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ionization of nitric acid in water

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Question:a. Nitric Acid b. Ethanoic Acid c. ammonia d. magnesium hydroxide

Answers:a. Nitric Acid HNO3 (aq) H+ (aq) + NO3- (aq) b. Ethanoic Acid C2H4O2 (aq) H+ (aq) + C2H3O2- (aq) c. ammonia NH3 (aq) + H2O NH4+ (aq) + OH- (aq) d. magnesium hydroxide Mg(OH)2 (s) Mg++ (aq) + 2 OH- (aq)

Question:A) nitric acid B) cesium hydroxide

Answers:A) HNO3 <---> H^+ + NO3^- (you could also write: HNO3 + H2O <---> H3O^+ + NO3^- this is done because there are actually no free H^+ in aqueous solution, they always combine with one or more water molecules to form hydronium (H3O^+) or other composite ions) B) CsOH <---> Cs^+ + OH^- the <---> arrows should better be written als two half arrows indicating the reversibility of the reactions

Question:I've got 25% how do I concentrate it to a higher concentration?

Answers:If you distill the nitric acid solution, it will form an azeotrope with water. The concentrated nitric acid of commerce consists of the maximum boiling azeotrope of nitric acid and water. Technical grades are normally 68% HNO3, (approx 15 molar). This occurs when the boiling temperature is 120.5 C. Beware!!!, This is extremely dangerous and must only be attempted in properly equiped laboratories, with proper safety equipment in use. It is definitely not something that you should try to do at home.

Question:Doing a lab for AP Chem and this question has stumped me. We were finding out how to determine the mass of silver in an alloy and this is during the filtration process. Sorry if it is too vague but help would be great!

Answers:hmmm Since ur NItric acid in water will be dilute, and Silver chloride is insoluble in many solutions...maybe u should use a more concentrated NItric acid, if u want to dissolve the chloride. Have u checked into the solubility of Silver Chloride in Acidic solutions?

From Youtube

Oxidizing Property Of Nitric Acid :You can Analysis the Nitric Acid And the Property of Nitric Acid when oxidize .First add Nitric Acid to a test tube. .Followed by some highly purity copper or coper wire. .Brown NO2 can be clearly seen. .When water is add blue copper ll Nitrate is form.

Nitric Acid Synthesis :IMPORTANT: I do not recommend anyone repeat this lab, it was one of the more dangerous ones I have done and will ever do, and only recommend you attempt it if you are outside or in a fume hood and have copious amounts of water and sodium carbonate on hand. ALSO IMPORTANT: I made a critical mistake in this lab. When letting the glassware cool it is necessary to remove the rubber tube from the sodium carbonate solution. If you do not the cooling of the gases will causer some of the solution to be pulled into the apparatus and into the nitric acid, ruining the nitric acid and producing large quantities of nitrogen dioxide. I came close to doing this and almost lost my nitric acid. I did not show this important step, and what you did not see in this video was disassembling the apparatus, which proved to be rather difficult. Always be safe!