Is metaaluminic acid a precipitate??? Is aluminum oxalate a precipitate

Metaaluminic acid is also aluminum hydroxide, so it is weakly reduced.

The answer to this can be found on page 545 of the second volume of the textbook "Inorganic Chemistry", which says: "Al(OH)3 is slightly more basic than acidic.

Metaaluminic acid is a weak acid, an acid that is weaker than carbonic acid, because it can react with strong acid, strong acid has strong oxidation, so metaaluminic acid is reducing, and metaaluminic acid can ionize hydrogen ions, so metaaluminic acid is a weak acid".

Cannot react with CO2. But if it's a metaaluminate solution, it's fine. Because metaaluminic acid is less acidic than carbonic acid, it is equivalent to the replacement of weak acid by strong acid, (taking sodium metaaluminate as an example) to generate sodium carbonate and aluminum hydroxide precipitation, and if CO2 is excessive, sodium bicarbonate and aluminum hydroxide precipitation will be generated.

Metaaluminate can be the addition of excess hydrogen ions to generate trivalent aluminum ions ALO2- +4H+ =Al3+ +2H2OALO2- +H+ +H2O==Al(OH)3 Al(OH)3+3H+==Al3+ +3H20AL(OH)3 can be regarded as a single weak acid or a ternary weak base, for the following reasons: Al(OH)3 + 3H =AL+ 3H2OAL(OH)3 + OH =ALO2 + 2H2O, so it can be regarded as a ternary weak base and acid reaction, Monobasic weak acid reacts with base.

Note: The reason why it is said weak is because it is all weakly ionized. The compound is an amphoteric compound.

No, whoever he encounters is combined with water, and there is no problem of precipitation or non-precipitation.

Metaaluminic acid is halo2, which is generally combined with water in water. Written as Al(OH)3, it is a substance of both sexes, acidic and alkaline.

When the amount of metaaluminium is sufficient, it will form a heavy weight in the case of insufficient acidity

Be! Halo2 can be seen as al(oh)3 removing a portion of water.

In fact, the acid ionization of aluminum hydroxide is the ionization of metaaluminic acid.

Metaaluminic acid does not exist, it can only combine with water to form aluminic acid, which is Al(OH)3

Metaaluminic acid H3alo3 substance, I usually use Al(OH)3 instead and Al(OH)3 is an absolute white precipitate.

There is absolutely no such thing as metaaluminic acid, aluminum is obviously alkaline in an acidic environment, and only aluminum ions are possible!

Only metaaluminate, such as sodium metaaluminate. There is no metaaluminic acid.

Absolutely! It can be said to be aluminum hydroxide.

Metaaluminic acid is a weak acid, not a precipitate, it exists in water in the form of Al(OH)3. Metaaluminic acid can also be regarded as a product of aluminum hydroxide dehydration.

True sodium metaaluminate does not exist.

Sodium metaaluminate itself should be sodium tetrahydroxyaluminate.

And we generally think of metaaluminic acid as the product of aluminum hydroxide dehydration.

Aluminum hydroxide itself is a precipitation.

Therefore, metaaluminic acid is generally regarded as a precipitation!

Aluminum oxalate itself is not a precipitate, but aluminum oxalate will form a precipitate, aluminum oxalate will be completely dissolved in a high concentration of phosphoric acid aqueous solution, and at a lower concentration, it will form an aluminium phosphate precipitate.

Aluminum oxalate hydrate, molecular formula C6Al2O12·XH2O, CAS number.

814-87-9, which is slightly harmful to water, do not allow undiluted or large quantities of products to come into contact with groundwater, waterways or sewage systems, and do not discharge materials into the surrounding hail cracking environment without ** permission.

Physical properties of several rounds of wanton speculation:

Properties: white powder.

Solubility. Soluble in inorganic acids, insoluble in water and ethanol.

Properties and stability: stable at room temperature and pressure, avoiding oxide moisture contact.

Storage: Keep the container tightly sealed and store in a cool, dry place in Lachang.

The above content refers to the encyclopedia - aluminum oxalate.

Aluminium carbonate does not precipitate. Because it's too late to crystalline. with soluble aluminum salts andCarbonatesreaction, instantaneously produces aluminium carbonate, but instantaneously hydrolyzes into itAluminum hydroxide

So it can not exist in aqueous solution, 3CO32- +2Al+ +6H2O=2Al(OH)3 +3CO2 +3H2O, but in industry it can be passed by alumina andCarbon dioxideSynthesized under specific conditions.

Where is the width of aluminum carbonate?

Mix aluminum fluoride with sodium carbonate.

Mixing, melting at high temperature, can be prepared. The by-product is cryolite.

Equation: 4ALF3 + 3NA2CO3 = Gao Shen blind code temperature = 2NA3 [ALF6] + AL2 (CO3) 3 Pay attention to control the temperature and prevent the decomposition of aluminum carbonate.

When the aluminium carbonate is precipitated from the mixture in solid form, it is filtered to obtain a relatively pure aluminium carbonate. This process is strictly waterproof to prevent hydrolysis of aluminum carbonate.

The above content refers to Encyclopedia - Aluminum Carbonate.

Summary. Al3+ begins to precipitate at pH, precipitates completely at pH, and then converts aluminum hydroxide to metaaluminate as pH increases.

Al3+ begins to precipitate at pH, precipitates completely at pH, and then converts aluminum hydroxide to metaaluminate as pH increases.

Kiss, between pH = 5 and 9, can be precipitated completely.

The L-H2O series -PH diagram shows that the stable Li of alumina in the hydrogen section exists in the range, and theoretically the pH value can be controlled within this range. As shown in the figure below, it is basically left and right.

No. There is a small amount of aluminium carbonate in aluminum hydroxide, which reacts with soluble aluminium salts and carbonates to form aluminium carbonate instantaneously, but it is hydrolyzed into aluminium hydroxide instantaneously.

Aluminum carbonate hydrolysis: 2Al+3Co3HO=2Al(OH)3Co

Immediately after the formation, the aluminium carbonate reacts with water to form aluminium hydroxide, Al(OH) and carbon dioxide Co.

This is because the chemical bond (oxygen bond) between aluminum, carbon, and oxygen in the resulting aluminium carbonate is too weak and weaker than silver hydroxide, so it is immediately hydrolyzed in contact with water to form aluminum hydroxide Al(OH) and carbon dioxide CO. Equation AL (CO3) +3H O= 2AL(OH) 3CO

When aluminum ions encounter carbonate ions in solution, they will be double hydrolyzed to form aluminum hydroxide and carbon dioxide, so aluminum carbonate cannot be obtained in solution.

The hydrolysis of iron carbonate and copper carbonate is similar to that of aluminium carbonate, while magnesium carbonate needs to be heated and hydrolyzed.

Question 1: Is aluminum sulfate a precipitation? When dissolved in water, it is colloidal, has metastability, and will coalesce and sink when the ionization equilibrium is disrupted.

Question 2: Can aluminum sulfate be compared with sodium hydroxide Sodium hydroxide: At first, precipitated aluminum hydroxide is generated, and then sodium hydroxide is excessive, and the precipitate dissolves and disappears, becoming sodium metaaluminate.

Ammonia: Because it is a weak alkali, even if it is excessive, it can only produce aluminum hydroxide, and the precipitation cannot disappear.

Question 3: Which is the precipitate of aluminum sulfate, alumina or iron oxide Alumina and iron oxide are both solid and insoluble in water.

Question 4: Why does the reaction and precipitation of aluminum sulfate and excess ammonia not disappear Because ammonia is a weak alkali, it can only be partially hydrolyzed to achieve equilibrium, and the large amount does not make the balance move. The resulting OH and Al ions can only form a precipitate and cannot dissolve the resulting Al(OH)3.

Just like a drop of NaOH is a strong alkali in Huaisen, and a bottle of ammonia is still a weak alkali, because NaOH is a strong electrolyte that is completely ionized, while ammonia is a weak electrolyte that can only be partially hydrolyzed.

Question 5: To make all the aluminum ions in the aluminum sulfate solution precipitate clearly, the appropriate reagent is to choose B, first of all, aluminum sulfate is a strong acid and weak alkali salt, hydrolysis is acidic, so first of all, exclude a and D two options, because they will not react, and secondly, sodium hydroxide is a strong base, after adding it, he can react with aluminum sulfate to form aluminum hydroxide precipitate, but if more sodium hydroxide is added, then the generated aluminum hydroxide will react with sodium hydroxide to form sodium metaaluminate.

The selection of ammonia does not have the above problems, because ammonia is a weak alkali, even if it is added too much, it will not react with the aluminum hydroxide generated by the reaction.

Hope it helps, thank you.

Question 6: Add the following reagents dropwise to the aluminum sulfate solution, and the precipitation will not disappear due to the excessive addition of reagentsH2 A drops the NaOH solution into the aluminum sulfate solution drop by drop until it is excessive, and the white precipitate of aluminum hydroxide will continue to react with sodium hydroxide and the precipitate disappears, so A is wrong; b Add NH3?

H2O is dropped into the aluminum sulfate solution drop by drop, until it is excessive, and the aluminum hydroxide becomes a white precipitate, because the aluminum hydroxide only reacts with a strong alkali and will not dissolve with NH3?H2O solution, so the precipitate does not disappear, so B is correct; c Aluminum sulfate does not react with NaCl and does not precipitate, so C is wrong; d Aluminum sulfate does not react with magnesium chloride, and no precipitation is generated, so D is wrong, so B is selected

Aluminum sulfate is a white crystal, soluble in water, insoluble in ethanol, etc.

The first major use of aluminum sulfate is used in papermaking, and the second largest use is as a flocculant in drinking water, industrial water and industrial wastewater treatment. When aluminium sulfate is added to this type of water, colloidal aluminium hydroxide flakes that can adsorb impurities and other suspended solids can be generated, which can be used in the treatment of lead drinking water to control the color of water.

The industrial products are gray-white flakes, granularities or blocks, which are light green because of the low iron salt belt, and the surface is yellow due to the oxidation of the low-cost iron salt. The crude product is grayish-white fine-grained structure porous stool.