Problems that do not conform to the law in chemical reactions.

Whether it is a strong acid to a weak acid, or a precipitation, it is essentially the result of chemical equilibrium movement. When the two exist with each other, it is necessary to consider the combination of factors.

First of all, the production of strong acid to weak acid is relative, that is to say, this acid must be quite weak in order to drive the reaction in the direction of forming weak acid. In an aqueous system, there is no – at least not very significant – difference in acidity between sulphuric acid and hydrochloric acid, so this approach is not feasible.

Of course, there is a possible way for concentrated sulfuric acid and silver chloride to react at a very high temperature, so that the reaction is possible, and the principle is that the so-called high boiling point acid makes low boiling point acid, which is similar. In fact, all acid-base reactions involving carbonic acid and carbon dioxide are essentially like this.

Therefore, as far as this special reaction is concerned, because there is no difference between sulfuric acid and hydrochloric acid under water conditions, it is not suitable for strong acids to make weak acids.

Of course, a more appropriate example could be the reaction of silver phosphate and sulfuric acid. Phosphoric acid is a weak acid, and the boiling point is high, so does silver phosphate react with sulfuric acid or not? These are two factors, one is the insoluble nature of silver phosphate, and the other is that phosphoric acid itself is a weak acid.

In this case, the reaction equation can only be written, and the thermodynamic calculation under different conditions can be used to determine whether the reaction proceeds or not.

a The mass of the candle becomes smaller after combustion, because the oxygen participating in the reaction is not included in the total mass of the substances participating in the reaction, and the carbon dioxide produced escapes and is not included in the total mass of the product. A Isn't it the conservation of mass?

AGCL is not tolerated with acid-base salts, which is a special case and the general law does not apply.

The KSP of silver chloride is much smaller than that of silver sulfate, so there is no way to convert silver chloride into silver sulfate during the reaction.

Phenomenon: 1. The reaction between aluminum sheet and hydrochloric acid is exothermic, and the reaction of Ba(OH)2 with NH4Cl is endothermic; 2. Na reacts with H2O (phenolphthalein), melts, floats on the water surface, rotates, and gas is released; (melting, floating, swimming, hissing, red) 3. Flame color reaction: na yellow, k purple (through blue cobalt glass), cu green, ca brick red, na + yellow), k + purple).

4. Cu filament is burned in Cl2 to produce brown smoke; 5, H2 burns in Cl2 and is a pale flame; 6. Na burns in Cl2 to produce a large amount of white smoke; 7. P burns in Cl2 to produce a large amount of white smoke; 8. SO2 is introduced into the magenta solution to fade first, and then return to the original color after heating; 9. NH3 meets HCl to produce a large amount of white smoke; 10. The aluminum foil burns violently in oxygen to produce dazzling white light; 11. Magnesium strips are burned in the air to produce dazzling white light, and white powder (MGO) is burned in CO2, producing black smoke; 12. Iron wire burns in Cl2, producing brown smoke; 13. HF corrosive glass: 4HF + SI2 SIF4 + 2H2 O 14. Fe(OH)2 is oxidized in the air: from white to gray-green and finally to reddish-brown; 15. At room temperature:

Fe, Al passivated in concentrated H2SO4 and concentrated HNO3; 16. Inject FeCl3 solution into the test tube containing phenol solution, and the solution is purple; Phenol is pink when exposed to air. 17. The protein turns yellow when it is concentrated with Hno 3, and it has the smell of burnt feathers when it is burned; 18. Burning in the air: S - faint light blue flame H2 - light blue flame H2 S - light blue flame CO - blue flame Ch 4 - bright and blue flame S burning in O 2 - bright blue-purple flame.

19 Characteristic reaction phenomena: 20 Light yellow solid: S or Na2O2 or AGBR 21 Gases that fade magenta solutions:

SO2 (red again after heating), Cl2 (no red color after heating) 22 Colored solution: Fe2+ (light green), Fe3+ (yellow), Cu2+ (blue), MnO4 - violet) Colored solids: red (Cu, Cu2O, Fe2O3), reddish-brown [Fe(OH)3] black (Cuo, Feo, Fes, Cus, AG2S, PBS) Blue [Cu(OH)2] Yellow (AG3PO4) White [Fe(0h) 2, CaCo3, BaSO4, AGCL, Baso3] Non-ferrous gases:

Cl2 (yellow-green), NO2 (reddish-brown).

Is there a pattern to chemical reactions? : Regular redox reaction between strong oxidizing substances and strong reducing substances to form weak oxidizing substances and weakly reducing substances.

1. According to the second law of thermodynamics, any isothermal isobaric closed system tends to reduce Gibbs free energy. In the absence of the influence of an external force, the same is true for any reaction mixture. 2. The essence of a chemical reaction is the process of breaking old chemical bonds and forming new chemical bonds.

3. The process of chemical reaction is the process of recombining the atoms of various substances (reactants) participating in the reaction to form other substances. In a chemical reaction, the type of atoms does not change before and after the reaction, the number does not increase or decrease, and the mass of the atoms does not change. 4. In chemical reactions, it is often accompanied by luminescence, heating, discoloration, and the formation of precipitates.

The basis for determining whether a reaction is chemical is whether the reaction produces a new substance.

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