Chapter 12: Problem 13
BaSO \(_{4}\) would be product of the reaction of what acid and what base?
Short Answer
Expert verified
BaSO₄ is formed by the reaction of sulfuric acid (H₂SO₄) with barium hydroxide (Ba(OH)₂).
Step by step solution
01
Identify the Compound
The given compound is barium sulfate, represented as BaSO\(_{4}\). This is a salt which is typically formed by the reaction of an acid with a base.
02
Identify the Anion in the Salt
Barium sulfate (BaSO\(_{4}\)) contains the sulfate anion (SO\(_4^{2-}\)). Sulfate is derived from sulfuric acid (H\(_2\)SO\(_4\)). This means the acid used in the reaction could be sulfuric acid.
03
Identify the Cation in the Salt
BaSO\(_{4}\) contains the barium cation (Ba\(^{2+}\)). Barium ions (Ba\(^{2+}\)) typically come from barium compounds such as barium hydroxide (Ba(OH)\(_2\)) a common example of a base.
04
Write the Reaction Equation
The reaction involves sulfuric acid (H\(_2\)SO\(_4\)) and barium hydroxide (Ba(OH)\(_2\)). The balanced chemical equation for the reaction is:\[Ba(OH)_2 + H_2SO_4 \rightarrow BaSO_4 + 2H_2O\]This reaction forms barium sulfate (BaSO\(_4\)) and water (H\(_2\)O).
05
Confirm the Reaction Type
This is a typical acid-base neutralization reaction where an acid reacts with a base to form a salt and water. Here, sulfuric acid reacts with barium hydroxide to form barium sulfate and water.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Barium Sulfate Formation
Barium sulfate, represented by the chemical formula \( \text{BaSO}_4 \), is a white, crystalline compound commonly used in various industries, including in medical imaging as a contrast agent. It is formed through a chemical reaction between an acid and a base. This product is classified as a salt, specifically due to its formation from the interaction of a sulfate ion with barium ions. The process typically involves the combination of a sulfate anion \( \text{(SO}_4^{2-}) \) and a barium cation \( \text{(Ba}^{2+}) \).
These reactants combine to form the insoluble barium sulfate compound. This reaction is often utilized in chemistry for making barium sulfate precipitates, which are easy to separate from the solution due to their insolubility. Understanding the formation of barium sulfate is crucial for recognizing how certain salts are produced through acid-base reactions.
These reactants combine to form the insoluble barium sulfate compound. This reaction is often utilized in chemistry for making barium sulfate precipitates, which are easy to separate from the solution due to their insolubility. Understanding the formation of barium sulfate is crucial for recognizing how certain salts are produced through acid-base reactions.
Sulfuric Acid
Sulfuric acid, known by its chemical formula \( \text{H}_2\text{SO}_4 \), is a strong mineral acid composed of two hydrogen atoms, one sulfur atom, and four oxygen atoms. It is a highly corrosive and dense liquid that plays a vital role in a variety of chemical processes.
In the context of forming barium sulfate, sulfuric acid provides the sulfate component of the salt. When sulfuric acid dissociates in water, it releases two protons \(\text{H}^{+}\) and forms the sulfate ion \( \text{SO}_4^{2-} \). These sulfate ions can then react with suitable metal cations, such as barium ions, to form sulfates.
The versatility and reactivity of sulfuric acid make it a significant acid in both industrial and laboratory environments, where it is used in the manufacture of fertilizers, charge batteries, and in the synthesis of other chemicals.
In the context of forming barium sulfate, sulfuric acid provides the sulfate component of the salt. When sulfuric acid dissociates in water, it releases two protons \(\text{H}^{+}\) and forms the sulfate ion \( \text{SO}_4^{2-} \). These sulfate ions can then react with suitable metal cations, such as barium ions, to form sulfates.
The versatility and reactivity of sulfuric acid make it a significant acid in both industrial and laboratory environments, where it is used in the manufacture of fertilizers, charge batteries, and in the synthesis of other chemicals.
Barium Hydroxide
Barium hydroxide, with the chemical formula \( \text{Ba(OH)}_2 \), is a strong base commonly used in chemical reactions. It contains barium ions \( \text{(Ba}^{2+}) \) and hydroxide ions \( \text{(OH}^{-}) \). This compound is typically found in its octahydrate form, meaning it has eight water molecules attached (\( \text{Ba(OH)}_2 \cdot 8\text{H}_2\text{O} \)).
When barium hydroxide dissolves in water, it dissociates completely to release barium cations and hydroxide anions. The free barium ions can then react with sulfate ions from sulfuric acid to form barium sulfate. This quality of barium hydroxide makes it an ideal candidate for reactions requiring strong basicity.
Barium hydroxide is used in laboratories for titration reactions due to its strong basic properties and in various industrial processes such as the manufacture of glass and ceramics.
When barium hydroxide dissolves in water, it dissociates completely to release barium cations and hydroxide anions. The free barium ions can then react with sulfate ions from sulfuric acid to form barium sulfate. This quality of barium hydroxide makes it an ideal candidate for reactions requiring strong basicity.
Barium hydroxide is used in laboratories for titration reactions due to its strong basic properties and in various industrial processes such as the manufacture of glass and ceramics.
Neutralization Reaction
A neutralization reaction is a chemical process where an acid and a base react together to form a salt and usually water. This type of reaction is exemplified by the combination of sulfuric acid and barium hydroxide to form barium sulfate and water.
The reaction can be expressed by the balanced equation: \[\text{Ba(OH)}_2 + \text{H}_2\text{SO}_4 \rightarrow \text{BaSO}_4 + 2\text{H}_2\text{O}\] During this process, sulfuric acid donates hydrogen ions \(\text{H}^{+}\), while barium hydroxide provides hydroxide ions \(\text{OH}^{-}\). These ions combine to form water, which results in the cancellation of the acidic and basic properties, hence the term neutralization.
This reaction is significant in many chemical applications, including titrations used to determine unknown concentrations. Understanding neutralization helps in recognizing the balance of equations and the formation of non-toxic products from potentially hazardous reactants.
The reaction can be expressed by the balanced equation: \[\text{Ba(OH)}_2 + \text{H}_2\text{SO}_4 \rightarrow \text{BaSO}_4 + 2\text{H}_2\text{O}\] During this process, sulfuric acid donates hydrogen ions \(\text{H}^{+}\), while barium hydroxide provides hydroxide ions \(\text{OH}^{-}\). These ions combine to form water, which results in the cancellation of the acidic and basic properties, hence the term neutralization.
This reaction is significant in many chemical applications, including titrations used to determine unknown concentrations. Understanding neutralization helps in recognizing the balance of equations and the formation of non-toxic products from potentially hazardous reactants.
