When a sufficient amount of CO2 is introduced into the following solutions, precipitation can be gen

A right. CO2 is introduced into water to form carbonic acid, which is more acidic than silicic acid, so it can form silicic acid, which is a precipitate that is insoluble in water.

B false. Mr. precipitates CaCO3, and since the amount of CO2 is sufficient, the precipitate continues to react to generate Ca(HCO3)2

C false. Not reacting.

D false. Not reacting.

I don't know how to ask I hope mine is helpful to you, o( o!

Choose A because in B, calcium carbonate will be mixed with carbon dioxide.

Water reacts to form calcium bicarbonate and dissolves.

CaCO3 + CO2 + H2O = Ca(HCO3)2C, the principle is the same as B, barium carbonate will also form barium bicarbonate with carbon dioxide and water.

The equation is similar to above.

Replace calcium with barium

No precipitation will be generated.

According to the principle of strong acid to weak acid, no reaction will occur.

After selecting a sufficient amount of CO2.

A produces H2SiO3 (silicic acid precipitation) B because the generated CaCO3 reacts with CO2 to form Ca(HCO3) (soluble).

So C and D that can't be selected are both because Cl- is HCL and is an acid root, so they can't react, thank you.

C was chosen because of the actual amount of CO2

Therefore, the precipitate formed by Mr. B and Mr. C will dissolve again.

aNo precipitation!

The question is about sufficient amount, so after entering B, it will precipitate into CaCo3, and then CaCo3 will also form Ca(HCO3)2 with water and CO2, which is soluble in water. In the case of A, Na2CO3 and H2SiO3 (insoluble in water) are generatedThe situation of C and D is similar to A, both of which form bicarbonate solubles, so choose A!

A sodium silicate solution is more acidic than silicic acid.

Otherwise, you cannot.

Lime water eventually produces calcium bicarbonate which can be dissolved.

CD is irregular.

b, lime water. Clarified lime water (composition is Ca(OH)2) CO2 --CaCO3 (precipitation symbol) + H2O

This is a characteristic reaction that examines CO2.

Saturated sodium carbonate.

na₂co₃+co₂+h₂o→2nahco₃↓

Barium chloride, calcium chloride, etc., but only through CO is not precipitated, and a small amount of alkali must be added, such as NH, etc.

Calcium hydroxide. Barium hydroxide, etc., but if too much is introduced, the precipitate will dissolve. So be careful when doing the questions.

Silver nitrate. etc., (Note: Silver carbonate is a yellowish precipitate.) In small amounts, it looks white. Only this one has color. Everything else is white precipitate. ）

Also, if I'm not mistaken, magnesium hydroxide can also be used to crack and co-react. Although magnesium hydroxide is also a precipitate, magnesium carbonate is more difficult to dissolve in water than magnesium hydroxide. Therefore, socks can also be reacted.

Barium hydroxide solution, closed hydrogen resistant calcium oxide solution, calcium bicarbonate solution, bicarbonate solution.

Upstairs the hydrogen car stall spring magnesium oxide is wrong. Magnesium hydroxide is inherently insoluble.

Option 12, barium chloride does not react with CO2 at all.

3. When a small amount of CO2 is generated, white precipitate is generated; In excess of CO2, CaCO3 dissolves to give sodium bicarbonate.

A small amount: CO2 + Ca(OH)2=CaCO3 (white precipitate) + H2O excess: 2CO2 + Ca(OH)2=Ca(HCO3)24, a small amount:

CO2+2Naclo+H2O=Na2CO3+2HClo excess: CO2+Naclo+H2O=NaHCO3+HCo does not precipitate at all.

First of all, the topic is not very well presented.

The first one definitely has precipitated Na2SiO3+CO2+H2O=H2SiO3 +Na2CO3

Second, weak acids cannot make strong acids, and barium carbonate precipitates are not produced.

The third is because it is an excess of carbon dioxide, so it finally generates calcium bicarbonate (high solubility), no precipitation CO2 + Ca(OH)2=CaCO3 +H2OCAco3 + CO2 + H2O=Ca(HCO3)2 The fourth is not easy to say, if it is a saturated solution of sodium hypochlorite, then CO2 + 2Naclo + H2O = Na2Co3 + 2HClona2CO3 + CO2 + H2O = 2NaHCO3 Because the solubility of sodium bicarbonate is relatively small, So it is possible to precipitate and form a precipitate.

There is a precipitate in the final solution that produces 1 precipitate as H2SiO3

Choose 11, Na2SiO3 + CO2 + H2O = H2SiO3 precipitation + Na2CO3

2. Barium chloride does not react with CO2 at all.

3. White precipitation is produced first, and then the precipitation disappears.

CO2 + Ca(OH)2 = CaCO3 (white precipitate) + H2OCAco3 + CO2 + H2O = Ca(HCO3)24, a small amount: CO2 + 2Naclo + H2O = Na2CO3 + 2HCo Excess : CO2 + NaClo + H2O = NaHCO3 + HCO no precipitation at all.

2.Barium carbonate 3 calcium carbonate.

The others don't know.

A and C are the same, and the composition is calcium hydroxide solution.

When CO2 is passed, it is precipitated in clarification, and the active ingredient in D is Ca(ClO)2, which reacts with CO2 and water to form CaCO3 and HCl. Since HCl is more acidic than H2CO3, it does not react back, so the answer is B

ACA(OH)2+CO2=CAC3 +H2OCAco3+CO2+H2O=CA(HCO3)2 precipitated and then clarified.

bbacl2

No response. So have been clarifying.

Because there is no reaction of BaCl2+CO2+H2O=BaCO3 +2HCl, weak acid cannot make strong acid. c Same as a

DCA(CLO)2+CO2+H2O=CAC3 +2HCOs, strong acid to weak acid.

CaCO3+CO2+H2O=Ca(HCO3)2 precipitates first and then clarifies.

A is not right because calcium chloride is originally a product of CO2 made from marble and hydrochloric acid, and no matter how much CO2 you use

B is not right because the Ca(OH)2 of lime water, excess CO2 will turn Ca(OH)2 into CaHCO3, this thing is not precipitation.

C is not right because, this itself does not reflect when it passes through and does not precipitate D Yes, the reason is that the generated NaHCO3 is melted in water, but because it is a saturated sodium carbonate solution, the solubility of NaHCO3 is less than that of Na2CO3, so it is precipitated

AB produces calcium bicarbonate ......Soluble in water.

d, sodium bicarbonate will be generated, which requires the participation of water, the solution is saturated, and the water needs to react, so it will become a supersaturated solution......There will definitely be precipitation.

CaCO3 precipitate will be generated when it is just passed, but CaHCO3 will be generated as soon as CO2 is more, this product is soluble in water, probably the formula is CaCO3 + CO2 + H20 CaHCO3, A, B have Ca, so they are not right, d saturated sodium carbonate Na2CO3 and C02 form slightly soluble NaHCO3, so there must be a precipitation, probably the formula is Na2CO3 + H20 + CO2 NaHCO3, no trimming, I hope it will help you.

AB can form bicarbonate, which is calcium bicarbonate, which is soluble in water.

Saturated sodium carbonate, here emphasizes the saturated sodium carbonate solution, when carbon dioxide is introduced, the concentration of carbonate in the solution increases, because of the homoionic effect, so there is sodium carbonate precipitation.

A calcium chloride and b lime water are not emphasized to be saturated solutions, when their concentration is relatively small, even if the carbon dioxide introduced reaches the saturation level, it cannot guarantee that the concentration of calcium carbonate reaches the saturation level. At the same time, we also know that the solubility of carbon dioxide is very small.

I choose AACarbon dioxide is introduced to generate carbonic acid ionization, and hydrogen ions are combined with silicates to form silicic acid, which is a white precipitate.

b.It does not react, because if the reaction is assumed, HCl will be formed, and the reaction with the precipitation C will continue to form the aluminum hydroxide precipitate.

d.In the same way b, there are chloride ions that do not react into precipitate.

e.Carbon dioxide dissolves because of the excessive production of bicarbonate is not a precipitation.

AH2SIO3 and Al(OH)3 are insoluble in carbonic acid.

Carbonic acid is weaker than hydrochloric acid, CO2 and CaCl2 solution will not react, and no precipitation is generated, so it is wrong;

Carbonic acid is stronger than silicic acid, and excess CO2 reacts with Na2SiO3 solution: 2CO2 + Na2SiO3 + 2H2O 2NaHCO3 + H2SiO3 to produce silicic acid precipitation, so it is correct;

Acidic oxides can react with alkalis, and excess CO2 reacts with Ca(OH)2: Ca(OH)2+2CO2 Ca(HCO3)2, no precipitation is generated, so it is wrong;

Excess CO2 is passed into the saturated Na2CO3 solution to react: Na2CO3 + H2O + CO2 2NaHCO3, because the solubility of sodium bicarbonate is smaller than that of sodium carbonate, so there is NaHCO3 crystal precipitation, so it is correct;

Therefore, d

I choose BBecause CO2 reacts with saturated soda ash to form NaCO3, and NaCO3 reacts with CO2 to form NaHCO3, because the solubility of NaHCO3 is relatively small, a sufficient amount of CO2 is introduced into the solution, and eventually there must be precipitation (or crystallization) precipitation.

1. Pass a sufficient amount of CO2 into the acidic solution.

HCO3- is not formed

Because HCO3- is an amphoteric substance.

It cannot be present in acidic solutions.

A reaction will occur, HCO3-+H+=CO2+H2O2, and a sufficient amount of CO2 will be introduced. Alkaline solution.

HCO3- is formed

At first, CO2 was insufficient.

Occurrence: CO2 + 2OH - = CO32 - + H2O When CO2 is exceeded: CO32 - +H2O + CO2 = 2HCO3-3, if the solution contains C6H5O-, carbonate and other weak acid groups.

As long as these acids are weaker acidic than carbonic acid.

The reaction of strong acid to weak acid will occur.

C6H5O-+CO2+H2O=C6H5OH+HCO3-Others: Sufficient CO2 is introduced into Naalo2 solution, sodium silicate solution, etc.

Let me tell you, the solution you listed, no matter how much the reaction reaches that level, will have bicarbonate! Because, there is a balance of ions! First of all, you have to understand that strong acid makes weak acid, but, you haven't seen it, weak acid makes strong acid! Hehe, in the future, if you continue to study chemistry, you will understand D

In fact, carbon dioxide has a certain solubility in these solutions, but it is relatively low, and there is a transition equilibrium between them, that is, there is the presence of bicarbonate, but the amount is very small.