Which of the following ions does not liberate hydrogen gas on reaction with dilute acids?

Question

Which of the following oxides is paramagnetic?

Answer 1

To determine which of the given ions does not liberate hydrogen gas when reacting with dilute acids, we need to consider the properties of these ions in relation to the reactivity series. The reactivity series of metals is a list that ranks metals by their reactivity, particularly with acids.

Reactivity with Dilute Acids: Metals or metal ions higher in the reactivity series than hydrogen have the ability to displace hydrogen ions from acids, thus liberating hydrogen gas. Conversely, metals lower in the reactivity series than hydrogen will not liberate hydrogen gas when reacting with dilute acids.

The question provides us with the ions ${Ti^{2+}}$, ${V^{2+}}$, ${Cr^{2+}}$, and ${Mn^{2+}}$. Let's analyze each:

${Ti^{2+}}$: Titanium is relatively reactive and above hydrogen in the reactivity series.
${V^{2+}}$: Vanadium, like titanium, is also above hydrogen in the reactivity series.
${Cr^{2+}}$: Chromium is more reactive than hydrogen and will displace hydrogen from dilute acids.
${Mn^{2+}}$: Manganese(II) ions are less reactive compared to the above elements and are characterized by being lower in the reactivity series relative to hydrogen.

Conclusion: The ion ${Mn^{2+}}$ does not liberate hydrogen when reacted with dilute acids, as manganese in the +2 oxidation state does not have sufficient reactivity compared to hydrogen. Hence, the correct answer is ${Mn^{2+}}$.

Answer 2

To determine which of the given ions does not liberate hydrogen gas when reacting with dilute acids, we need to consider the properties of these ions in relation to the reactivity series. The reactivity series of metals is a list that ranks metals by their reactivity, particularly with acids.

Reactivity with Dilute Acids: Metals or metal ions higher in the reactivity series than hydrogen have the ability to displace hydrogen ions from acids, thus liberating hydrogen gas. Conversely, metals lower in the reactivity series than hydrogen will not liberate hydrogen gas when reacting with dilute acids.

The question provides us with the ions ${Ti^{2+}}$, ${V^{2+}}$, ${Cr^{2+}}$, and ${Mn^{2+}}$. Let's analyze each:

${Ti^{2+}}$: Titanium is relatively reactive and above hydrogen in the reactivity series.
${V^{2+}}$: Vanadium, like titanium, is also above hydrogen in the reactivity series.
${Cr^{2+}}$: Chromium is more reactive than hydrogen and will displace hydrogen from dilute acids.
${Mn^{2+}}$: Manganese(II) ions are less reactive compared to the above elements and are characterized by being lower in the reactivity series relative to hydrogen.

Conclusion: The ion ${Mn^{2+}}$ does not liberate hydrogen when reacted with dilute acids, as manganese in the +2 oxidation state does not have sufficient reactivity compared to hydrogen. Hence, the correct answer is ${Mn^{2+}}$.

Which of the following ions does not liberate hydrogen gas on reaction with dilute acids?

The Correct Option is D

Solution and Explanation

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