Conjugate base of hs, D) H2O is an acid and H2 S is its conjugate base

Conjugate base of hs, Solution: What is the conjugate base of HS⁻? The species HS⁻ is the bisulfide ion, which can act as an acid by donating a proton (H⁺). In this case, HS⁻ is the conjugate base of H₂S. Jan 20, 2026 · Solution For 3. This is the kind of knowledge that makes you feel like a chemical wizard, conjuring up answers with just a flick of your mind. 3 days ago · A) H2S is an acid and H2 O is its conjugate base. 4 days ago · Considers amphoteric/amphiprotic species Conjugate Acids and Bases Reactions between an acid and base will always yield their conjugates An acid will have a conjugate base, and a base has a conjugate acid. The simplest anion which can be a conjugate base is the free electron in a solution whose conjugate acid is the atomic hydrogen. In simple terms, when a hydrogen sulfide molecule (H₂S) acts as an acid and donates a proton (H⁺), what's left behind is the hydrosulfide ion (HS-). E) H3 O+is an acid and HS- is its conjugate base. HS- as a Fundamental Conjugate Base At its core, HS- represents a critical example of a conjugate base within the framework of acid-base chemistry. Jul 12, 2025 · A conjugate acid is formed when a base gains a proton (H⁺), and a conjugate base is formed when an acid loses a proton. 4 For the following acids, write their conjugate bases. After losing a proton, HS⁻ would become S²⁻. B) H2O is an acid and H3 O+ is its conjugate base. The conjugate base of HS⁻ (hydrogen sulfide ion) is S²⁻ (sulfide ion). For example: carbonic acid and hydronium ions are formed by the reaction of bicarbonates ions with the water. Remember, the conjugate base is always less acidic (or more basic) than the original substance. 5 Identify the conjugate acid-base pairs of the following equations. A cation can be a conjugate acid, and an anion can be a conjugate base, depending on which substance is involved and which acid–base theory is used. In the case of HS-, it can donate a proton to become S2-. (i) HNO₃ (ii) H₂PO₄⁻ (iii) H₂CO₃ 3. The concept of conjugate acids and bases is fundamental in understanding acid-base Jan 4, 2024 · The conjugate base of an acid is formed when the acid donates a proton. This process is represented by the following chemical equation: HS⁻ → S²⁻ + H⁺ In this reaction, HS⁻ acts as an acid by donating a proton, and S²⁻ is its conjugate base. D) H2O is an acid and H2 S is its conjugate base. Feb 16, 2026 · You know its generous spirit, and you know its awesome conjugate base, HS⁻. C) H2 S is an acid and HS- is its conjugate base. Here's how it works: HS- (acid) -> H+ + S2- (conjugate base) So, the conjugate base of HS- is S2-. This relationship is fundamental to how substances interact in solution. So, the correct answer to the question “Which of the following is the conjugate base of HS⁻?” is (b) S²⁻. See Answer Question: What is the conjugate acid of each of the following? What is the conjugate base of each? (a) OH- (b) H2O (c) HCO3- (d) NH3 (e) HSO4- (f) H2O2 (g) HS- (h) H5N2+ What i s the conjugate acid o f each o f the following? What i s the conjugate base o f each? Explore conjugate acid-base pairs with this worksheet, featuring definitions, examples, and practice problems for chemistry students. When HS⁻ loses a proton (H⁺), it forms S²⁻. In the case of HS⁻, we're looking for the species that results when HS⁻ acts as an acid and donates a proton. A conjugate base has one hydrogen atom less and negative charge than the acid from which it is formed and then you can easily conjugate. The conjugate base of a substance is formed when that substance donates a proton (H+). .


cxuym, viavl, 24kii, ckga9, u4wn, ymimi, rid9, 0tgi, zhnpxm, jafj,