The question asks to identify the ion common to all acids when they are dissolved in water. This relates to the definition of acids according to the Arrhenius theory and the behavior of hydrogen ions in aqueous solutions.
B) Hydrogen ion (H+), which exists as hydronium ion (H3O+). This option correctly identifies the hydrogen ion as the fundamental acidic species and explains its existence in water as the hydronium ion.
This question tests basic knowledge about the properties of acids, specifically their effect on litmus paper and their characteristic taste. Understanding these fundamental properties is crucial in chemistry.
B) Sour taste; turns blue litmus paper red. This option correctly describes both the characteristic taste of acids and their effect on blue litmus paper.
The question asks to identify which statement is NOT a characteristic property of bases. We need to recall the common properties of bases and then compare them with the given options.
Correct Option: A) Turns blue litmus paper red
This question tests the understanding of the Arrhenius definition of acids and bases. We need to recall what Arrhenius specifically stated about bases when dissolved in water.
Correct Option: C) Releases hydroxide (OH-) ions
The question asks about the gas released when a reactive metal (like zinc or magnesium) reacts with a dilute acid. This is a classic single displacement reaction where a more reactive metal displaces hydrogen from an acid.
\[ \text{Metal} + \text{Dilute Acid} \rightarrow \text{Metal Salt} + \text{Hydrogen gas} \]
\[ \text{Zn} \text{(s)} + 2\text{HCl} \text{(aq)} \rightarrow \text{ZnCl}_2 \text{(aq)} + \text{H}_2 \text{(g)} \]
Similarly, with magnesium and sulfuric acid:\[ \text{Mg} \text{(s)} + \text{H}_2\text{SO}_4 \text{(aq)} \rightarrow \text{MgSO}_4 \text{(aq)} + \text{H}_2 \text{(g)} \]
In both cases, hydrogen gas (\(\text{H}_2\)) is produced.A) Hydrogen gas is typically released when a reactive metal such as zinc or magnesium reacts with a dilute acid. This is a fundamental chemical property of acids reacting with metals more reactive than hydrogen.
To understand why aqueous solutions of acids and bases conduct electricity, we need to recall the fundamental requirements for electrical conductivity in a solution. Electrical conductivity requires the presence of mobile charge carriers. We will examine how acids and bases behave when dissolved in water to determine if they produce such carriers.
\[ HCl(aq) \rightarrow H^+(aq) + Cl^-(aq) \]
These \(H^+\) and \(Cl^-\) ions are free to move in the solution.\[ NaOH(aq) \rightarrow Na^+(aq) + OH^-(aq) \]
These \(Na^+\) and \(OH^-\) ions are free to move in the solution.Correct Option: C) Because they dissociate into free ions in water
This option correctly identifies that acids and bases, when dissolved in water, break apart into charged particles (ions) that are free to move, thereby enabling the conduction of electricity.