Acids and bases: definitions Consider the following reactions: (a) NH4+ + CO32- → NH3 + HCO3...
Acids and bases: definitions Consider the following reactions: (a) 2 NH3 + Ag* [Ag(NH3)2] (b) NH4 CO32- -NH3 + HCO3 (c) 2 HBr+ Ca(OH)2 CaBr2 + 2 H20 Match with the definitions that apply for the substances indicated. Note: In a given reaction, the same definition must apply for both the acid and base for it to hold true. NH3 in reaction (a) Brønsted-Lowry and Lewis base Agt Brønsted-Lowry and Lewis acid NH4+ Arrhenius, Brønsted-Lowry, and Lewis acid Соз2- Arrhenius,...
Acids and bases: Part I Consider the following reactions: (a) 2 NH3 + Ag+ → [Ag(NH3)2]+ (b) NH4+ + CO32- → NH3 + HCO3- (c) 2 HBr + Ca(OH)2 → CaBr2 + 2 H2O Match with the definitions that apply for the substances indicated. Note: In a given reaction, the same definition must apply for both the acid and base for it to hold true. Choices: a)Lewis-base b)Bronsted-Lowry and Lewis Base c) Lewis acid d) Arrhenius, Bronsted-Lowry, and Lewis acid...
Acids and bases: definitions ut of Consider the following reactions: (a) Ca(OH)2 + 2 HCI - CaCl + 2 H2O (b) CaH2 + 2 H2O + Ca(OH)2 + 2 H2 (c) BF3 + F - BF4 Match with the definitions that apply for the substances indicated. Note: In a given reaction, the same definition must apply for both the acid and base for it to hold true, Ca(OH)2 in reaction (a) Arrhenius, Bransted-Lowry, and Lewis base HCI Arrhenius, Bransted-Lowry, and...
Answer the question below: 1: i) Identify the Lewis acids and bases in each of the following reactions: a. NH3 + BF3 → F3B NH3 b. H2O + SO3 → H2SO4 c. NH4+ + OH- → NH3 + H2O d. CO2 + H2O → H2CO3 e. OH−+H+→H2O ii) Identify the following compounds as either a Lewis acid or Lewis base and as either Soft or Hard: a. Cr3+ b. SO3 c. SCN− d. I
need help with these 2 questions HCO3 + OH -> H2O + CO32- Acid: Base: Conjugate Acid: Conjugate Base: Question 21 HCI + NH3-NH4++CI Acid: Base: Conjugate Acid: Conjugate Base:
CO32−(aq)+H2O(l)←−→HCO3−(aq)+OH−(aq) acid (proton donor) CO32−, base (proton acceptor) H2O acid (proton donor) H2O, base (proton acceptor) CO2−3 Part B NH3(aq)+H2O(l)←−→NH4+(aq)+OH−(aq) acid (proton donor) H2O, base (proton acceptor) NH3 acid (proton donor) NH3, base (proton acceptor) H2O
a. List the following substances in decreasing order (strongest to weakest) of strength as acids and bases. Some may be used more than once. CO32–, NH4+, SO42¯, HS–, HPO42–, HO2–, H2Te b. Explain whether the reactants or products are favored at equilibrium HPO42– + S2– PO43– + HCO3¯ Fe(H2O)63+ + HS¯ HSO4– + NO3–
Identify conjugate acid-base pairs in each of the following reactions. NH3(aq) + H2O(l) = NH4+ (aq) + OH- (aq) Check all that apply. H2O/NH3 NH4+/NH3 H2O/OH NH4+/OH- Submit Request Answer Part B OH(aq) + HF(aq) = H20(1)+F- (aq) Check all that apply. H2O/F- H20/OH HF/F- HF/OH
Write equations for the reaction of each of the following Brønsted-Lowry acids and bases. Identify the conjugated acids and bases. a. Acid: H20; base: NH3 b. Acid: NH4+, base: OH- c. Acid: HSO4; base: H2O d. Acid: HCl; base: H2PO4 6.4
I am studying Acids & Bases. I understand that Acids ionize, creating ions that were not previously there. I understand that Bases dissociate, simply breaking the compound apart into its individual ions. Acids ionize to create (H3O) ions by producing/donating an (H+) ion Bases dissociate, with one ion being (OH-) But I am confused about the Bases.... I get that the compound breaks apart, and that bases dissolve/accept protons but if you are looking at this chemical equation, which dissociates...