According to the Arrhenius definitions of acids and bases, choose the acids from the list of acids and bases. Check all that apply.
HBr
[tex]$Sr ( OH )_2$[/tex]
HClO
[tex]$H _2 S$[/tex]
LiOH
Answer (2)
HBr dissociates in water to form H + ions, thus it is an Arrhenius acid.
HClO dissociates in water to form H + ions, thus it is an Arrhenius acid.
H 2 S dissociates in water to form H + ions, thus it is an Arrhenius acid.
Therefore, the Arrhenius acids are HBr, HClO, and H 2 S .
Explanation
Analyzing the Compounds Let's analyze the given compounds based on the Arrhenius definitions of acids and bases. According to Arrhenius, acids increase the concentration of H + ions in water, while bases increase the concentration of O H − ions. We will examine each compound to determine if it fits the definition of an Arrhenius acid.
Identifying Acids and Bases
HBr (Hydrobromic acid): HBr is a strong acid. When dissolved in water, it dissociates completely to form H + and B r − ions: H B rr i g h t a rro w H + + B r −
Since it increases the concentration of H + ions, it is an Arrhenius acid.
S r ( O H ) 2 (Strontium hydroxide): S r ( O H ) 2 is a strong base. When dissolved in water, it dissociates to form S r 2 + and O H − ions: S r ( O H ) 2 r i g h t a rro wS r 2 + + 2 O H −
Since it increases the concentration of O H − ions, it is an Arrhenius base, not an acid.
HClO (Hypochlorous acid): HClO is a weak acid. When dissolved in water, it dissociates partially to form H + and Cl O − ions: H ClO r i g h tl e f t ha r p oo n s H + + Cl O −
Since it increases the concentration of H + ions, it is an Arrhenius acid.
H 2 S (Hydrogen sulfide): H 2 S is a weak acid. When dissolved in water, it dissociates partially to form H + and H S − ions: H 2 S r i g h tl e f t ha r p oo n s H + + H S −
Since it increases the concentration of H + ions, it is an Arrhenius acid.
LiOH (Lithium hydroxide): LiOH is a strong base. When dissolved in water, it dissociates to form L i + and O H − ions: L i O Hr i g h t a rro w L i + + O H −
Since it increases the concentration of O H − ions, it is an Arrhenius base, not an acid.
Conclusion Based on the analysis, the Arrhenius acids from the given list are HBr, HClO, and H 2 S .
Examples
Understanding Arrhenius acids and bases is crucial in many real-world applications. For instance, in environmental science, knowing the acidity or basicity of a water source helps assess its impact on aquatic life. In medicine, understanding how different compounds affect the pH levels in the body is vital for drug development and treatment. In agriculture, the pH of the soil affects plant growth, and adjusting it with acids or bases can improve crop yields. These concepts are also fundamental in industrial processes, such as chemical synthesis and manufacturing, where controlling acidity and basicity is essential for efficient and safe operations.
The Arrhenius acids from the list provided are HBr, HClO, and H₂S. Both HBr and HClO increase H⁺ ion concentration in solution, while H₂S also acts as an acid. Sr(OH)₂ and LiOH are bases, as they increase OH⁻ ion concentration.
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