What is an electrolyte in chemistry. Refers to electrolytes. What particles carry charges?

These are substances whose solutions or melts conduct electric current. They are also an indispensable component of liquids and dense tissues of organisms.

Electrolytes include acids, bases and salts. Substances that do not conduct electric current in a dissolved or molten state are called nonelectrolytes. These include many organic substances, such as sugars, alcohols, etc. The ability of electrolyte solutions to conduct electric current is explained by the fact that when dissolved, electrolyte molecules disintegrate into electrically positively and negatively charged particles - ions. The amount of charge on an ion is numerically equal to the valence of the atom or group of atoms that form the ion. Ions differ from atoms and molecules not only in the presence of electrical charges, but also in other properties, for example, chlorine ions have no odor, color, or other properties of chlorine molecules.

Positively charged ions are called cations, negatively charged ions are called anions. Cations form hydrogen atoms H +, metals: K +, Na +, Ca 2+, Fe 3+ and some groups of atoms, for example the ammonium group NH + 4; Anions form atoms and groups of atoms that are acidic residues, for example Cl -, NO - 3, SO 2- 4, CO 2- 3.

The term E. was introduced into science by Faraday. Until very recently, K. E. included typical salts, acids and alkalis, as well as water. Studies of non-aqueous solutions, as well as studies at very high temperatures, have greatly expanded this field. I. A. Kablukov, Kadi, Karara, P. I. Walden and others showed that not only aqueous and alcohol solutions conduct current noticeably, but also solutions in a number of other substances, such as, for example, liquid ammonia, liquid sulfur dioxide anhydride, etc. It has also been found that many substances and mixtures are excellent insulators at ordinary temperatures, such as anhydrous metal oxides (calcium oxide, magnesium oxide, etc.), and become electrolytic conductors when the temperature increases. The famous Nernst incandescent lamp, the principle of which was discovered by the brilliant Yablochkov, provides an excellent illustration of these facts. A mixture of oxides - an “incandescent body” in a Nernst lamp, which is not conductive at ordinary temperatures, becomes excellent at 700° and, moreover, retains a solid state electrolytic conductor. It can be assumed that most complex substances studied in inorganic chemistry, with appropriate solvents or at a sufficiently high temperature, can acquire the properties of electrons, with the exception, of course, of metals and their alloys and those complex substances for which metallic conductivity has been proven. At the moment, indications of the metallic conductivity of molten silver iodide, etc. should be considered not yet sufficiently substantiated. Something else must be said about most substances containing carbon, i.e., those studied in organic chemistry. It is unlikely that there will be solvents that will make hydrocarbons or their mixtures (paraffin, kerosene, gasoline, etc.) conductors of current. However, in organic chemistry we have a gradual transition from typical electrolytes to typical non-electrolytes: starting from organic acids to phenols containing a nitro group, to phenols not containing such a group, to alcohols, aqueous solutions of which belong to insulators with low electrical exciting forces and , finally, to hydrocarbons - typical insulators. For many organic, and also partly some inorganic compounds, it is difficult to expect that an increase in temperature will make them E., since these substances decompose earlier from the action of heat.

The question of what electrolyte was was in such an uncertain state until the theory of electrolytic dissociation was brought in to solve it.

Electrolytic dissociation.

The disintegration of electrolyte molecules into ions is called electrolytic dissociation, or ionization, and is a reversible process, i.e., an equilibrium state can occur in a solution in which as many electrolyte molecules disintegrate into ions, so many of them are formed again from ions.

The dissociation of electrolytes into ions can be represented by the general equation: , where KmAn is an undissociated molecule, K z+ 1 is a cation carrying z 1 positive charges, And z- 2 is an anion having z 2 negative charges, m and n are the number of cations and anions , formed during the dissociation of one electrolyte molecule. For example, .
The number of positive and negative ions in a solution may be different, but the total charge of the cations is always equal to the total charge of the anions, so the solution as a whole is electrically neutral.
Strong electrolytes almost completely dissociate into ions at any concentration in solution. These include strong acids (see), strong bases and almost all salts (see). Weak electrolytes, which include weak acids and bases and some salts, such as sublimate HgCl 2, dissociate only partially; the degree of their dissociation, i.e., the proportion of molecules disintegrated into ions, increases with decreasing solution concentration.
A measure of the ability of electrolytes to disintegrate into ions in solutions can be the electrolytic dissociation constant (ionization constant), equal to
where the concentrations of the corresponding particles in the solution are shown in square brackets.

1. ELECTROLYTES

1.1. Electrolytic dissociation. Degree of dissociation. Electrolyte Power

According to the theory of electrolytic dissociation, salts, acids, hydroxides, dissolving in water, completely or partially disintegrate into independent particles - ions.

The process of decomposition of substance molecules into ions under the influence of polar solvent molecules is called electrolytic dissociation. Substances that dissociate into ions in solutions are called electrolytes. As a result, the solution acquires the ability to conduct electric current, because mobile electric charge carriers appear in it. According to this theory, when dissolved in water, electrolytes break up (dissociate) into positively and negatively charged ions. Positively charged ions are called cations; these include, for example, hydrogen and metal ions. Negatively charged ions are called anions; These include ions of acidic residues and hydroxide ions.

To quantitatively characterize the dissociation process, the concept of the degree of dissociation was introduced. The degree of dissociation of an electrolyte (α) is the ratio of the number of its molecules disintegrated into ions in a given solution ( n ), to the total number of its molecules in solution ( N), or

α = .

The degree of electrolytic dissociation is usually expressed either in fractions of a unit or as a percentage.

Electrolytes with a degree of dissociation greater than 0.3 (30%) are usually called strong, with a degree of dissociation from 0.03 (3%) to 0.3 (30%) - medium, less than 0.03 (3%) - weak electrolytes. So, for a 0.1 M solution CH3COOH α = 0.013 (or 1.3%). Therefore, acetic acid is a weak electrolyte. The degree of dissociation shows what part of the dissolved molecules of a substance has broken down into ions. The degree of electrolytic dissociation of an electrolyte in aqueous solutions depends on the nature of the electrolyte, its concentration and temperature.

By their nature, electrolytes can be divided into two large groups: strong and weak. Strong electrolytes dissociate almost completely (α = 1).

Strong electrolytes include:

1) acids (H 2 SO 4, HCl, HNO 3, HBr, HI, HClO 4, H M nO 4);

2) bases – metal hydroxides of the first group of the main subgroup (alkali) – LiOH, NaOH, KOH, RbOH, CsOH , as well as hydroxides of alkaline earth metals – Ba (OH) 2, Ca (OH) 2, Sr (OH) 2;.

3) salts soluble in water (see solubility table).

Weak electrolytes dissociate into ions to a very small extent; in solutions they are found mainly in an undissociated state (in molecular form). For weak electrolytes, an equilibrium is established between undissociated molecules and ions.

Weak electrolytes include:

1) inorganic acids ( H 2 CO 3, H 2 S, HNO 2, H 2 SO 3, HCN, H 3 PO 4, H 2 SiO 3, HCNS, HClO, etc.);

2) water (H 2 O);

3) ammonium hydroxide ( NH 4 OH);

4) most organic acids

(for example, acetic CH 3 COOH, formic HCOOH);

5) insoluble and slightly soluble salts and hydroxides of some metals (see solubility table).

Process electrolytic dissociation depicted using chemical equations. For example, dissociation of hydrochloric acid (HC l ) is written as follows:

HCl → H + + Cl – .

Bases dissociate to form metal cations and hydroxide ions. For example, the dissociation of KOH

KOH → K + + OH – .

Polybasic acids, as well as bases of polyvalent metals, dissociate stepwise. For example,

H 2 CO 3 H + + HCO 3 – ,

HCO 3 – H + + CO 3 2– .

The first equilibrium - dissociation according to the first step - is characterized by the constant

.

For second stage dissociation:

.

In the case of carbonic acid, the dissociation constants have the following values: K I = 4.3× 10 –7, K II = 5.6 × 10–11. For stepwise dissociation always K I> K II > K III >... , because the energy that must be expended to separate an ion is minimal when it is separated from a neutral molecule.

Average (normal) salts, soluble in water, dissociate to form positively charged metal ions and negatively charged ions of the acid residue

Ca(NO 3) 2 → Ca 2+ + 2NO 3 –

Al 2 (SO 4) 3 → 2Al 3+ +3SO 4 2–.

Acid salts (hydrosalts) are electrolytes containing hydrogen in the anion, which can be split off in the form of the hydrogen ion H +. Acid salts are considered as a product obtained from polybasic acids in which not all hydrogen atoms are replaced by a metal. Dissociation of acid salts occurs in stages, for example:

KHCO 3 → K + + HCO 3 – (first stage)

Electrolytes are substances whose melts or solutions conduct electric current. Electrolytes include acids, bases, and most salts.

Electrolyte dissociation

Electrolytes include substances with ionic or highly polar covalent bonds. The former exist in the form of ions even before they are transferred to a dissolved or molten state. Electrolytes include salts, bases, and acids.

Rice. 1. Table the difference between electrolytes and non-electrolytes.

There are strong and weak electrolytes. Strong electrolytes, when dissolved in water, completely dissociate into ions. These include: almost all soluble salts, many inorganic acids (for example, H 2 SO 4, HNO 3, HCl), hydroxides of alkali and alkaline earth metals. Weak electrolytes, when dissolved in water, slightly dissociate into ions. These include almost all organic acids, some inorganic acids (for example, H 2 CO 3), many hydroxides (except for hydroxides of alkali and alkaline earth metals).

Rice. 2. Table of strong and weak electrolytes.

Water is also a weak electrolyte.

Like other chemical reactions, electrolytic dissociation in solutions is written in the form of dissociation equations. At the same time, for strong electrolytes the process is considered to be irreversible, and for electrolytes of medium strength and weak – as a reversible process.

Acids– these are electrolytes, the dissociation of which in aqueous solutions occurs with the formation of hydrogen ions as cations. Polybasic acids dissociate stepwise. Each subsequent step proceeds with greater and greater difficulty, since the resulting ions of acidic residues are weaker electrolytes.

Grounds– electrolytes that dissociate in an aqueous solution to form the hydroxide ion OH- as an anion. The formation of hydroxide ion is a common feature of bases and determines the general properties of strong bases: alkaline character, bitter taste, soapiness to the touch, reaction to an indicator, neutralization of acids, etc.

Alkalis, even slightly soluble ones (for example, barium hydroxide Ba(OH) 2) dissociate completely, example:

Ba(OH) 2 =Ba 2 +2OH-

Salts are electrolytes that dissociate in an aqueous solution to form a metal cation and an acid residue. Salts do not dissociate stepwise, but completely:

Сa(NO 3) 2 =Ca 2 + +2NO 3 –

Electrolytic dissociation theory

Electrolytes– substances that undergo electrolytic dissociation in solutions or melts and conduct electric current due to the movement of ions.

Electrolytic dissociation is the breakdown of electrolytes into ions when dissolved in water.

The theory of electrolytic dissociation (S. Arrhenius, 1887) in the modern understanding includes the following provisions:

• When dissolved in water, electrolytes break down (dissociate) into ions - positive (cations) and negative (anions). Ionization occurs most easily for compounds with ionic bonds (salts, alkalis), which, when dissolved (endothermic process of destruction of the crystal lattice), form hydrated ions.

Rice. 3. Scheme of electrolytic dissociation of salt.

Ion hydration is an exothermic process. The ratio of energy costs and gains determines the possibility of ionization in a solution. When a substance with a polar covalent bond (for example, hydrogen chloride HCl) is dissolved, the water dipoles are oriented at the corresponding poles of the dissolved molecule, polarizing the bond and turning it into an ionic one, followed by hydration of the ions. This process is reversible and can occur either completely or partially.

• hydrated ions are stable and move randomly in solution. Under the influence of an electric current, the movement becomes directional: cations move towards the negative belt (cathode), and anions move towards the positive belt (anode).
• dissociation (ionization) is a reversible process. The completeness of ionization depends on the nature of the electrolyte (alkali salts dissociate almost completely), its concentration (with increasing concentration, ionization becomes more difficult), temperature (increasing temperature promotes dissociation), and the nature of the solvent (ionization occurs only in a polar solvent, in particular, water).

Electrolytes are solutions containing a high concentration of ions that allow the passage of electric current. As a rule, these are aqueous solutions of salts, acids and alkalis.

In the human and animal body, electrolytes play an important role: for example, blood electrolytes with iron ions transport oxygen to tissues; electrolytes with potassium and sodium ions regulate the body’s water-salt balance, intestinal and heart function.

Properties

Pure water, anhydrous salts, acids, and alkalis do not conduct current. In solutions, substances disintegrate into ions and conduct current. This is why electrolytes are called second-order conductors (as opposed to metals). Electrolytes can also be melts and some crystals, in particular zirconium dioxide and silver iodide.

The main property of electrolytes is the ability for electrolytic dissociation, that is, the disintegration of molecules when interacting with molecules of water (or other solvents) into charged ions.

Based on the type of ions formed in the solution, the electrolyte is distinguished as alkaline (electrical conductivity is due to metal ions and OH-), saline and acidic (with H+ ions and acid base residues).

To quantitatively characterize the ability of an electrolyte to dissociate, the “degree of dissociation” parameter was introduced. This value reflects the percentage of molecules that have undergone decay. It depends on:
the substance itself;
solvent;
substance concentration;
temperature.

Electrolytes are divided into strong and weak. The better the reagent dissolves (breaks down into ions), the stronger the electrolyte, the better it conducts current. Strong electrolytes include alkalis, strong acids and soluble salts.

For electrolytes used in batteries, a parameter such as density is very important. The operating conditions of the battery, its capacity and service life depend on it. Density is determined using hydrometers.

Precautions when working with electrolytes

The most popular electrolytes are a solution of concentrated sulfuric acid and alkali - most often potassium, sodium, and lithium hydroxides. All of them cause chemical burns to the skin and mucous membranes, and very dangerous burns to the eyes. That is why all work with such electrolytes must be done in a separate, well-ventilated room, using protective equipment: clothing, masks, goggles, rubber gloves.
A first aid kit with a set of neutralizing agents and a water tap should be kept near the room where work with electrolytes is carried out.
Acid burns are neutralized with a solution of soda (1 tsp per 1 cup of water).
Alkali burns are neutralized with a solution of boric acid (1 tsp per 1 cup of water).
To wash the eyes, neutralizing solutions should be twice as weak.
Damaged skin areas are first washed with a neutralizer, and then with soap and water.
If the electrolyte is spilled, it is collected with sawdust, then washed with a neutralizer and wiped dry.

When working with electrolyte, you should all safety requirements. For example, acid is poured into water (and not vice versa!) not manually, but with the help of devices. Pieces of solid alkali are lowered into water not with your hands, but with tongs or spoons. You cannot work in the same room with batteries with different types of electrolytes, and storing them together is also prohibited.

Some jobs require “boiling” the electrolyte. This releases hydrogen, a flammable and explosive gas. In such premises, explosion-proof electrical wiring and electrical appliances must be used, smoking and any work with open flames is prohibited.

Store electrolytes in plastic containers. Glass, ceramic, porcelain dishes and tools are suitable for work.

In the next article we will tell you more about the types and uses of electrolyte.

Electrolytes as chemical substances have been known since ancient times. However, they have conquered most areas of their application relatively recently. We will discuss the industry's highest priority areas for using these substances and figure out what the latter are and how they differ from each other. But let's start with an excursion into history.

Story

The oldest known electrolytes are salts and acids, discovered in the Ancient world. However, ideas about the structure and properties of electrolytes have evolved over time. Theories of these processes have evolved since the 1880s, when a number of discoveries were made related to theories of the properties of electrolytes. Several qualitative leaps were observed in theories describing the mechanisms of interaction of electrolytes with water (after all, only in solution do they acquire the properties due to which they are used in industry).

Now we will examine in detail several theories that had the greatest influence on the development of ideas about electrolytes and their properties. And let's start with the most common and simple theory, which each of us went through in school.

Arrhenius theory of electrolytic dissociation

In 1887, the Swedish chemist and Wilhelm Ostwald created the theory of electrolytic dissociation. However, it’s not that simple here either. Arrhenius himself was a proponent of the so-called physical theory of solutions, which did not take into account the interaction of the constituents of a substance with water and argued that free charged particles (ions) exist in the solution. By the way, it is from this position that electrolytic dissociation is considered in school today.

Let's talk about what this theory provides and how it explains to us the mechanism of interaction of substances with water. Like any other, she has several postulates that she uses:

1. When interacting with water, the substance breaks down into ions (positive - cation and negative - anion). These particles undergo hydration: they attract water molecules, which, by the way, are charged positively on one side and negatively on the other (forming a dipole), as a result they are formed into aqua complexes (solvates).

2. The dissociation process is reversible - that is, if a substance has broken up into ions, then under the influence of any factors it can again turn into its original form.

3. If you connect electrodes to the solution and turn on the current, the cations will begin to move to the negative electrode - the cathode, and the anions to the positively charged one - the anode. That is why substances that are highly soluble in water conduct electric current better than water itself. For the same reason they were called electrolytes.

4. electrolyte characterizes the percentage of a substance that has undergone dissolution. This indicator depends on the properties of the solvent and the dissolved substance itself, on the concentration of the latter and on the external temperature.

Here, in fact, are all the main postulates of this simple theory. We will use them in this article to describe what happens in an electrolyte solution. We will look at examples of these connections a little later, but now let’s look at another theory.

Lewis theory of acids and bases

According to the theory of electrolytic dissociation, an acid is a substance in the solution of which a hydrogen cation is present, and a base is a compound that disintegrates in solution into a hydroxide anion. There is another theory, named after the famous chemist Gilbert Lewis. It allows us to somewhat expand the concept of acid and base. According to Lewis's theory, acids are molecules of a substance that have free electron orbitals and are capable of accepting an electron from another molecule. It is easy to guess that the bases will be particles that are capable of donating one or more of their electrons to the “use” of the acid. What is very interesting here is that not only an electrolyte, but also any substance, even insoluble in water, can be an acid or base.

Brendsted-Lowry protolytic theory

In 1923, independently of each other, two scientists - J. Brønsted and T. Lowry - proposed a theory that is now actively used by scientists to describe chemical processes. The essence of this theory is that the meaning of dissociation comes down to the transfer of a proton from an acid to a base. Thus, the latter is understood here as a proton acceptor. Then the acid is their donor. The theory also explains well the existence of substances that exhibit the properties of both acids and bases. Such compounds are called amphoteric. In the Bronsted-Lowry theory, the term ampholytes is also used for them, while acids or bases are usually called protolytes.

We come to the next part of the article. Here we will tell you how strong and weak electrolytes differ from each other and discuss the influence of external factors on their properties. And then we will begin to describe their practical application.

Strong and weak electrolytes

Each substance interacts with water individually. Some dissolve well in it (for example, table salt), while others do not dissolve at all (for example, chalk). Thus, all substances are divided into strong and weak electrolytes. The latter are substances that interact poorly with water and settle at the bottom of the solution. This means that they have a very low degree of dissociation and high bond energy, which does not allow the molecule to disintegrate into its constituent ions under normal conditions. Dissociation of weak electrolytes occurs either very slowly or with increasing temperature and concentration of this substance in solution.

Let's talk about strong electrolytes. These include all soluble salts, as well as strong acids and alkalis. They easily disintegrate into ions and are very difficult to collect into precipitation. Current in electrolytes, by the way, is carried out precisely thanks to the ions contained in the solution. Therefore, strong electrolytes conduct current best. Examples of the latter: strong acids, alkalis, soluble salts.

Factors influencing the behavior of electrolytes

Now let's figure out how changes in the external environment affect Concentration directly affects the degree of dissociation of the electrolyte. Moreover, this relationship can be expressed mathematically. The law describing this relationship is called Ostwald's dilution law and is written as follows: a = (K / c) 1/2. Here a is the degree of dissociation (taken in fractions), K is the dissociation constant, different for each substance, and c is the concentration of the electrolyte in the solution. Using this formula, you can learn a lot about a substance and its behavior in solution.

But we have deviated from the topic. In addition to concentration, the degree of dissociation is also affected by the temperature of the electrolyte. For most substances, increasing it increases solubility and chemical activity. This is precisely what can explain the occurrence of some reactions only at elevated temperatures. Under normal conditions, they go either very slowly or in both directions (this process is called reversible).

We have analyzed the factors that determine the behavior of a system such as an electrolyte solution. Now let's move on to the practical application of these, without a doubt, very important chemicals.

Industrial use

Of course, everyone has heard the word “electrolyte” in relation to batteries. The car uses lead-acid batteries, the electrolyte in which is 40% sulfuric acid. To understand why this substance is needed there at all, it is worth understanding the operating features of batteries.

So what is the principle of operation of any battery? They undergo a reversible reaction of converting one substance into another, as a result of which electrons are released. When charging a battery, an interaction of substances occurs that does not occur under normal conditions. This can be thought of as the accumulation of electricity in a substance as a result of a chemical reaction. During the discharge, the reverse transformation begins, leading the system to the initial state. These two processes together constitute one charge-discharge cycle.

Let's look at the above process using a specific example - a lead-acid battery. As you might guess, this current source consists of an element containing lead (as well as lead dioxide PbO 2) and acid. Any battery consists of electrodes and the space between them filled with electrolyte. As the latter, as we have already found out, in our example we use sulfuric acid with a concentration of 40 percent. The cathode of such a battery is made of lead dioxide, and the anode consists of pure lead. All this is because different reversible reactions take place at these two electrodes with the participation of ions into which the acid has dissociated:

1. PbO 2 + SO 4 2- + 4H + + 2e - = PbSO 4 + 2H 2 O (reaction occurring at the negative electrode - cathode).
2. Pb + SO 4 2- - 2e - = PbSO 4 (Reaction occurring at the positive electrode - anode).

If we read the reactions from left to right, we get processes that occur when the battery is discharged, and if from right to left, we get processes that occur when the battery is charged. In each of these reactions, these reactions are different, but the mechanism of their occurrence is generally described in the same way: two processes occur, in one of which electrons are “absorbed”, and in the other, on the contrary, they “leave out”. The most important thing is that the number of electrons absorbed is equal to the number of electrons released.

Actually, besides batteries, there are many applications for these substances. In general, the electrolytes, examples of which we have given, are only a grain of the variety of substances that are united under this term. They surround us everywhere, everywhere. Here, for example, is the human body. Do you think these substances are not there? You are very mistaken. They are found everywhere in us, and the largest amount is made up of blood electrolytes. These include, for example, iron ions, which are part of hemoglobin and help transport oxygen to the tissues of our body. Blood electrolytes also play a key role in regulating water-salt balance and heart function. This function is performed by potassium and sodium ions (there is even a process that occurs in cells called the potassium-sodium pump).

Any substances that you can dissolve even a little are electrolytes. And there is no branch of industry or our life where they are not used. It's not just car batteries and batteries. These are any chemical and food production, military factories, clothing factories, and so on.

The composition of the electrolyte, by the way, varies. Thus, acidic and alkaline electrolytes can be distinguished. They are fundamentally different in their properties: as we have already said, acids are proton donors, and alkalis are acceptors. But over time, the composition of the electrolyte changes due to the loss of part of the substance; the concentration either decreases or increases (it all depends on what is lost, water or electrolyte).

We come across them every day, but few people know exactly the definition of such a term as electrolytes. We've looked at examples of specific substances, so let's move on to slightly more complex concepts.

Physical properties of electrolytes

Now about physics. The most important thing to understand when studying this topic is how current is transmitted in electrolytes. Ions play a decisive role in this. These charged particles can transfer charge from one part of the solution to another. Thus, anions always tend to the positive electrode, and cations - to the negative. Thus, by acting on the solution with electric current, we separate the charges on different sides of the system.

A very interesting physical characteristic is density. Many properties of the compounds we are discussing depend on it. And the question often comes up: “How to increase the density of the electrolyte?” In fact, the answer is simple: it is necessary to reduce the water content in the solution. Since the density of the electrolyte is largely determined, it largely depends on the concentration of the latter. There are two ways to achieve your plan. The first is quite simple: boil the electrolyte contained in the battery. To do this, you need to charge it so that the temperature inside rises to just above one hundred degrees Celsius. If this method does not help, do not worry, there is another one: simply replace the old electrolyte with a new one. To do this, you need to drain the old solution, clean the insides from residual sulfuric acid with distilled water, and then fill in a new portion. As a rule, high-quality electrolyte solutions immediately have the desired concentration. After replacement, you can forget for a long time about how to increase the density of the electrolyte.

The composition of the electrolyte largely determines its properties. Characteristics such as electrical conductivity and density, for example, strongly depend on the nature of the solute and its concentration. There is a separate question about how much electrolyte a battery can contain. In fact, its volume is directly related to the declared power of the product. The more sulfuric acid inside the battery, the more powerful it is, i.e., the more voltage it can produce.

Where will this be useful?

If you are a car enthusiast or just interested in cars, then you yourself understand everything. Surely you even know how to determine how much electrolyte is in the battery now. And if you are far from cars, then knowledge of the properties of these substances, their use and how they interact with each other will not be superfluous. Knowing this, you will not be confused if you are asked to tell what electrolyte is in the battery. Although, even if you are not a car enthusiast, but you have a car, then knowledge of the battery structure will not be superfluous and will help you with repairs. It will be much easier and cheaper to do everything yourself than to go to an auto center.

And in order to better study this topic, we recommend reading a chemistry textbook for school and universities. If you know this science well and have read enough textbooks, the best option would be “Chemical Current Sources” by Varypaev. The entire theory of operation of batteries, various batteries and hydrogen cells is outlined there in detail.

Conclusion

We've come to the end. Let's summarize. Above we have discussed everything related to such a concept as electrolytes: examples, theory of structure and properties, functions and applications. Once again, it is worth saying that these compounds form part of our life, without which our bodies and all areas of industry could not exist. Do you remember about blood electrolytes? Thanks to them we live. What about our cars? With this knowledge, we can fix any problem related to the battery, since we now understand how to increase the density of the electrolyte in it.

It’s impossible to tell everything, and we didn’t set such a goal. After all, this is not all that can be told about these amazing substances.