In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base. (C,H)3N(aq) + H0(1) → (C,H3)3NH*(aq) + OH (aq) BL B-L The formula of the reactant that acts as a proton donor is The formula of the reactant that acts as a proton acceptor is Submit Answer Retry Entire Group 8 more group attempts remaining

= 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 O

search ||| 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 I (aq) + H₂O (aq) HI(aq) + H₂O(l) HI(aq) + H,O) → I (aq) + H,O (aq) I (aq) + H,O (aq) → HI(aq) + H,O HI(aq) + H₂O(1) → I¯ (aq) + H₂O¯(aq) Ei Explmmation Check BROM C C S highlighted reactant Bronsted-Lowry Bronsted-Lowry neither acid base X $ 3/5 O Jessica V 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 000 Ar 图]

Match 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)