Reaction of metal and acid base, reaction of alkali with metal

Na can react with either an acid solution (whether concentrated or dilute) or an alkaline solution. As long as there is water, which is a solution system, NA can react. Because of the metallic nature of na.

Very strong and can directly grab hydrogen from the water.

Mg can react with acids, and concentrated acids do not passivate. Does not react with alkalis. It can react with water under heated conditions.

Al can react with oleic acid and base, passivate in case of concentrated acid, and heat to break the passivation. Al can also react slowly (very slowly) with water when heated.

FE reacts with oleic acid, does not react with alkali, passivates when encountering concentrated acid, and is broken by heating. Fe can also be combined with water vapor under harsh conditions.

React. Cu with dilute sulfuric acid.

Does not react with concentrated sulfuric acid at room temperature.

It also does not react (this is either passivation, or does not react), and heating can react. However, Cu can react with concentrated dilute nitric acid without heating. Cu does not react with alkalis.

Oxidants such as concentrated HNO3, concentrated H2SO4, HCO3, K2Cr2O7, and KMno4 are responsible for passivation.

The metals that can be passivated are, CR (chromium), Ni (nickel), CO (cobalt), MO (molybdenum), Al (aluminum), TA (tantalum), NB (niobium) and W (tungsten), among which the most passivated metals are CR (chromium), MO (molybdenum), Al (aluminum), Ni (nickel), Fe (iron).

Again, passivation is the formation of a thin oxide layer on the surface of the metal, which makes the metal react rate.

Greatly reduced process, strictly speaking, is not unresponsive. However, a dense oxide film on the surface prevents the reaction from proceeding further.

Concentrated hydrochloric acid, dilute nitric acid: with sodium, magnesium, aluminum, iron, copper are violently dissolved;

Dilute hydrochloric acid, dilute sulfuric acid, dilute sodium hydroxide, concentrated sodium hydroxide: violently dissolved with sodium, magnesium and aluminum; Slow dissolution reaction with iron and copper;

Concentrated sulfuric acid: almost can not dissolve and react with any metal, and the metal surface is passivated; However, it can undergo a sharp oxidation reaction with active metals such as sodium and magnesium;

Concentrated nitric acid: It can have a sharp dissolution reaction with active metals such as sodium and magnesium; Aluminum is passivated in concentrated nitric acid and does not dissolve; Iron and copper both dissolve slowly.

Metals and oleic acids basically react, and concentrated acids will be passivated (because concentrated acids have strong oxidizing properties, the metal surface will form an oxide film, preventing the reaction), and only active metals and amphoteric metals (aluminum, zinc, etc.) can react with lye.

Reaction of metals with dilute hydrochloric acid and dilute sulfuric acid.

Alkali can react with metal, but this metal must be amphoteric metal, alkali is generally a strong alkali and is an active metal that can replace the relatively inactive metal in the alkali. Metals generally can not react with alkali (except for amphoteric metals), reason: alkali can be ionized as OH- and metal ions in water, first of all, the metal has to undergo a chemical reaction, and the valency can only be increased, and the oxygen element in oh-is negative divalent, and the hydrogenin is positive monovalent is very stable, so it is difficult to have a chemical reaction.

There will be no metal replacement reaction, because the zero-valent state of metal elements in alkalis that can be dissolved in water is very active, and metals that are more active than them are soluble in alkalis (solutions), and there will be no intermetal-to-metal displacement reactions, but direct reaction with water to generate hydrogen and alkali, so it cannot react with alkalis. (Amphoteric metals refer to metals that can react with both acids and bases, such as aluminum, and alkalis react with water and OH- (in bases) to produce hydrogen and metaaluminate ions.)

We refer to the metal that preceded copper as a reactive metal.

Therefore, magnesium, zinc, iron, and aluminum are all reactive metals.

Then each metal reacts with dilute hydrochloric acid and dilute sulfuric acid respectively.

Magnesium with dilute sulfuric acid and dilute hydrochloric acid:

The metal dissolves quickly and a large amount of gas is released to produce a large amount of heat.

Zinc with dilute sulfuric acid and dilute hydrochloric acid:

The metal dissolves quickly and releases gases.

Iron with dilute sulphuric acid and dilute hydrochloric acid:

The metal gradually dissolves to produce a small amount of gas, and the solution changes from colorless to light green.

Aluminum with dilute sulfuric acid and dilute hydrochloric acid:

Metals dissolve slowly Air bubbles are produced on the surface of metals.

The phenomenon is basically the same, but because the metal activity is different, the reaction rate is not the same, so there are some differences.

After reacting with the acid solution, the solution becomes colorless metals, including magnesium, zinc, and aluminum.

When the iron and acid solution is reacted, the solution turns light green.

Later you will learn that light green is actually a positive 2-valent iron ion, also called ferrous ion.

The metal reacts with the acid to produce hydrogen gas and may produce a soluble solution of metal ions, as well as salts of some acids.

The reaction of a metal and an acid refers to the displacement of an acid with a metal. Not all metals react with acid ruler states.

Only the metal that is in front of hydrogen in the order of metal activity reacts with the acid. Elemental metal + acid --salt + hydrogen (displacement reaction), elemental metal + salt (solution) - another metal + another salt, metal oxide charcoal or hydrogen metal carbon dioxide or water.

When you put a piece of iron or zinc into the acid, they react very quickly: it is heat-released, it is bubbling, and then the metal slowly disappears. This often leads people to think that all metals can react with acids.

Actually, not all of them are like that. Some metals react with one acid, but not with another; And every acid doesn't necessarily react with every metal.