Chemistry, 03.07.2019 22:00 xojade

What kind of reaction occurs when you mix aqueous solutions of barium sulfide and sulfuric acid? what kind of reaction occurs when you mix aqueous solutions of barium sulfide and sulfuric acid? neutralization gas evolution precipitation precipitation and gas evolution?

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Answer from: blackwhiteroses383

The reactions that occur by mixing aqueous solutions of barium sulfide and sulfuric acid are

$\boxed{{\text{Precipitation and gas evolution reactions}}}$

Further Explanation:

Precipitation reaction:

It is the type of reaction in which an insoluble salt is formed by the combination of two solutions containing soluble salts. That insoluble salt is known as precipitate and therefore such reactions are named precipitation reactions. An example of precipitation reaction is,

${\text{AgN}}{{\text{O}}_3}\left( {aq}\right)+{\text{KBr}}\left( {aq}\right)\to {\text{AgBr}}\left( s \right)+{\text{KN}}{{\text{O}}_3}\left( {aq}\right)$

Here, AgBr is a precipitate.

Neutralization reaction:

It is the reaction that occurs between an acid and a base in order to form salt and water. It is named so as it neutralizes the excess amount of hydrogen or hydroxide ions present in the solution. It is used to decrease the acidity in the stomach, wastewater treatment, antacid tablets and to control the pH of soil. An example of neutralization reaction is,

${\text{HCl}}+{\text{NaOH}}\to{\text{NaCl}}+{{\text{H}}_2}{\text{O}}$

Gas evolution reaction:

It is the type of chemical reaction in which one of the products is a gas. These reactions are often carried out in a fume chamber if poisonous gases are produced. An example of gas evolution reaction is,

${\text{Zn}}+2{\text{HCl}}\to{\text{ZnC}}{{\text{l}}_2}+{{\text{H}}_2}$

Here, ${{\text{H}}_2}$ is evolved so it is a gas evolution reaction.

The solubility rules to determine the solubility of the compound are as follows:

1. The common compounds of group 1A are soluble.

2. All the common compounds of ammonium ion and all acetates, chlorides, nitrates, bromides, iodides, and perchlorates are soluble in nature. Only the chlorides, bromides, and iodides of ${\text{A}}{{\text{g}}^ + }$ , ${\text{P}}{{\text{b}}^{2 + }}$ , ${\text{C}}{{\text{u}}^ + }$ and ${\text{Hg}}_2^{2 + }$ are not soluble.

3. All common fluorides, except for ${\text{Pb}}{{\text{F}}_{\text{2}}}$ and group 2A fluorides, are soluble. Moreover, sulfates except ${\text{CaS}}{{\text{O}}_{\text{4}}}$ , ${\text{SrS}}{{\text{O}}_{\text{4}}}$ , ${\text{BaS}}{{\text{O}}_{\text{4}}}$ , ${\text{A}}{{\text{g}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}$ and ${\text{PbS}}{{\text{O}}_{\text{4}}}$ are soluble.

4. All common metal hydroxides except ${\text{Ca}}{\left( {{\text{OH}}}\right)_{\text{2}}}$ , ${\text{Sr}}{\left( {{\text{OH}}} \right)_{\text{2}}}$ , ${\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}$ and hydroxides of group 1A, are insoluble.

5. All carbonates and phosphates, except those formed by group 1A and ammonium ion, are insoluble.

6. All sulfides, except those formed by group 1A, 2A, and ammonium ion are insoluble.

7. Salts that contain ${\text{C}}{{\text{l}}^ - }$ , ${\text{B}}{{\text{r}}^ - }$ or ${{\text{I}}^ - }$ are usually soluble except for the halide salts of ${\text{A}}{{\text{g}}^ + }$ , ${\text{P}}{{\text{b}}^{2 + }}$ and ${\left({{\text{H}}{{\text{g}}_2}}\right)^{{\text{2 + }}}}$ .

8. The chlorides, bromides, and iodides of all the metals are soluble in water, except for silver, lead, and mercury (II). Mercury (II) iodide is water insoluble. Lead halides are soluble in hot water.

9. The perchlorates of group 1A and group 2A are soluble in nature.

10. Almost all the sulfides of transition metals are highly insoluble. These include CdS, FeS, ZnS, and ${\text{A}}{{\text{g}}_2}{\text{S}}$ . The sulfides of arsenic, antimony, bismuth, and lead are also insoluble.

11. All the acetates and chlorates are soluble in nature.

The reaction between barium sulfide and sulfuric acid is as follows:

${\text{BaS}}\left({aq} \right)+{{\text{H}}_2}{\text{S}}{{\text{O}}_4}\left( {aq}\right) \to {\text{BaS}}{{\text{O}}_4}\left( s \right)+{{\text{H}}_2}{\text{S}}\left( g \right)$

According to the solubility rules, ${\text{BaS}}{{\text{O}}_4}$ is an insoluble salt. So ${\text{BaS}}{{\text{O}}_4}$ will form precipitate in the above reaction and therefore this is a precipitation reaction.

Also, ${{\text{H}}_2}{\text{S}}$ is evolved during this reaction, so it is also a gas evolution reaction.

Learn more:

1. Balanced chemical equation

2. The main purpose of conducting experiments:

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: precipitate, soluble, insoluble, solubility rules, solubility, precipitation reaction, BaSO4, H2S, BaS, H2SO4, neutralization reaction, gas evolution reaction.

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