How to solve the problem of ion coexistence in junior high school chemistry fast and convenient ?

Select d na+, no3-, CO3(2-), cl-a, h+, no3-, ag+, cl-

Cannot coexist because AG+ and CL- produce AGClb,H+,Cl-,CO3(2-),Na+

It cannot coexist because H+ binds to CO3(2-) as unstable H2CO3, which readily decomposes into CO2

C,Na+,Cl-,SO4(2-),Ba2+ cannot coexist because SO4(2-) and Ba2+ form BaSO4 precipitate.

I don't understand hi

To see whether ions can coexist is to see if they can form gas precipitated water. Each option requires 4 ions to generate 16 substances. It's a must.

As long as there is gas and water precipitation, it means that it cannot coexist. According to this, it can be seen that AG+ and Cl- in A form AGCL precipitation, and H+ and CO32- in B, generate H2CO3It's unstable.

It is immediately decomposed into CO2 and water at the same time as it is generated. C Ba2+ and SO42- generate BaSO4 precipitates. So only d can.

A, Ag+, Cl- will combine to form a precipitate.

B,,H+,CO3(2-), which will form gas CO2C, SO4(2-), and Ba2+ will form precipitate.

d, do not react.

a. Silver ions and chloride ions form silver chloride precipitates.

Hydrogen ions and carbonate ions in b produce carbon dioxide and water.

In c, barium ions and sulfate ions produce barium sulfate precipitation.

Select and cl- to generate agcl

H+ and CO3(2-) produce H2O and CO2

SO4(2-) and BA2+ to form BASO4

Needless to say, the Ag+ ions in A will be oxidized in strong acids, so only D Na+ can exist in acids.

1) Read the solubility table after reading the book and remember the insoluble or slightly soluble substances. If two ions produce these things, they can't coexist. For example, calcium ions and carbonate ions.

2) If gas is generated, it cannot coexist. The most typical liquid spring in junior high school should be hydrogen ions, carbonate, and sulfite.

3) Produce water. For example, hydrogen ions and hydroxides.

4) If it is said in the stem that the solution is colorless, then the colored ions cannot exist. For example, copper ions, iron ions.

In other words, this should be all there is to junior high school, metathesis is still relatively simple redox reaction and the like, that is, oxidizing ions and reducing ions cannot coexist; In addition, there is a double hydrolysis or something (because it should not be rough is the content of junior high school.、So don't talk about it.、If you're interested, you can search for it yourself)., 2, there is a table at the back of the book, which talks about what ions and what ions together produce precipitates, gases.

Just put up with that back stool.

There is also a mantra that potassium, sodium, and nitric acid are soluble or something, give you a **, and it is more specific over there.

For chemistry at the junior high level, just look at whether water, gas, or solids are formed in the product. If there is, it cannot coexist; If not, they can coexist. Personal insights, I hope it will be useful to you. ,0,ions cannot coexist,0,

1 Under acidic conditions: no hydroxide. There can be no gas that can coexist with hydrogen ions. Swift Fight.

2. The ions that cannot exist under acidic conditions are: weak acid ions and weak acid acid root ions. Reason: strong acid to weak acid. Thiosulfate ions, silver ammonia ions.

3. Some ions can exist alone under acidic conditions, but they cannot coexist under the influence of other ions, because nitrate has strong oxidation and can oxidize ferric.

The above can not coexist in an acidic environment, and the rest can coexist in an acidic environment as long as it produces precipitation, gas and electrolyte in a weak ear with ions in an acidic environment, and no redox reaction can occur.