Multiple Choice
Determine if SrCl₂ is acidic, basic, or neutral in an aqueous solution and explain why.
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17. Acid and Base Equilibrium
Acids Introduction
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In water, which of the following is the strongest acid?
A
B
C
D
Verified step by step guidance1
Understand that acid strength in water is often related to the ability of the acid to donate a proton (H\textsuperscript{+}) to water, forming hydronium ions (H\textsubscript{3}O\textsuperscript{+}).
Recall that for binary hydrogen halides (HX), acid strength generally increases as the bond strength between hydrogen and the halogen decreases, because weaker bonds break more easily to release H\textsuperscript{+}.
Consider the bond strengths and electronegativities of the halogens: Fluorine (F), Chlorine (Cl), Bromine (Br), and Iodine (I). Fluorine forms the strongest H-F bond, making HF a weak acid, while the bond strength decreases down the group to HI, which has the weakest H-I bond.
Recognize that the weaker H-I bond in hydroiodic acid (HI) allows it to dissociate more completely in water, making HI the strongest acid among the given options.
Summarize that acid strength in this series increases in the order HF < HCl < HBr < HI due to decreasing bond strength and increasing ease of proton donation.
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