Respuesta :
Answer: The correct answer is option(A).
Explanation:
Sulfates and carbonates of barium are highly insoluble in water. but they are soluble in acids except sulfuric acid because with sulfuric acid they form barium sulfate which is a highly insoluble salt in water.
[tex]BaCl_2(aq)+Na_2CO_3(aq)\rightarrow BaCO_3(\text{white ppt})+2NaCl(aq)[/tex]
Where as barium chloride, barium nitrate and barium perchlorates are highly soluble in water.
Hence, the correct answer is option(A).
[tex]\boxed{{\text{A) BaC}}{{\text{O}}_{\text{3}}}}[/tex] is insoluble in water.
Further Explanation:
Solubility rules
These help in predicting whether the given compound is soluble or insoluble in nature. Some of the solubility rules are as follows:
1. Group 1A compounds are soluble in nature.
2. All the common compounds of ammonium ion and all acetates, chlorides, nitrates, bromides, iodides, and perchlorates are soluble in nature. But the ions whose chlorides, bromides, and iodides are not soluble are [tex]{\text{A}}{{\text{g}}^ + }[/tex], [tex]{\text{P}}{{\text{b}}^{2 + }}[/tex], [tex]{\text{C}}{{\text{u}}^ + }[/tex] and [tex]{\text{Hg}}_2^{2 + }[/tex].
3. All common fluorides, except for [tex]{\text{Pb}}{{\text{F}}_{\text{2}}}[/tex] and group 2A fluorides are soluble. Also, all sulfates except [tex]{\text{CaS}}{{\text{O}}_{\text{4}}}[/tex], [tex]{\text{SrS}}{{\text{O}}_{\text{4}}}[/tex], [tex]{\text{BaS}}{{\text{O}}_{\text{4}}}[/tex], [tex]{\text{A}}{{\text{g}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}[/tex] and [tex]{\text{PbS}}{{\text{O}}_{\text{4}}}[/tex] are soluble.
4. All common metal hydroxides except [tex]{\text{Ca}}{\left( {{\text{OH}}} \right)_{\text{2}}}[/tex], [tex]{\text{Sr}}{\left( {{\text{OH}}} \right)_{\text{2}}}[/tex], [tex]{\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}[/tex] and hydroxides of group 1A and that of transition metals are insoluble in nature.
5. All carbonates are insoluble in nature, except for sodium, potassium and ammonium.
6. Salts having ions like [tex]\text{Cl}^-[/tex], [tex]\text{Br}^-[/tex] or [tex]\text{I}^-[/tex] are generally soluble except those of [tex]\text{Ag}^+[/tex], [tex]\text{Pb}^{2+}[/tex] and [tex]{\left( {{\text{H}}{{\text{g}}_2}} \right)^{{\text{2 + }}}}[/tex].
7. Group 1A and group 2A perchlorates are soluble in nature.
8. All sulfates of metals are soluble, except for lead, mercury (I), barium, and calcium sulfates.
9. The salts having nitrate ions are soluble in nature.
According to the solubility rules, only carbonates of sodium, potassium and ammonium are soluble in nature. So barium carbonate [tex]\left( {{\text{BaC}}{{\text{O}}_{\text{3}}}} \right)[/tex] is insoluble in nature. But chlorides, nitrates and perchlorates of barium are soluble in water. Therefore option A is the correct answer.
Learn more:
- Identify the precipitate in the reaction: https://brainly.com/question/8896163
- What type of reaction occurs by mixing barium sulfide and sulfuric acid? https://brainly.com/question/5464325
Answer details:
Grade: Senior School
Chapter: Chemical reaction and equation
Subject: Chemistry
Keywords: barium, water, insoluble, solubility rules, soluble, insoluble, water, BaCO3.
