in the world,” he said.

It is a future technique and it has opened many doors for the scientists in the field of dairy research, said Srivastava.Garima II, born on August 22, 2010 attained maturity in 19 months compared to her contemporaries that normally take 28 months. It was inseminated with frozen-thawed semen of a progeny tested bull of NDRI on March 27, 2012, he said.

She was maintained under standard scientific management system during the gestation period.

On Friday, she showed impending calving symptoms and was given medical care. She calved normally upon medical assistance. According to Srivastava, when Garima II was born, she also weighed 32 kg .

The NDRI is known across the globe and came into the limelight for production of world’s first buffalo cloned calf Garima.

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Cadbury Dairy Milk

Dairy Milk is a brand of milk chocolate currently manufactured by Cadbury, except in the United States where it is made by The Hershey Company. It was introduced in the United Kingdom in 1905 by and now consists of a number of products. Every product in the Dairy Milk line is made with exclusively milk chocolate.
In June 1905 in England, Cadbury made its first Dairy Milk bar, with a higher proportion of milk than previous chocolate bars, and it became the company's best selling product by 1914. George Cadbury Junior, responsible for the development of the bar, has said "All sorts of names were suggested: Highland Milk, Jersey and Dairy Maid. But when a customer’s daughter suggested Dairy Milk, the name stuck.".Fruit and Nut was introduced as part of the Dairy Milk line in 1928, soon followed by Whole Nut in 1933. By this point, Cadbury's was the brand leader in the United Kingdom. In 1928, Cadbury's introduced the "glass and a half" slogan to accompany the Dairy Milk bar, to advertise the bar's higher milk content.
In September 2012, Cadbury made the decision to change the shape of the bar chunks to a more circular shape to keep the bar current. The bar had not seen such a significant change in shape since 1905.

Cadbury has a trademark in the United Kingdom for the distinctive purple it uses on the wrappers of its milk chocolate bars.

DETERMINATION OF AVAILABLE CHLORINE IN CHLORINE STERILIZER

Principle:

The chemical sterilization of some of the dairy equipment is carried out by hypochlorite solution. Different strengths are suggested for different types of operations. The stock solution of sodium hypochlorite with about 5 percent available chlorine is available. As the strength of chlorite sterilizers decreases on storing it is necessary to check the strength. This method is based on the reaction between available chlorine from hypochlorite solution and acidified potassium Iodine solution in which Iodine is liberated.

            NaOCL + 2 KI + 2CH₂COOH                      NaCl + 2CH₂COOK + I₂ + H₂O

The liberated Iodine is titrated against N/10 sodium thiosulphate using starch as indicator. From the reading of sodium thiosulphate the quantity of available chlorine can be found out.

Procedure:

1.      Pipette 10 ml of the sodium hypochlorite sample into 250 ml volumetric flask.

2.      Make up the volume upto the mark with distilled water and mix well.

3.      Pipette 25 ml of diluted solution in a conical flask.

4.      Add 2 g. potassium Iodine crystals to the solution and dissolve them followed by 10 ml glacial acetic acid.

5.      Available chlorine which is liberated from hypochlorite by the action of acid liberates an equivalent amount of Iodine from potassium Iodine which produces a yellowish brown colour.

6.      Immediately titrate the mixture against N/10 sodium thiosulphate until the brown colour changes to light straw yellow.

7.      Immediately add 1 percent of freshly prepared starch solution and titrate till the colour disappears.

8.      Note the reading of N/10 sodium thiosulphate as V ml.

9.      Make the blank determination using the same reagents and deduct from     V ml.

10. Record the values of both the titration in appropriate table.

Observation:

Burette reading	Titration I	Titration II	Titration III
Final reading
Initial reading
Volume delivered in ml.

Calculation:

1 ml of N/10 sodium thiosulphate = 0.003546 g. available chlorine

V ml of N/10 sodium thiosulphate = (V) (0.003546) g. available chlorine

This quantity of chlorine is from 25 ml diluted solution

    V X 0.003546 X 250

Therefore, available chlorine in 250 ml diluted solution =                                  = x

                                                                                                                 25

Which is equal to 10 ml of stock solution  = x

                                                                         x  X 100

Therefore, percent of available chlorine =                        = 10 x

                                                                             10

Note: If necessary the dilution of stock solution can be changed and the above formula will have to be modified accordingly.

Result: The available chlorine in chlorine sterilizer is ________ %

STANDARDISATION OF AgNO3 SOLUTION (MOHR’S METHOD)

Principle:

Silver nitrate reacts with sodium chloride and forms a white precipitate of silver chloride

            AgNO₃ + NaCl                 AgCl + NaNO₃

When all the chloride ions are precipitated as AgCl, excess of AgNO₃ reacts with potassium chromate indicator and forms a reddish brown precipitate of silver chromate. 

            2 AgNO₃ + K₂CrO₄                   Ag₂CrO₄ + 2 KNO₃

Procedure:

1.      Weigh accurately about 1.5 g. of NaCl (Equivalent weight = 58.46) transfer to a 250 ml volumetric flask.

2.      Dissolve with a little quantity of distilled water and make up the volume with distilled water to the mark. Mix the solution thoroughly.

3.      Fill the burette with the given silver nitrate solution.

4.      Pipette out exactly 25 ml of the NaCl solution into a 250 ml conical flask.

5.      Add few drops of potassium chromate (5% aqueous solution) and mix the content of the flask.

6.      Run down the AgNO₃ solution from the burette into the conical flask in small quantities till the reddish brown precipitate begins to appear, which is the end point.

7.      Repeat the above experiment till concordant titration values are obtained.

8.      Carryout a blank with 25 ml of distilled water and same quantity of K₂Cr₂O₄ to get reddish brown colour when titrated with AgNO₃.

9.      Deduct the blank reading with previous reading obtained for NaCl solution.

Calculation:

Volume of NaCl pipetted out                     = V₁ ml

Normality of NaCl (by calculation)          = N₁

Volume of AgNO₃                                        = V₂ ml

                                                                    V₁   X  N₁

Normality of AgNO₃  (N₂)               =

                                                                           V₂

Result: The strength of the given AgNO₃ solution = _____ N

STANDARDISATION OF IODINE SOLUTION

Principle:

Iodine reacts with sodium thiosulphate forming sodium iodine and sodium tetrathionate. The end point of the reaction is indicated by the disappearance of the blue colour produced by the solution with the starch indicator

            2Na₂S₂O₃ + I_2­                  Na₂S₄O₆ + 2NaI

Procedure:

1.      Rinse a clean burette with the N/10 sodium thiosulphate solution.

2.      Fill the burette with thiosulphate solution and fix it to the stand.

3.      Pipette out given 25 ml of Iodine solution to an Erlenmeyer flask and add 100 ml distilled water with a measuring cylinder.

4.      Run down the thiosulphate solution to the Iodine solution in the flask till the colour of the solution turns to straw yellow.

5.      At this stage add about 1 ml of freshly prepared starch indicator into the flask when an intense blue colour is formed. Mix well.

6.      Continue the addition of the thiosulphate solution drop wise till the blue colour disappears (the first disappearance of the blue colour should be considered the correct end point since the blue colour reappears after some time).

7.      Note the volume of the thiosulphate required to affect the disappearance of the blue colour.

8.      Repeat the experiment till at least two concordant results are obtained.

9.      Record the burette readings in the tabular form.

Observation:

Burette reading	Titration I	Titration II	Titration III
Final reading
Initial reading
Volume delivered in ml.

Calculation:

Volume of N/10 Na₂SO₃ required to react with 25 ml of Iodine solution = V₁ ml

Volume of Na₂S₂O₃  X  Normality = Volume of Iodine (V₂)  X  Normality (N₂)

                                    V₁ X N₁

Therefore   N₂ =

                                         V₂

N₂ X Equivalent weight of Iodine (126.9) = g / l

Result: The given iodine solution contains ____ g. of iodine per liter

ESTIMATION OF SODIUM HYDROXIDE AND SODIUM CARBONATE IN THE GIVEN MIXTURE OF A SOLUTION (DETERGENT)

Principle:

The detergent used in Dairy contains a mixture of sodium carbonate (1.5%) and sodium hydroxide (0.5%). It is necessary to check carbonate and caustic alkalinity because NaOH is converted into Na₂CO₃ when it is exposed to atmosphere due to absorption of CO₂ from the atmosphere. The reaction of Na₂CO₃ with acid is a two-step process

 

I

            2 NaOH + H₂SO₄                       Na₂SO₄ + 2H₂O                                  

            2 Na₂CO₃ + H₂SO₄                    2 NaHCO₃ + Na₂SO₄                  

            2 NaHCO₃ + H₂SO₄                   Na₂ SO₄ + 2 CO₂                        II

When the solution containing both Na₂CO₃ and NaOH are titrated against standard acid using phenolphthalein as indicator entire NaOH and ½ of Na₂CO₃ (step – I) will be neutralized at the end point. Remaining ½ of Na₂CO₃ (step – II) can be titrated using methyl orange as indicator.

Procedure:

1.      Rinse a clean burette with the given N/10 sulphuric acid solution.

2.      Fill the burette with the sulphuric acid solution and fix it to the stand.

3.      Pipette out 25 ml of the mixture solution to a Erlenmeyer flask.

4.      Add 1 – 2 drops of phenolphthalein indicator and mix the contents of the flask.

5.      Run down the sulphuric acid solution from the burette and mix the contents of the flask.

6.      Note the volume of the acid required to change the pink colour to colourless.

7.      Now add a drop of methyl orange indicator and continue titration till the yellow colour just change to a light orange colour.

8.      Repeat the titration till at least two concordant readings are obtained.

9.      Record the result in a tabular form.

Observation:

Burette reading	Titration I	Titration II	Titration III
With phenolphthalein indicator
Final reading
Initial reading
Volume delivered in ml.
With methyl orange indicator
Final reading
Initial reading
Volume delivered (ml)

Calculation:

For sodium carbonate

Normality of acid                             =          0.1 N

Volume of acid of second titration           =          V ml

Volume of acid required to neutralize all Na₂CO₃ in the given mixture = 2 X V ml.

                                                            2 X V X 0.1                         

Strength of sodium carbonate =     

                                                                     25

Weight per litre of sodium carbonate =  Strength  X  Equivalent weight

Strength  X   53.0  g / l or Percent of Na₂CO₃ =  Strength  X  5.3

For sodium hydroxide

Normality of acid = 0.1 N

Volume of acid required for first titration  – volume for second titration (V ml) = x ml

                                                x X 0.1

Strength of NaOH =  

                                                   25

Weight per litre NaOH = strength X equivalent weight = Strength  X   40

Percent of NaOH = Strength X 4.0.

PREPARATION OF STANDARD SODIUM CARBONATE SOLUTION AND STANDARDIZATION OF THE GIVEN ACID SOLUTION

 Principle:

One gram equivalent of Na₂CO₃ (53 g) dissolved in 1000 ml water gives 1N solution Na₂CO₃ is a weak alkali and used in standardization of acid solution. When a solution of a weak alkali is titrated against a strong acid, methyl orange indicator should be used.

            Na₂CO₃ + H₂SO₄                   Na₂SO₄ + H₂O + CO₂

Procedure:

A.  Preparation of standard Na₂CO₃ solution:

1.      Weigh by difference into a 250 ml beaker accurately about 1.325 g. of sodium carbonate using a weighing bottle.

2.      Add some distilled water into the beaker and dissolve the sodium carbonate with the help of glass rod.

3.      Transfer the solution into a clean 250 ml volumetric flask through a funnel.

4.      Wash the beaker 3 – 4 times with small amounts of distilled water and transfer the washings into the volumetric flask.

5.      Make up the volume with distilled water to the mark.

6.      Shake the solution thoroughly.

B.  Titration of given acid solution with standard Na₂CO₃ solution:

1.      Take clean burette and rinse it with the given sulphuric acid solution.

2.      Fill the burette with sulphuric acid solution and fix it in a burette stand.

3.      Pipette out 25 ml of the prepared sodium carbonate solution into a 250 ml Erlenmeyer flask.

4.      Add one drop of methyl orange indicator and mix the contents of the flask.

5.      Run down acid solution from the burette slowly and mix the contents of the flask.

6.      Note the volume of the acid required to change the colour of the solution into a permanent orange colour.

7.      Repeat the titration till at least two concordant readings are obtained.

Observation:

Weight of weighing bottle with sodium carbonate before transferring              =   a g.

Weight of weighing bottle with sodium carbonate after transferring    =   b g.

Weight of sodium carbonate transferred                                                     =   (a – b) g.

Normality of sodium carbonate solution

            (a – b)             1

N₂ =                 X

            1.325           10

Burette reading	Titration I	Titration II	Titration III
Final reading
Initial reading
Volume delivered in ml.

Normality of sodium carbonate solution = N₂

Volume of sodium carbonate solution     = V₂ (25 ml)

Volume of acid solution required            = V₁ ml

Normality of acid                                         = N₁ (to be calculated)

Calculation:

Volume of acid solution X normality of acid solution = Volume of alkali solution X normality of alkali

N₁ X V₁  =  N₂ X V₂

             N₂ X V₂

N₁ =                                         

                 V₁

                                           1000 X 0.1

1000 ml of 0.1 N acid =                  = x ml of given acid solution diluted to 1000ml                                                  N₂

Result: The strength of given sulphuric acid solution is _______

Note: To obtain anhydrous sodium carbonate, pure sodium carbonate in porcelain dish at 29°C for one hour. To ensure complete conversion of the sodium bicarbonate weight till a constant weight is obtained. Immediately transfer the dish containing sodium carbonate to a desiccator.