This is the easiest way, though not "scientifically correct":
Liters concentrated HNO3 = [ 200 L diluted HNO3 * 10 % ] / [ 68% ] = 29.4 L of the 68%
Take the calculated amount and carefully add this to 171 L of water while good mixing!
(if you take 30 L (easier measurable!) in stead, then with 170 L water you get about 200 L of 10.2% diluted acid)
This may due to Magnesium metal has high reactivity and concentration of nitric acid is dilute, thus magnesium reacts with H+ in water/ in nitric acid to give hydrogen
Nitric acid can be dilute or concentrated. This is simply a matter of how much of it you have in a given amount of a solution, which is variable.
Cu + 2HNO3 -> Cu(NO3)2 + H2 Ideally, yes. How dilute? In school experiments the nitric acid would be dilute.
By diluting the concentration of nitric acid (and the concentration of H+).
When sodium bicarbonate reacts with nitric acid, sodium nitrate salt is formed along with carbonic acid (double replacement reaction), which immediately decomposes to water and gaseous carbon dioxide (which explains the fizzing). The concentration of the nitric acid affects the rate of reaction, the more dilute it is, the slower the reaction will progress. The more pure the nitric acid, the faster the reaction will take place.
This may due to Magnesium metal has high reactivity and concentration of nitric acid is dilute, thus magnesium reacts with H+ in water/ in nitric acid to give hydrogen
Nitric acid can be dilute or concentrated. This is simply a matter of how much of it you have in a given amount of a solution, which is variable.
Cu + 2HNO3 -> Cu(NO3)2 + H2 Ideally, yes. How dilute? In school experiments the nitric acid would be dilute.
By diluting the concentration of nitric acid (and the concentration of H+).
When sodium bicarbonate reacts with nitric acid, sodium nitrate salt is formed along with carbonic acid (double replacement reaction), which immediately decomposes to water and gaseous carbon dioxide (which explains the fizzing). The concentration of the nitric acid affects the rate of reaction, the more dilute it is, the slower the reaction will progress. The more pure the nitric acid, the faster the reaction will take place.
Nitric acid is an electrolyte.
HNO3 is nitric acid. De[emdimng on its level of concentration it can vary from '0' (very concentrated ; 16M) to '3'. ) low concentration (dilute ' say 0.6 M).
confusion
Potassium hydroxide is a powerful base with a pH of 14. Dilute nitric acid is a strong acid with a pH of between 0-1 usually.
Dilute nitric and sulfuric acid fall to earth as acid rain.
zinc and copper
Yellow