Can OH root ions coexist with Ag ions?

No, you can't

At first, silver hydroxide is formed, but because silver hydroxide is very unstable, it will decompose into silver oxide and water almost at the same time as it is formed. So we generally think that silver hydroxide cannot exist.

Upstairs mistakes, can not coexist.

Silver hydroxide precipitates are formed (after a period of time, silver hydroxide decomposes into silver oxide and water).

It can also be said that silver oxide precipitation.

No. OH ions cannot coexist with AG ions.

Silver hydroxide is generated, but because silver hydroxide is unstable, it is easy to decompose into water and silver oxide. According to the rules of ion coexistence, it is impossible to coexist.

No. Silver hydroxide precipitates are generated.

oh-+ag+=agoh (precipitation).

If there is only hydroxide and silver ions.

It doesn't coexist, because the synthesized silver hydroxide is very unstable and will decompose into silver oxide hydrate (this decomposition can occur at room temperature, just like the reaction of carbonic acid decomposition into water, so there is no silver hydroxide, and hydroxide and silver ions together will produce silver oxide hydroxide, so the two do not coexist).

But if you think about complexes.

That's different, for example, in the silver ammonia solution (diamine hydroxide combined with silver), hydroxide and silver ammonia ions can coexist, because of the silver ammonia ions

Hope it works for you.

No. The OH ion reacts with the AG ion to form silver oxide.

Yes, silver can only precipitate with CL.

It will form a silver oxide precipitate, not silver hydroxide.

Silver hydroxide precipitates are formed, but they decompose immediately because the substance is unstable.

Let's look at the OH root (which binds to these ions to form a precipitate): Mg2+, Modified Lead Al3+, Mn2+, Zn2+, Fe3+, Fe2+, Cu2+, Ca2+ (slightly soluble).

CO3 roots (combined with these ions to form precipitate): Ba2+, Ca2+, Mn2+, Zn2+, Fe3+, Cu2+, Ag+

SO4 (combined with these ions to form sedimentation and annihilation) roots: Ba2+, Ca2+ (microlytic hall).

Cl ions (combined with these ions to form precipitates): AG+

Of course, acids and alkalis cannot coexist for the most part. That is, h+ and oh- cannot coexist.

You have to remember that to see if two substances coexist is to see if there is precipitation, gas, water formation in these two reactions, and if at least one of the above three substances is formed, then they do not coexist.

Let's start with OH roots (which bind to these ions to form precipitates): Mg2+, Al3+, Mn2+, Zn2+, Fe3+, Fe2+, Cu2+, Ca2+ (slightly soluble).

CO3 roots (combined with these ions to form precipitate): Ba2+, Ca2+, Mn2+, Zn2+, Fe3+, Cu2+, Ag+

SO4 (conjugated to these ions to form a precipitate) root: Ba2+, Ca2+ (slightly soluble) Cl ions (conjugated to these ions to form a precipitate): Ag+

Of course, acids and alkalis cannot coexist for the most part. That is, H+ and OH- cannot coexist, you have to remember that to see if two substances coexist is to see if there is precipitation, gas, water formation in these two reactions, and if at least one of the above three substances is generated, then they do not coexist.

Hydrogen ions, magnesium ions, silver ions, fluoride ions, a small amount of aluminum ions, ferric ions, divalent iron ions, copper ions, ammonium ions, 、...

There's nothing that can't, it's just a matter of quantity.

It cannot coexist with acids and will produce water.

It cannot coexist with soluble copper salts, iron salts, magnesium salts, ammonium salts, etc., and will form precipitates.

Hydroxide (chemical formula: OH-) is a root with a valence of -1 valence, which can be combined with hydrogen ions (H+) to form water molecules, and ammonia and water are formed when it encounters ammonium ions (NH4+). A hydroxide root is made up of one atom each of hydrogen and oxygen, not an atom, and therefore does not have an independent relative atomic mass.

Substances that ionize anions in water that are only hydroxides are bases (such as sodium hydroxide NaOH).

Common hydroxides are ammonium hydroxide (NH4OH), barium hydroxide BA (OH) 2, calcium hydroxide CA (OH) 2, cobalt hydroxide CO(OH) 2, potassium hydroxide (KOH), gold hydroxide AU (OH) 3, lithium hydroxide (LiOH or Lioh·H2O), aluminum hydroxide AL (OH) 3, magnesium hydroxide MG (OH) 2, sodium hydroxide (NaOH), beryllium hydroxide BE(OH) 2, hydrogen hydroxide (HOH), strontium hydroxide SR (OH). 2, iron hydroxide Fe(OH)3, copper hydroxide Cu(OH)2, zinc hydroxide Zn(OH)2, ferrous hydroxide Fe(OH)2, etc.

Test: Dropwise addition of methyl orange test solution; Colorless phenolphthalein test solution (turns red after dropping); Red litmus solution (turns blue after dropping) or dip on pH test paper (the darker the concentration, the darker the color, dark blue).

Hydroxide is different from hydroxyl group.

There is an essential difference between hydroxide and hydroxyl group, (1) hydroxide is a group ion composed of h and O, hydroxyl group is a group atom composed of h and O, (2) hydroxide is always equivalent to a single ion, and hydroxyl group is sometimes equivalent to a single atom, and sometimes it can be separated, such as 2C2H5OH + 2NA=2C2H5ONA + H2

In addition to the bond of the hydrogen and oxygen atoms themselves, the hydrogen and oxygen atoms also carry an electron from the outside world, so that the two atoms in the hydroxide group reach the outermost saturation structure, so the hydroxide group can exist stably in a large number of solitary parts in the solution;

The hydroxyl group is only bonded by its own hydrogen and oxygen atoms, and it lacks an electron to reach saturation, so it must be combined with other atomic groups in the form of functional groups and cannot exist stably alone.

h+hco3-

Only sodium, potassium, and barium can be abundant in metal ions.

Anything that reacts with OH is not allowed.

1.In principle, metal ions that can form insoluble substances with hydroxide can be used. These metal hydroxides are all hydroxide complexes in nature.

Not only that, but non-electrically neutral ligands can also be formed between them, such as Fe(Oh)2+, Fe(Oh)4-, which are often dehydrated to form metaferrite ions, as is the case with aluminum and zinc.

More broadly, in concentrated solutions, such as alkali metal hydroxides, water-soluble alkaline earth metals, etc., can be regarded as metal hydroxide complexes. However, the coordination bond is weak, and the coordination bond is only significantly present in concentrated solutions.

The concept of coordination compounds is extremely broad, and most of the common inorganic compounds can be considered complexes. For example, all acid groups can be regarded as complexes of oxygen, solvated ions in aqueous solution are also complexes, and there are no truly simple free ions.

2.Typical complexes of ammonia: copper ammonia with ions, silver ammonia with ions, etc.

Again, any transition metal ion can form stable or relatively stable ammonia complexes, with the exception of the corresponding hydroxide solubility being very small.

There are six kinds of lithium (Li), sodium (Na), potassium (K), rubidium (RB), cesium (CS), and francium (FR), the first five of which exist in nature, and francium can only be produced by nuclear reactions.

After reading the first answer, I pointed out that these metals are alkali metals, and most of them can react directly with water to form hydroxide R (R stands for metal ion). Francium is a radioactive element, and reflective elements are generally not considered, but the principle is the same (elements of the same group have the same properties).

Silver ammonia solution: We often say that the silver ammonia complex ion AG(NH3)2OH (silver ammonia hydroxide), is one of them. There are also heavy metals that can form complexes with hydroxides. Such as: PB, CD, NI, etc.

On the issue of ion coexistence in solution.

The essence of the problem of ion coexistence in solution is which ions cannot react with each other. Ions that can react cannot coexist, and ions that cannot react can coexist in large quantities.

1. When some ions in the solution can react with each other to form insoluble substances and slightly soluble substances, these ions cannot coexist in large quantities.

2. When ions can combine to form difficult ionization substances, these ions cannot coexist in large quantities.

3. When ions can combine to form volatile substances (gases), these ions cannot coexist in large quantities.

4. When redox reactions can occur between ions, they cannot coexist in large quantities, so these ions cannot coexist in large quantities. Generally speaking, oxidizing ions (such as Mno4, Clo, Fe3+, NO3, etc.) and reducing ions (such as S2, I, Br, SO32, Fe2+, etc.) cannot coexist in large quantities.

Ca2+ and OH- cannot coexist in large quantities. It is mainly the soluble strong alkali Naoh, Koh, Ba(OH)2 that reacts with the soluble calcium salts CaCl2, Ca(NO3)2.

No, calcium hydroxide is slightly soluble, and the specific needs to be calculated by KSP, but the statement that a large number of coexist is false.

Calcium hydroxide is slightly soluble in water, and the concentration of calcium ions and root clearing ions is not high, and it cannot exist in large quantities.

It can react, because the solubility of calcium hydroxide is small (slightly soluble), when the concentration of sodium hydroxide and calcium chloride is large, there is calcium hydroxide precipitation.

ca2+ +2oh- = ca(oh)2

Yes, it is difficult for CA examples and OH ions to coexist.

In an alkaline solution, all weakly alkaline cations.

and H+ cannot coexist in large quantities. In middle school chemistry, the ones that cannot coexist in large quantities in alkaline solution are: H+, Fe2+, Fe3+, Cu2+, Ag+, Zn2+, Mg2+, Al3+, NH4+, HCO3-, HPO42-, H2PO4-, HSO3-, HS-, Hooc-

coo- etc.

You are talking about potassium ions (k+).

Hydroxide ion (oh-).

Chloride ions. cl-）

Carbonate ions can coexist in large quantities in alkaline solutions.

Whether the ions coexist can be judged by whether the ions are suppressed or whether they can react.

There are 3 types of ions that react with OH-:

Formation of insoluble substances (precipitate): OH- and Fe3+

fe2+mg2+

Cu + Ca2+ (calcium hydroxide.

Slightly soluble) ag+ (agoh is a white precipitate, easy to decompose into brown silver oxide.

and water) here corrects the strong alkali under calcium hydroxide

Formation of volatile substances (gases): NH4+

Formation of a substance that is difficult to ionize (e.g., spine water): H+

hco3-、hpo42-、h2po4-、hso3-、hs-、hooc-