2- Given HCO3(aq) +HSO3(aq) = H₂CO3(aq) + SO3²- (aq) The Bronsted - Lowry acids in the above equation are HCO3(aq) and HSO3(aq) O HSO3(aq) 2- O and S03²- O HSO3(aq) (aq) and H₂CO3(aq) HCO3(aq) and H₂CO3(aq)
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- In the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HClO2(aq) + H2O(l) = H3O+(aq) + ClO2 (aq) H2CO3(aq) + H2O(l) → H3O+(aq) + HCO3(aq) Answer Bank H2O(l) + CH3NH3(aq) = CH3NH2(aq) + H3O+ (aq) CA B CB A CH3COOH(aq) + H2O(1) = CH3COO¯(aq) + H3O+ (aq)For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. highlighted reactant reaction Bronsted-Lowry acid Bronsted-Lowry base neither HCl(aq) + OH (aq) → Cl (aq) + H,O(1) HCl(aq) + OH (aq) → Cl (aq) + H,O(1) Cl (aq) + H,O(1) HCl(aq) + OH (aq) Cl (aq) + H,O(1) → HCl(aq) + OH (aq)Which of the following are acid-base reactions? 1. AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq) 2. NH3(aq) + H2O(1) + OH-(aq) NH4" (aq) + 3. Zn(s) + 2Ag*(aq) → 2Ag(s) + Zn2+ (aq) a. 3 only b. 1, 2, and 3 c. 2 only d. 2 and 3 e. 1 only
- O ACID-BASE EQUILIBRIA Identifying Bronsted-Lowry acids and bases For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. highlighted reactant reaction Bronsted-Lowry Bronsted-Lowry neither acid base HBr(aq) + H,O(1) → Br (aq) + H;O*e Br (aq) + H,O(1) → HBr(aq) + OH (aq) NH3(aq) + H,O(1) → NH(aq) + OH (aq) NH (aq) + H,O(1) → NH3(aq),+ H;O"(aq) Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use I Priva MacBook Air IIPhosphoric acid, H3PO4, is a polyprotic acid. What is the THIRD ionization reaction for phosphoric acid in water? HPO (aq) → H+ (aq) + PO³ (aq) ○ H3PO4 (aq) → 3 H+ (aq) + PO¾- (aq) 4 H₂PO (aq) → HPO²¼¯ (aq) + H+ (aq) H3PO4 (aq) → H₂PO (aq) + H+ (aq)Identify the Bronsted-Lowry acid and base on the left side of the equation and the conjugate acid and conjugate base on the right side. HBr0 (aq) + H,0 (I) H30* (aq) + Bro (aq) HSO, (aq) + HCO, (aq) so, (aq) + H,CO3 (aq) 2- HSO; (aq) + H,0* (aq) H,SO; (aq) + H,0 (1)
- Identify the equation that shows the anion functioning as a base in the correct manner. O NO2 (aq) + H20(liq) 2 NO3 (aq) + OH (g) O F'(aq) + H2O(1) 2 HF(aq) + H3O*(aq) O HPO,2 (aq) + H2O(liq) 2 H,PO,'(aq) + OH'(aq) O clO (aq) + H20(liq) 2 HCIO(ag) + H2(g)= O ACIDS AND BASES Identifying Bronsted-Lowry acids and bases For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. reaction NH(aq) + OH (aq) → NH3(aq) + H₂O(1) NH3(aq) + H₂O(1)→ NH(aq) + OH(aq) NH4(aq) + OH (aq) ► NH3(aq) + H₂O(1) NH3(aq) + H₂O(1)→ NH(aq) + OH(aq) 1 highlighted reactant Bronsted-Lowry Bronsted-Lowry acid base O O O O O neither O O 0 0/5 O31. For each reaction, identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conju- gate base. (a) HBr(aq) + H₂O(l) →→→ H3O+ (aq) + Br¯(aq) (b) NH3(aq) + H₂O(l) — NH4+ (aq) + OH¯(aq) (c) HNO3(aq) + H₂O(1) H3O+ (aq) + NO3¯(aq) (d) C₂H5N(aq) + H₂O(l) — C₂H5NH+ (aq) + OH¯(aq)
- When NaCLO(s) dissolves in water it dissociates as follows NaCLO(s) + H2O(l) →Na+(aq) + CLO-(aq) is the conjugate base of the weak acid, hypochlorous acid, as follows: CLO- (aq) + H2O(l) ⇌HCLO(aq) + OH- (aq) How many grams of NaCLO must be added to 2.00 L of water to make a solution with a pH of 10.50? Kb = [HCLO-][OH-]/[CLO-] = 3.3x10−7 a) 0.46 grams b) 23 grams c) 0.31 grams d) 46 gramsMatch the acid to the correct chemical equation showing its reaction with water. hydrochloric acid hypochlorous acid chlorous acid chloric acid perchloric acid A. HClO2(aq) + H2O(l) ⇌ ClO2−(aq) + H3O+(aq) B. HCl(aq) + H2O(l) ⇌ Cl−(aq) + H3O+(aq) C. HClO2(aq) + H2O(l) → ClO2−(aq) + H3O+(aq) D. HClO3(aq) + H2O(l) ⇌ ClO3−(aq) + H3O+(aq) E. HClO(aq) + H2O(l) → ClO−(aq) + H3O+(aq) F. HClO(aq) + H2O(l) ⇌ ClO−(aq) + H3O+(aq) G. HClO4(aq) + H2O(l) → ClO4−(aq) + H3O+(aq) H. HClO3(aq) + H2O(l) → ClO3−(aq) + H3O+(aq) I. HClO4(aq) + H2O(l) ⇌ ClO4−(aq) + H3O+(aq) J. HCl(aq) + H2O(l) → Cl−(aq) + H3O+(aq)O ACID-BASE EQUILIBRIA Identifying Bronsted-Lowry acids and bases For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. highlighted reactant reaction Bronsted-Lowry Bronsted-Lowry neither acid base NH3(aq) + H,O(1) → NH(aq) + OH (aq) NH,(aq) + H,O(1) → NH (aq) + OH (aq) NH (aq) + OH (aq) → NH3(aq) + H,O(1) t. NH(aq) + OH (aq) → NH3(aq) + H,0(1) Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privac II