0
A normal solution contains 1 equivalent mass, in grams, of the solute in 1 litre of solution. Firstly, you calculate the mole mass of ammonium acetate.
(77g). Weigh this out in a small, clean beaker.
Add de-ionized water to dissolve the solid, then transfer the solution to a 1 litre volumetric flask, remembering to wash out the beaker three times with small volumes of de-ionized water, and add the washings to the volumetric flask. Similarly rinse the glass rod with small volumes of the water into the flask.
Now add de-ionized water to the 1 litre mark and then mix the solution thoroughly by inverting the stoppered flask many times.
Normality is not used much any more, molarity is more usual, though for this solid the two happen to be the same. Ammonium acetate has the systematic name ammonium ethanoate.
Wiki User
∙ 9y ago
Add your answer:
Earn +20 pts
How do you prepare 200ml of ethyl acetate of 0.1 Normality solution?
Density of etyl acetate
How can a solution of ammonia be used to prepare ammonia sulphate?
A solution of ammonia can be used to prepare ammoniumsulfate by reacting it with a solution of sulfuric acid to produce a solution of ammonium sulfate, which can be dried if desired to prepare solid ammonium sulfate.
How do you prepare 6 percent Ammonium Acetate?
Weight 6 gram NH4-O2C-CH3 and add this to 96 g H2O and you'll have 100 g of the desired 6% solution. Simple though?
How do you prepare one liter of a 1.25M ammonium hydroxide solution?
This depends on the concentration of the primary solution; for a 25 % ammonium hydroxide solution you need 85,15 mL.
Why it is recommended to prepare ferrous ammonium sulfate solution in acidic medium?
It is recommended to prepare ferrous ammonium sulphate solution in acidic medium because iron when combined with water gives the precipitates of oxides of Iron.
How do you prepare 200ml of ethyl acetate of 0.1 Normality solution?
Density of etyl acetate
How do you prepare 100mM ammonium acetate?
To prepare the buffer using solid form reagents, prepare a 0.1 M ammonium acetate solution by dissolving 7.7 g ammonium acetate in a 1000 ml water. Adjust 1 L of this solution to pH 4.5 by adding acetic acid (about 8 ml) and 5 ml of 1 M p-TSA (equivalent to 5 mM p-TSA).
Preparation of 0 38 M sodium acetate solution?
how will you prepare 0.38M sodium acetate solution
How can a solution of ammonia be used to prepare ammonia sulphate?
A solution of ammonia can be used to prepare ammoniumsulfate by reacting it with a solution of sulfuric acid to produce a solution of ammonium sulfate, which can be dried if desired to prepare solid ammonium sulfate.
How do you prepare acetate buffer pH 3.5?
Dissolve 25g of Ammonium acetate in 25ml of water and add 38ml of 7M hydrochloric acid. Adjust the pH of the solution to 3.5 with either 2M hydrochloric acid or 6M ammonia and dilute with water to 100ml
How do you prepare 6 percent Ammonium Acetate?
Weight 6 gram NH4-O2C-CH3 and add this to 96 g H2O and you'll have 100 g of the desired 6% solution. Simple though?
How do you prepare one liter of a 1.25M ammonium hydroxide solution?
This depends on the concentration of the primary solution; for a 25 % ammonium hydroxide solution you need 85,15 mL.
How do you prepare a solution sodium chloride normality?
Dissolve 39,665 g NaCl in 1 kg water.
Why it is recommended to prepare ferrous ammonium sulfate solution in acidic medium?
It is recommended to prepare ferrous ammonium sulphate solution in acidic medium because iron when combined with water gives the precipitates of oxides of Iron.
How do you prepare ammonium chloride?
Mix ammonia with a solution of hydrochloric acid, then evaporate the solution. The remaining salt is what you want.
How do you prepare 0.1 NORMALITY of silver- nitrate solution?
Dissolve 16,99 g silver nitrate in 1 L demineralized water.
How do you prepare 6n ammonium hydroxide from 30 percent solution?
To prepare 6 nM ammonium hydroxide a 30 percent solution you need to know the volume of the 30 percent solution that you have and the volume of 6nM solution you would like to make. Then use the following formula: C1V1 = C2V2 where C = concentration in moles/Liter and V = volume in liters.
