a Choose balanced equations showing how the HSO3 ion of sodium hydrogen sulfite, NaHSO3, can be a Brønsted acid. (Select all that apply.) HSO; (aq) + CIo (aq) 2 So,2 (aq) + HC1O(aq) HSO; (aq) + HNO3(aq) 2 H2SO3(aq) + NO3 (aq) HSO; (aq) + HCI(aq) 2 H2 SO3 (aq) + Cl (aq) HSO3 (aq) + OH (aq) 2 So32 (aq) + H20(€) O HSO3 (aq) + Na* (aq) 2 NAHSO3 (s)

a Choose balanced equations showing how the HSO3 ion of sodium hydrogen sulfite, NaHSO3, can be a Brønsted acid. (Select all that apply.) HSO; (aq) + CIo (aq) 2 So,2 (aq) + HC1O(aq) HSO; (aq) + HNO3(aq) 2 H2SO3(aq) + NO3 (aq) HSO; (aq) + HCI(aq) 2 H2 SO3 (aq) + Cl (aq) HSO3 (aq) + OH (aq) 2 So32 (aq) + H20(€) O HSO3 (aq) + Na* (aq) 2 NAHSO3 (s)

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section16.10: The Lewis Concept Of Acids And Bases

Problem 1RC: 1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot...

See similar textbooks

Similar questions

Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. CaO b. SO2 c. Cl2O
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
For solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesnt change). a. [H+] b. pH c. [OH] d. pOH e. Ka
Write a net ionic equation to show that ascorbic acid, H2C6H6O6, behaves as an acid in water. Consider only its first ionization. ____ + H2O(l) → ____ + ____ Classify ascorbic acid as a monoprotic, diprotic or triprotic acid.
Arrange the following substances in order from weakest to strongest acid: HClO3, HOI, HBrO2, HClO2, HIO2.
Citric acid, which is present in citrus fruits, is a triprotic acid. (a) Calculate the pH of a 0.040 M solution ofcitric acid. (b) Did you have to make any approximationsor assumptions in completing your calculations? (c) Is theconcentration of citrate ion (C6H5O73-) equal to, less than,or greater than the H+ ion concentration?
Hydrazine, N2H4 has Kb= 1.3E-6. Calculate the pH of 0.486M solution of N2H4.
A solution has a pOH of 6.50 at 50∘C. What is the pH of the solution given that Kw=6.22×10−15 at this temperature?
A 0.0698 M solution of a base is 2.5% ionized. Calculate the base ionization constant Kb. How many acidic hydrogen atoms and how many nonacidic hydrogen atoms are present in each of the following molecules?(a) HC2H2ClO2 (chloroacetic acid),(b) H2C4H4O4 (succinic acid),(c) H2C8H4O4 (phthalic acid),(d) H2C4H6O2 (butyric acid)
Assuming the forward reactions are favored in the chemical equations below, arrange the acids according to INCREASING acid strength. HNO2(aq) + HCOO–(aq) ⇌ NO2–(aq) + HCOOH(aq) HN3(aq) + BrO–(aq) ⇌ N3–(aq) + HBrO(aq) N3– + HCOOH(aq) ⇌ HN3(aq) + HCOO–(aq) (a) < (b) < (c) < (d) acids: HNO2, CHOOH, HN3, HBrO
When SO2 dissolves in water to form sulfurous acid, H2SO3(aq), that acidcan donate a hydrogen ion to water. Write a balanced chemical equation forthis reaction, and identify the stronger Brønsted–Lowry acid and base in theequation.
Consider the base hydroxylamine, NH2OH. (a) What is theconjugate acid of hydroxylamine? (b) When it acts as a base,which atom in hydroxylamine accepts a proton? (c) Thereare two atoms in hydroxylamine that have nonbondingelectron pairs that could act as proton acceptors. Use Lewisstructures and formal charges to rationalizewhy one of these two atoms is a much better proton acceptorthan the other.