Chemical electrolyte problems. Chemistry questions about electrolytes

They are non-electrolytes, the reason: in the high-temperature molten state, can not ionize the free-moving ions, and after dissolving in water, the original substance is changed, sulfur dioxide plus water becomes sulfurous acid, sulfur trioxide becomes sulfuric acid, so that there are free-moving hydrogen ions in the solution, ammonia is dissolved in water to form ammonia monohydrate, ionization of free-moving hydroxide, so they are not electrolytes, but non-electrolytes.

SO2SO3NH3 they are not electrolytes, although the substances they form by dissolving in water are electrolytes, they themselves are not conductive, like CO2 and the above are like this.

Neither electrolytes nor non-electrolytes are generally elemental: e.g. Cl2 or something.

I suggest you take a second look at the electrolytes in the chemistry book, because the book is a good thing, and it is always new.

1.Pair: CuSO4 ionizes out of Cu in the dissolved state

2+ and SO4

2-, so is the electrolyte, and instead of being dissolved in water, it is essentially also CuSO4 ionized out of Cu2+ and SO4

2-, which itself cannot be ionized.

2.Right: The principle is similar to the above.

It is a weak electrolyte, which ionizes a small amount of hydrogen ions and hydroxide ions; Al2O3 can ionize Al in the molten state

3+ and o2-. These are all questions about the concept of electrolytes, and as long as you closely follow the concept of electrolytes, you can understand it.

Support the first floor answer... To add, by definition, it should be one: it is a chemical compound; Second:

It dissolves in water and conducts electricity. In fact, everyone actually ignores one point, it is already a CuSO4 solution when dissolved in water, not a solution Just like SO3, it becomes an H2SO4 solution when dissolved in water!!

1.Wrong.

According to the definition of electrolyte, as long as it is a compound that can conduct electricity in water or in a molten state, it is an electrolyte, then CuSO4*5H2O meets the conditions of electrolyte. is a special class of electrolytes2. Wrong.

Although Na2O dissolves in water and becomes another electrolyte, in the molten state, Na2O is ionized, so it is an electrolyte.

3。Water is a very weak electrolyte, and its conductivity cannot be measured by ordinary instruments, but there are ionized H and OH in liquid water. Al2O3 can conduct electricity in the molten state, and it is the electrolytic molten Al2O3 that smelts the metal aluminum.

1.This is true because Cu2SO4 conducts electricity when dissolved in water, but is only a blue crystal.

2.Yes, the fundamental reason why Na2O is soluble in water and conductive is because of the formation of NaOH, 3Water can be weakly ionized to produce H+ and OH-, and Al2O3 can conduct electricity in a molten state, so it is also.

1.Wrong.

CuSO4 is a compound, its aqueous solution can conduct electricity, so it is an electrolyte, and copper sulfate crystals are also pure, and they also meet this condition, so they are all electrolytes.

2.Yes, the electrolyte must be ionized by itself, and Na2O reacts with water to form NaOH, so Na2O is not an electrolyte.

3.Water is also an electrolyte because water is a compound and its aqueous solution also conducts electricity.

Hydrochloric acid is not an electrolyte, HCL and NaCl are electrolytes, and the electrolyte must be pure, and the electrolyte that can conduct electricity in a solution or molten state is called an electrolyte.

Hello first of all, the electrolyte must be pure, hydrochloric acid and table salt are mixtures, remember that the chemical formula is generally written is pure, so HCL and NaCl are both electrolytes.

At the beginning: anode: 2cl-

2e---cl2

Cathode: 2h+

2e---h2

After reverse connection: anode: Fe-2E---Fe2+

Cathode: 2H2O+2E---H2+2OH-

fe2+2oh-==fe(oh)2

Now the energizing time is half of the original, and the electrons are half of the original.

When connected: anode: 2cl (-).

2e（-）cl2

Cathode: 2h+

2e（-）h2

Because the gas produced by the cathode is, as can be seen from the above two reaction formulas, Cl2 and H2 are equal in amount, both are. In this case, the amount of oh(-) is 1mol

After reverse connection: anode: Fe+

2e（-）2oh(-)fe(oh)2

Cathode: 2h(+)2e---h2

The gas produced should be , i.e., oh(-) produced

The anode will be consumed at the same time, so the pH value will not be affected after reverse connection.

So the concentration of oh(-) at this time is 1 10=

Therefore, the pH value is 13

Make the topic clear, one minute of energizing produces the standard condition) gas, whether it is total or one pole, start cl-, h+ discharge, time and electron number are proportional, sodium hydroxide is generated, and then the number of electrons is calculated by time, anode iron discharge, cathode h+ discharge, calculate the generation and consumption can calculate the pH.

Analysis: Stone grinding is used as the anode, iron mesh is used as the cathode, salt water is electrolyzed, and chloride ions are discharged on the anode to generate chlorine gas; Hydrogen ions are discharged on the cathode to produce hydrogen gas; Sodium hydroxide is formed in solution. The pH value at this point can be calculated by the amount and concentration of sodium hydroxide.

When the electrodes are reversed, the electrode reaction changes. Cathode - Hydrogen ions are discharged on graphite to generate hydrogen gas; Anode - the iron net is discharged by the iron itself (iron is the active material, when the active material is used as the anode, the anion is not discharged, it is the active material discharge) to generate ferrous ions. Due to the consumption of hydrogen ions ionized by water on the cathode, there will be more hydroxide ions in the solution, and ferrous ions will combine with hydroxide ions to form ferrous hydroxide.

Once you understand this, this question is not difficult to solve.

You're right! According to the definition of electrolyte: a compound that can conduct electricity in an aqueous solution or in the molten state is an electrolyte, and a metal oxide can conduct electricity in the molten state, so it is an electrolyte.

However, it cannot be disassembled when writing the ion equation, why? Because the ionic reaction we are talking about is generally in an aqueous solution, you can see the problem, right? Do you think, can metal oxides still ionize ions in aqueous solutions?

The answer is no, so it can't be dismantled!

So what kind of substances can be dismantled when writing the ionic reaction equations? Remembered:

1 Easy ionization: that is, it must be a strong electrolyte, 2 It is easily soluble in water, that is, it has a great solubility in water.

The above two conditions must be met at the same time, and one is indispensable. Use this point of view to analyze the problem of whether metal oxides can be dismantled: metal oxides are not ionized in water and have very little solubility, so whether to dismantle or not, of course, not to dismantle!

If you think the explanation is clear enough, choose the best, haha!

The ionization form of oxide is: metal oxide ionizes negative oxygen ions and metal ions, and then the negative oxygen ions combine with water to form two hydroxide ions. However, when writing the ion equation, the reaction is generally the reaction of hydroxide ions, not the reaction of negative oxygen ions (because the negative oxygen ions are too alkaline, they react with water to form hydroxide ions when they enter the solution).

The negative oxygen ions generated by direct ionization in metal oxides cannot directly react with ions, and water needs to be used as an intermediate carrier to react, and it is not that negative oxygen ions react directly with ions, so the ionization of oxides has no direct impact on the reaction of ions, so there is no need to disassemble and write.

Oxides are electrically conductive in the molten state.

However, oxides (such as manganese heptaoxide) are difficult to ionize in water and instead form acids.

It can be seen from the melting point of only 277 degrees and the molten state of non-conductivity.

HgCl2 is a covalent compound, and the crystals belong to molecular crystals.

The weak conductivity of dilute solution indicates that it is partially ionized and belongs to a weak electrolyte.

Option A First of all, elemental substances are neither electrolytes nor non-electrolytes, so C is excluded, and then BaSO4 is a strong electrolyte, but it is insoluble in water, and then ethanol is more difficult to ionize than water, so its aqueous solution does not conduct electricity.

So only a SO2 is left as a covalent compound, which is a non-electrolyte, dissolves in water to form sulfurous acid or even sulfuric acid, which is electrically conductive.

But I don't think A is correct, because the chemical bond is not broken when SO2 is dissolved in water, and if the title is changed to "And this substance is neither an electrolyte nor a non-electrolyte," then it is C.

Answer: The aqueous solution conducts electricity, the chemical bond is covalently bond break, and Cl2 is elemental, non-electrolyte.

A b is an electrolyte c is an elemental d aqueous solution cannot conduct electricity.

1.Can conduct electricity is , 2Dissolved in water to conduct electricity is 3The ones that belong to the electrolytes are the ones that belong to the non-electrolytes

The reaction occurs: Ba(OH)2 + H2SO4 = BaSO4 + 2H2O, as the reaction progresses, the ion concentration in the solution decreases, the conductivity decreases, and when the reaction is complete, the conductivity is zero, and the lamp is completely extinguished.

If you continue to drop H2SO4, the sulfuric acid solution plays a role in conduction, and at the same time as dropping H2SO4, a white precipitate is generated, if HCl solution is used instead of H2SO4, there are always conductive ions in the solution, and the bulb will not go out and will not produce precipitation.

You're talking about electrolytes.

Giving you the four most typical ions, the others are all similar.

1 Electrolytic CuSO4 solution: 2CuSO4 + 2H2O = Electrolysis = 2Cu + O2 + 2H2SO4 (only cation reduction, the same is also AgNO3 solution).

2 Electrolytic NaCl solution: 2NaCl + 2H2O = Electrolysis = 2NaOH + H2 + Cl2 (anionic oxidation only).

3 Electrolytic nano3 solution: 2H2O = Electrolysis = 2H2 + O2 (equivalent to electrolyzed water).

4 Electrolytic CuCl2 solution: CuCl2 = Electrolysis = Cu + Cl2 (both cations and anions are involved in the reaction).

As long as you remember the order of electrolysis of ions in solution, you can write the electrolysis equation.

Cationic electrolysis sequence:

Ag+>Hg2+>Fe3+>Cu2+>H+(H in acid)>Pb2+>Sn2+>Fe2+>Zn2+>H+ (H in water)>Al3+>Mg2+>Na+>Ca2+>K+

Anion electrolysis order:

s2－>i－>br－>cl－>oh－>so42－>no3－>f－

1 Electrolytic CuSO4 solution: 2CuSO4 + 2H2O = Electrolysis = 2Cu + O2 + 2H2SO4 (only cation reduction, the same is also AgNO3 solution).

2 Electrolytic NaCl solution: 2NaCl + 2H2O = Electrolysis = 2NaOH + H2 + Cl2 (anionic oxidation only).

3 Electrolytic nano3 solution: 2H2O = Electrolysis = 2H2 + O2 (equivalent to electrolyzed water).

4 Electrolytic CuCl2 solution: CuCl2 = Electrolysis = Cu + Cl2 (both cations and anions are involved in the reaction).