Arrange the following substances in order from weakest to strongest acid: HClO3, HOI, HBrO2, HClO2, HIO2.

Question

BlackTom AI · Accepted Answer

Question restatement: Arrange the following substances in order from weakest to strongest acid: HOI, HIO2, HBrO2, HClO2, HClO3.

First, consider the general rules for oxoacids of halogens: adding more oxygen atoms (increasing oxidation state of the central halogen) tends to increase acidity because the conjugate base is stabilized by delocalizing negative charge over more O atoms. Also, for a given oxidation state, a more electronegative central atom (e.g., Cl vs Br vs I) stabilizes the conjugate base better through inductive effects, generally increasing acidity.

Option breakdown and reasoning:
- HOI (hypoiodous acid): Iodine is less electronegative and has the lowest oxidation state among the listed species, and it also has the fewest oxygens. This tends to make HOI the weakest acid in this set, since the conjugate base IO− is less stabilized.
- HIO2 (iodosoic acid): This adds an extra oxygen compared to HOI, raising the oxidation state of iodine. The presence of an additional oxo group increases acidity relative to HOI because the conjugate base (IO2−) is better stabilized by resonance with more oxygens.
- HBrO2 (bromous acid): Bromine is more electronegative than iodine, and HBrO2 has the same oxidation state (+3) as HIO2 but with a more electronegative center. This generally makes HBrO2 a stronger acid than HIO2 due to greater stabilization of the conjugate base via inductive effect from Br.
- HClO2 (chlorous acid): Chlorine is more electronegative than bromine, and HClO2 has Cl in the +3 oxidation state with two oxygens. Compared to HBrO2, the higher electronegativity of Cl tends to stabilize the conjugate base better, making HClO2 stronger than HBrO2.
- HClO3 (chloric acid): This has chlorine in the +5 oxidation state with three oxygens, which markedly increases acidity. It typically represents the strongest acid among the listed oxoacids due to both higher oxidation state and substantial resonance stabilization in the conjugate base.

Putting it together, the weakest to strongest order is:
HOI < HIO2 < HBrO2 < HClO2 < HClO3

Notes on the absence of other options: The dataset provided does not include a separate list of multiple-choice options to compare against, so the explanation focuses on validating the single stated ordering by applying the general trends for oxoacids of halogens. If alternative options were present, each would be weighed against these same principles (oxidation state, number of oxygens, and central atom electronegativity) to determine relative acidity.

CHEM 1220 SP2025 (18215) CHEM 1220 Practice Exam #3 v1 (16.6 - 16.10, 17.1 - 17.3)- Requires Respondus LockDown Browser

Arrange the following substances in order from weakest to strongest acid: HClO3, HOI, HBrO2, HClO2, HIO2.

查看解析

登录即可查看完整答案

类似问题

Question at position 29 What distinguishes a weak acid from a strong acid?Weak acids completely dissociate into ions in solutionWeak acids have higher acidity than strong acidsWeak acids release more hydrogen ions in water than strong acidsWeak acids only partially ionize in water

Which of the following 0.10 M aqueous solutions gives the lowest pH?

Examine the Ka values for the acids shown below. Acid Name Ka HOBr Hypobromous acid 3.3 × 10–9 CH3CO2H Acetic acid 1.8 × 10–5 HCO2H Formic acid 1.8 × 10–4 C6H5OH Phenol 1.0 × 10–10 Consider 0.10 M aqueous solutions of each acid. Arrange these solutions in order of increasing [H3O+].

Which acid is the strongest?

Which of the following is the weakest acid?

Consider the acid ionization constants given below: Acid Ka HOCl 3.5 × 10–8 HCO2H 1.8 × 10–4 HBrO3 ~ 2 HOI 2.0 × 10–11 HClO2 1.1 × 10–2 When the conjugate bases are listed from the strongest to the weakest base, the order is:

Which of the following is the weakest acid?

Rank the following acids from lowest to highest pka.

更多留学生实用工具

考试浏览器助手

风格化写作助手

论文查重助手

文献引用助手

课堂转译助手

课堂笔记助手

Quiz搜索助手

学校历年真题

智能刷题助手

智能匹配练习

希望你的学习变得更简单