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ammonium bicarbonate buffer

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From Wikipedia

Ammonium acetate

Ammonium acetate is a chemical compound with the formula CH3COONH4 (or C2H4O2.NH3 or C2H7NO2). It is a white solid, which can be derived from the reaction of ammonia and acetic acid. It is available commercially and, depending on grade, can be rather inexpensive.

Uses and distinctive properties

As the salt of a weak acid and a weak base, ammoniumacetate has a number of distinctive properties.

  • NH4C2H3O2 is occasionally employed as a biodegradable de-icing agent.
  • It is often used with acetic acid to create a buffer solution, one that can be thermally decomposed to non-ionic products
  • Ammonium acetate is useful in the Knoevenagel condensation in organic synthesis.
  • It is relatively unusual example of a salt that melts at low temperatures.
  • Can be used with distilled water to make a protein precipitating reagent.
  • Is often used as an aqueous buffer for ESImass spectrometry of proteins and other molecules.

Ammonium acetate is volatile at low pressures. Because of this it has been used to replace cell buffers with non-volatile salts, in preparing samples for mass spectrometry. It is also popular as a buffer for mobile phases for HPLC with ELSD detection for this reason. Other volatile salts which have been used for this include ammonium formate.


CH3COONH4 is hygroscopic. It decomposes easily at elevated temperatures into acetamide.


In this reaction, a salt is converted to two molecular species, which is a relatively uncommon conversion at mild temperatures.

From Yahoo Answers


Answers:Above 60 degrees C, sodium bicarbonate decomposes into sodium carbonate, water, and carbon dioxide. The yield is two moles of gas per mole of sodium bicarbonate. Above 36 degrees C ammonium bicarbonate decomposes into ammonia, water, and carbon dioxide, three moles of gas per mole of ammonium bicarbonate, and this reaction leaves no salt residue. From this it seems that ammonium bicarbonate has more rising power than sodium bicarbonate has. Avoidance of sodium is another advantage. These advantages of ammonium bicarbonate for baking may be outweighed by production of acrylamide, a toxin.

Question:Carbonic acid and sodium bicarbonate act as buffers in the blood. When a small amount of acid is added to this buffer, the H+ ions are used up as they combine with the bicarbonate ions. When this happens, the pH of the blood_________________________ is reversible becomes acidic doesn't change becomes basic ionizes

Answers:Doesn't change

Question:I am looking into how the pH of dichromated gelatin is affected after exposure to light in an attempt to selectively transfer acid fixing dyes to paper. I would like to raise a 10% solution of ammonium dichromate to pH 7, but I am not sure what buffer would be most effective and safe. Any insight?

Answers:(NH4)2Cr2O7 and NH4OH buffer.

Question:what happens when a large amount of a strong acid is added. H2CO3 + H2O <--> HCO3- + H3O+ A. The pH rises and the reaction moves to the left B. the pH falls and the reaction moves to the left C. the pH rises and the reaction moves to the right D. The pH falls and the reaction moves to the right

Answers:Think about the question- When a large amount of acid is added, what happens to the pH? The pH decreases (1 = very acid, 7 = neutral, and 14 = very basic). That means the answer can be B or D When a stress is put on an equilibrium reaction, the reaction shifts to relieve the stress. Adding a large amount of H3O+ to the right side of the reaction equilibrium will cause the equilibrium to shift to the left. The correct answer is B.

From Youtube

Bicarbonate extractable soil phosphorus :Step 1: Preparation of a 0.1 M acid bath Step 2: Preparation of 0.5 M sodium bicarbonate solution Step 3: Preparation of 2.5 M sulfuric acid solution Step 4: Preparation of 0.1 M ascorbic acid solution Step 5: Preparation of ammonium molybdate solution Step 6: Preparation of antimony potassium tartrate solution Step 7: Preparation of mixed reagent Step 8: Preparation of phosphate stock solution (100 mg p/L) Step 9: Preparation of working phosphate standard (5 mg P/L) Step 10: Mixing soil with sodium bicarbonate solution Step 11: Preparation of phosphorus standards and sample extract for spectrophotometer Step 12: Absorbance measurement of phosphorus standards and ample extract