2021年12月6日 · (1) H2SO4 + H2O = (double headed arrows) HSO4- + H3O+ The conjugate base of H2SO4 is HSO4- and this is because HSO4- if we consider the reverse reaction, HSO4- is a base and it would accept the proton to become H2SO4. so, its the conjugate base of H2SO4 and H2SO4 is the acid of HSO4- since it would donate H+ to become HSO4-.

2020年12月7日 · In the case of HSO4-, the substance could gain a H+ (in the presence of a separate acid), which would yield H2SO4. Or HSO4- could lose a H+ (in the presence of a separate base) to yield SO4 2-. Because the substance can either donate or gain an H+ (depending on the surrounding solution), then the substance is amphoteric.

2021年1月22日 · At first I thought the reaction would be: H2SO4 + H2O --> HSO4- + H3O+, since the first Ka was listed as "strong", [H3O+] = [H2SO4] and you calculate pH from there. However, when I looked at the answer key they went to the second Ka, and the reaction was: HSO4- + H2O --> SO4^2- + H3O+, and they found the pH after using the second Ka value and a ...

2020年12月6日 · I think in regards to HSO4- specifically, that it is not an amphoteric compound because its conjugate acid (if it were to accept a proton) is a strong acid, and thus will dissociate again; so HSO4-, if it does briefly accept a proton, will just dissociate again into HSO4- because of the strong acid nature of H2SO4.

2022年1月18日 · You have the correct Ka2 value to use but the ICE table should be set up for the equation HSO4- (aq) + H2O (l) --> SO4 2-(aq) + H3O+ (aq) with the initial concentrations being 0.15 M for HSO4- and H3O+ and 0 M for SO4 2-

2016年12月3日 · The first time, H2SO4 is completely ionized into HSO4- and H3O+. Since the ionization is complete, the concentration of HSO4- is 0.15M and the concentration of H3O+ is 0.15M (same concentration as H2SO4). The next ionization is incomplete, so an ICE table is needed. The equation for the second ionization is HSO4- + H2O (double arrow) SO42- + H3O+.

2019年12月5日 · The first reaction is SO2 + H2O = H2SO3, the next reaction is 2SO2 + O2= 2SO3, and the last reaction that takes place to form the sulfuric acid is SO3 + 2H2O = (H3O+) + (HSO4-). All of these equations and more details about acid rain …

2016年12月3日 · The chemical equation is HSO4- + H2O double arrows H3O+ +SO42-. You just use one equation for each part of this question and calculate the pH using the Henderson-Hasselbalch equation for the various concentrations of acid and conjugate base.

2020年12月7日 · For conjugate bases, a proton (H+) is removed, allowing the molecule to act as a base. For example, if we have HSO4- and H2O, the hydrogen on the SO4- becomes joined to the H2O, forming H3O+ (the conjugate acid since the H+ was added to it) and SO4-2 (the conjugate base since the H+ was removed from the molecule).

2018年12月6日 · Bronsted acids are actually characterized as donating protons, not accepting them, so in the case of H2SO4, the molecule would become deprotonated and lose one of its H atoms to become HSO4^(1-). This is a case in which an anion can act as an acid because HSO4^(1-) can donate another H+ to become SO4(2-).