Choose balanced equations showing how the HSO₃⁻ ion of sodium hydrogen sulfite, NaHSO₃, can be a Brønsted base. (Select all that apply.)- □ HSO₃⁻ (aq) + ClO⁻ (aq) ⇌ SO₃²⁻ (aq) + HClO (aq)- □ HSO₃⁻ (aq) + HNO₃ (aq) ⇌ H₂SO₃ (aq) + NO₃⁻ (aq)- □ HSO₃⁻ (aq) + HCl (aq) ⇌ H₂SO₃ (aq) + Cl⁻ (aq)- □ HSO₃⁻ (aq) + OH⁻ (aq) ⇌ SO₃²⁻ (aq) + H₂O (ℓ)- □ HSO₃⁻ (aq) + Na⁺ (aq) ⇌ NaHSO₃ (s)

Bronsted Lowry base is a substance which acts as proton acceptor whereas bronsted Lowry acid is a…

b Choose balanced equations showing how the HSO3 ion of sodium hydrogen sulfite, NaHSO3, can be a Bronsted base. (Select all that apply.) HSO3 (aq) + Cl0 (aq) 2 S03² (aq) + HC10(aq) HSO3 (aq) + HNO3(aq) 2 H2SO3(aq) + NO3 (aq) HSO3- (aq) + HCI(aq) 2 H2SO3 (aq) + Cl (aq) |HSO3 (aq) + OH (aq) 2 SO3² (aq) + H2O(£) | HSO3 (aq) + Na*(aq) 2 NaHSO3 (s)

b Choose balanced equations showing how the HSO3 ion of sodium hydrogen sulfite, NaHSO3, can be a Bronsted base. (Select all that apply.) HSO3 (aq) + Cl0 (aq) 2 S03² (aq) + HC10(aq) HSO3 (aq) + HNO3(aq) 2 H2SO3(aq) + NO3 (aq) HSO3- (aq) + HCI(aq) 2 H2SO3 (aq) + Cl (aq) |HSO3 (aq) + OH (aq) 2 SO3² (aq) + H2O(£) | HSO3 (aq) + Na*(aq) 2 NaHSO3 (s)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question in image attached. Balanced net ionic equation Which component in the net ionic equation is the acid? Which component in the net ionic equation is the base? Which component in the net ionic equation is the conjugate acid? Which component in the net ionic equation is the conjugate base?
Which equation below is correct when HCI is added to a buffer solution of HCO₂H/NaHCO₂? NaHCO2(aq) + HCO2H(aq) →→ HCl(aq) + NaCl(aq) NaHCO2(aq) + HCl(aq) → HCO₂H(aq) + NaCl(aq) HCO₂H(aq) + HCl(aq) + NaHCO2(aq) + NaCl(aq) NaOH(aq) + HCl(aq) →→→→ H₂O(l) + NaCl(aq)
Homework helppp
Determine the concentration of a NHCl aqueous solution that has a pH = 5.975. The base ionization constant of ammonia, NH, is: Kb=1.78 × 10-5. Round off your answer to 3 sig. figs. Reaction: NH4Cl (aq) → NH4+ (aq) + Cl- (aq) NH4+ (aq) + H2O (l) ↔ NH3 (g) + H3O+ (aq).
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)
Answer the following using acid, base, conjugate acid, conjugate base.
Question 16 of 21 Which one of the following represents the molecular equation for the reaction of HNO3 with CSOH? A) CSOH (aq) + HNO3 (aq) → H₂O (1) + CSNO, (aq) B) Cst (aq) + NO3(aq) → CSNO, (s) C) H+ (aq) + OH- (aq) → H₂O (1) D) CSOH (aq) + HNO3 (aq) → H₂O (aq) + CSNO, (s)
Which one of the following is classified as a base? Question 5 options: HCl (aq) CO2 (g) NaCl (aq) LiOH(aq)