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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.
What else can I help you with?
How do you prepare 6 percent Ammonium Acetate?
To prepare a 6% solution of Ammonium Acetate, weigh out 6 grams of Ammonium Acetate and dissolve it in 100 mL of water. Stir the mixture until the Ammonium Acetate is fully dissolved. This will give you a 6% Ammonium Acetate solution.
How do you prepare 200ml of ethyl acetate of 0.1 Normality solution?
To prepare 200ml of 0.1 N ethyl acetate solution, you will need to calculate the amount of ethyl acetate needed. Since the molecular weight of ethyl acetate is around 88.11 g/mol, for 200ml of 0.1 N solution, you would need around 1.76g of ethyl acetate. Dissolve this amount of ethyl acetate in distilled water to make up the final volume to 200ml.
How do you prepare 0.1 n ammonium ferrous sulphate solution?
To prepare 0.1N ammonium ferrous sulfate solution, weigh out the appropriate amount of solid ammonium ferrous sulfate based on its molar mass. Dissolve this in distilled water in a volumetric flask to make up a final volume that corresponds to 0.1 normality. Make sure to stir well to ensure complete dissolution.
How can a solution of ammonia be used to prepare ammonia sulphate?
To prepare ammonium sulfate from a solution of ammonia, you would react the ammonia solution with sulfuric acid. The chemical equation for this reaction is: 2NH3 + H2SO4 → (NH4)2SO4. This reaction will result in the formation of ammonium sulfate, which can then be isolated by evaporating the water.
How do you prepare acetate buffer pH 5.0?
To prepare an acetate buffer at pH 5.0, you would mix a solution of acetic acid and sodium acetate. Calculate the appropriate quantities based on the Henderson-Hasselbalch equation. Typically, you would mix an acetic acid solution and a sodium acetate solution in the correct ratio to achieve the desired pH.
How do you prepare 6 percent Ammonium Acetate?
To prepare a 6% solution of Ammonium Acetate, weigh out 6 grams of Ammonium Acetate and dissolve it in 100 mL of water. Stir the mixture until the Ammonium Acetate is fully dissolved. This will give you a 6% Ammonium Acetate solution.
How do you prepare 100mM ammonium acetate?
To prepare 100mM ammonium acetate solution, weigh out the appropriate amount of ammonium acetate powder based on its molecular weight and add it to a known volume of water, such as 1 liter. The final volume should be adjusted by adding more water and then mix well to dissolve the powder completely.
How do you prepare 200ml of ethyl acetate of 0.1 Normality solution?
To prepare 200ml of 0.1 N ethyl acetate solution, you will need to calculate the amount of ethyl acetate needed. Since the molecular weight of ethyl acetate is around 88.11 g/mol, for 200ml of 0.1 N solution, you would need around 1.76g of ethyl acetate. Dissolve this amount of ethyl acetate in distilled water to make up the final volume to 200ml.
How do you prepare 0.1 n ammonium ferrous sulphate solution?
To prepare 0.1N ammonium ferrous sulfate solution, weigh out the appropriate amount of solid ammonium ferrous sulfate based on its molar mass. Dissolve this in distilled water in a volumetric flask to make up a final volume that corresponds to 0.1 normality. Make sure to stir well to ensure complete dissolution.
How can a solution of ammonia be used to prepare ammonia sulphate?
To prepare ammonium sulfate from a solution of ammonia, you would react the ammonia solution with sulfuric acid. The chemical equation for this reaction is: 2NH3 + H2SO4 → (NH4)2SO4. This reaction will result in the formation of ammonium sulfate, which can then be isolated by evaporating the water.
How do you prepare acetate buffer pH 5.0?
To prepare an acetate buffer at pH 5.0, you would mix a solution of acetic acid and sodium acetate. Calculate the appropriate quantities based on the Henderson-Hasselbalch equation. Typically, you would mix an acetic acid solution and a sodium acetate solution in the correct ratio to achieve the desired pH.
How do you prepare a solution sodium chloride normality?
Dissolve 39,665 g NaCl in 1 kg water.
How would you prepare a sample of pure dry ammonium nitrate?
To prepare a sample of pure dry ammonium nitrate, dissolve ammonium nitrate in water to form a saturated solution, then allow the solution to cool and crystallize. Filter and dry the resulting crystals to obtain pure dry ammonium nitrate.
How do you prepare 0.1N potassium permanganate?
To prepare 0.1N potassium permanganate solution, dissolve 3.16 grams of potassium permanganate in 1 liter of water. This will give you a solution with a normality of 0.1N.
Preparation of 0 38 M sodium acetate solution?
To prepare a 0.38 M sodium acetate solution, you would need to dissolve the appropriate amount of sodium acetate trihydrate (CH₃COONa·3H₂O) in water. For example, to make 100 mL of a 0.38 M solution, you would dissolve 2.96 grams of sodium acetate trihydrate in sufficient water to make 100 mL. Ensure complete dissolution before use.
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 1 N ferrous ammonium sulphate?
To prepare 1 N ferrous ammonium sulfate solution, dissolve 392.15 g of the compound in distilled water and dilute to 1 L. This will yield a solution with a concentration of 1 N.
