In this video, Nitric acid is distilled with sulfuric acid to concentrate it. Afterwards, the concentrated Nitric acid is purified by distilling under vacuum.
Properties of nearly 100% Nitric acid are demonstrated
Isopropyl Nitrite is the Isopropanol ester of Nitrous acid. It is prepared by a solution of Isopropanol and Sulfuric acid with a solution of Sodium Nitrite
Dry Ice is added to Acetone, causing the temperature to drop to - 78,5 degrees Celsius.
Elemental Mercury has a freezing point of - 38,8 degrees Celsius.
The usual way of making Nitrous Oxide is by heating Ammonium Nitrate until decomposition. This reaction is very risky, as there is a danger of an explosion.
In this video, Nitrous Oxide is made using Sodium Nitrite and Hydroxylammonium Chloride, which is a lot safer. The reason why this is not done in industry, is because the chemicals are much more expensive.
A Nitrating solution is made by mixing Sulfuric and Nitric acid. These acids do not react, but creates an environment in which a Nitronium Ion (NO2+) can replace Hydrogen atoms. This is what happens when the Cellulose in the Cotton is nitrated.
NOTE!!
At 00:24, the KOH reduces the dichromate to a chromate, but the Chromium stays in oxidation state +6.
In this video, Potassium TetraPeroxochromate is synthesised using potassium dichromate. A tetraperoxochromate is a remarkable compound not often encountered, with Chromium being in oxidation state +5
Synthesis and properties are demonstrated
The three first alkali metals are: Lithium, Sodium and Potassium. These increase in reactivity down the periodic table.
In this video, physical and chemical properties are demonstrated.
A mixture is made of powdered Aluminum and powdered Iodine. When a drop of water is added, the oxidising properties of water is demonstrated as the rection gets hotter. When the necessary temperature is reached (which is relatively low), the Iodine and Aluminum starts reacting, giving Aluminum Iodide. Iodine smoke can be observed as well, as Iodine is in excess.
Two solutions, A and B, are made.
Solution A contains Luminol in an alkaline environment, whilst solution B contains Potassium Ferricyanide in a 0,03% Hydrogen Peroxide solution.
When the two solutions are mixed, they reacts and emit blue light
In this experiment, two solid (Ammonium Nitrate and Barium Hydroxide) are added to a beaker. As they react, Ammonia gas, water and Barium Nitrate are produced. This results in a large increase in entropy, which is the measure of randomness in a system. This again causes the temperature to drop, as there is an increase in Enthalpy
In this video, some liquid Nitrogen is placed in a small beaker, which is placed in a vacuum. The behavior of liquid Nitrogen in vacuum is demonstrated
Nitrogen Dioxide, as we know it, exists in equilibrium with many other Oxides of Nitrogen. These equilibriums are very affected by temperature, and in this video we'll see what happens when you flash freeze a sample of Nitrogen Dioxide
In this video, the classical "Barking Dog" reaction is demonstrated. In this reaction, a vessel is filled with an oxidising gas and a fuel, in this case Nitrous Oxide and Carbon Disulfide.
When ignited, the reactants decompose under strong evolution of heat. This is one of the rare examples of luminescence in the gas phase.
Silver Acetylide (also called Silver Carbide) is made by bubbling Acetylene (Ethyne) gas through an acidic solution of Silver Nitrate. Silver Acetylide precipitates, as it is not very soluble in water.
The relevant equation is as follows:
2 AgNO3(aq) + C2H2(g) ? Ag2C2(s) + 2 HNO3(aq)
The explosive properties of Silver Acetylide are also demonstrated
Aqueuous Potassium Iodide is added to 35% Hydrogen Peroxide with a detergent added. This catalyses the decomposition according to the following reaction:
H2O2 -- H2O + 1/2O2
In this video, an alloy between elemental Sodium and Potassium is made. If mixed in a proper ratio, the alloy is liquid at room- temperature.
It is extremely reactive with water, even more so than Sodium or Potassium alone.
