Which is NOT an amphiprotic species in water?
| HSO4– | |
| HS– | |
| HClO3 | |
| HSO3– | |
| HCO3– |
Which is NOT an amphiprotic species in water? HSO4– HS– HClO3 HSO3– HCO3–
Why is the H2SO4 unable to accept a proton?
Correct answer: HS- NH3 Amphiprotic species are able to both accept and donate protons. According to the Brønsted-Lowry definitions of acids and bases, amphiprotic species can act as both acids and bases. H2SO4 will donate, but not accept a proton. PO will accept a proton, but has no proton to donate.
6- (a) What is the conjugate base of each of the following HCIO4, H2S, PH4, HCO3- ? (b)- The hydrogen sulfite ion (HSO3) is amphiprotic. Write an equation for the reaction of HSO3- with water, in which the ion acts as an acid
Which species is the conjugate base of HS-? A. H2S ...number is a subscript B. HS- C. S^2- D. HSO4- ...number is a subscript E. H2SO4 ...numbers are subscripts
5. Which of the following species is amphiprotic in aqueous solution? (a) CH,NH, (b) H0 C)NH, (d) F (e) HSO, 6. Use Table 15.2 (page 529) to decide whether the species on the left or those on the right are favored by the reaction. a. NH, (aq) + H2PO4 (aq) # NH(aq) + H2O b.HCN (aq) + HS (aq) CN (aq) +HS
Which one of the following species is amphiprotic? Select one: PO43–(aq) HCl(g) HSO4–(aq) Cl–(aq) For the system NH2OH + CH3NH3+⇌ CH3NH2 + NH3OH+ 95% 95 % 5 % 5 % the state of equilibrium in the system is described by the percentages given. Which of the species is the strongest base in the system? Select one: NH2OH CH3NH3+ CH3NH2 NH3OH+ An aqueous solution at 25.0 oC has an H3O+ concentration of 4.0 × 10–2 mol L–1. What is the OH–...
3. Identify which reactants are amphoteric species in the following reactions. For those species, determine if the compound is also amphiprotic. Reaction Amphoteric Reactant Amphiprotic? (Y or N) HCO3 + HBr = H2CO3 + Br- 3 HCI + Al(OH)3 = AlCl3 + 3 H2O 2 HBr + ZnO = ZnBr2 + H2O
Which of the following could not be a Bronsted acid? O2- HCO3- HS- HCl NH4+
3.State which of the following species are amphiprotic and write chemical equations illustrating the amphiproticcharacter of these species.(a) NH3 (b)HPO4− (c) Br− (d)NH4+ (e)ASO43−
Write the balanced Ka and Kb reactions for
HSO3- in water. Be sure to include the
physical states of each species involved in the reaction.
Write the balanced Ka and Kb reactions for HSO3 in water. Be sure to include the physical states of each species involved in the reaction. Ka: NOTE: Use the chemical equation editor tool to input the physical states. Do not subscript the physical states of the compounds. Kb:
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e) HSO (d) F (b) Н:0" 6, Use Table 15.2 (page 529) to decide whether the species on the left or those on the right are favored by the reaction. a. NH4 (aq) + H2PO4" (aq) # NH3(aq) + HsPO b. HCN (aq) + HS(aq) CN" (aq) +H2S c. HCO +OH CO2 H2S d. Al(H20)6 3+ +OH = Al(H20) s2+ OH 7. The equilibrium constant...