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 |
part A
Here water molecule is donating a H+ ion to the carbonate ion, therefore,
water is the acid (proton donor) and CO32- is the base ( proton acceptor).
second option is correct.
part B
Here again, the water molecule is providing the H+ ion for ammonia to form ammonium molecule. Therefore, Ammonia is the base (proton acceptor) and water is the acid ( proton donor).
first option is correct.
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...
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:
Identify the conjugate acid-base pairs in each of the following equations: 1) HF(aq)+CO32?(aq)?F?(aq)+HCO3?(aq) Check all that apply. a) F?/HCO3? b) HF/F? c) HF/CO32? d) HCO3?/CO32? 2) HCl(aq)+OH?(aq)?Cl?(aq)+H2O(l) a) HCl/OH? b) HCl/Cl? c) H2O/OH? d) H2O/Cl?
Identify the reactant that is a Brønsted−Lowry acid in the following reaction: CO32−(aq)+H2O(l)⇌HCO3−(aq)+OH−(aq) Express your answer as a chemical formula.
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
CH,OH)02 [CO2]2(H20] c. Qc 19. A is a proton donor. a. Bronsted Base b. Bronsted Acid c. Conjugate base d. Polymor 20. In order for a substance to act as a Bronst a. at least one double bond. b. at least one H* to donate. C. at least one single bond. d. at least one lone pair of electrons. 16. The Gibhbs energy for the reaction beiow is CH ( 50(p-3C0p-4no a. 0 b. -2108 kJmol c. -608.1 kmol d....
HCO3- + H2O CO32- + As drawn, the acid in the reaction is (HCO3- ) and the base is ( H2O) The conjugate acid is ( CO32- ) and the conjugate base is (H3O+ ) b) If a solution has a H3O+ concentration of 0.817 M, what is the pH? Provide your answer with 2 decimal places (13.91) can you please check my answers? Thanks!
Acids and bases: definitions Consider the following reactions: (a) NH4+ + CO32- → NH3 + HCO3 (b) 2 HBr + Ca(OH)2 → CaBr2 + 2 H2O (C) SO3 + H2O → H2SO4 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. NH4+ Choose... CO32- Choose... HBr Choose... Ca(OH)2 Choose... Choose... SO3 H2O in (c) Choose...
Part A In the acid-base mechanism, the base is a proton acceptor, and the acid is the proton donor. An acid-base reaction is visualized as the reaction in which proton transfer takes place. However, in a nucleophilic substitution reaction, the nucleophile attacks a substrate (usually an electrophile), and the leaving group is removed from the substrate as a weaker nucleophile. The nature of the reactants determines whether a reaction will proceed as an acid-base reaction or a nucleophilic substitution reaction....
1 Part A: The net ionic hydrolysis equation for aqueous ammonium chloride is: a.H2O(l)⇄H+(aq)+OH-(aq) b.NH4+(aq)+H2O(l)⇄NH4OH(aq)+H+(aq) c. NH4OH(aq)+HCl(aq)⇄NH4Cl(aq)+H2O(l) d. NH4Cl(aq)⇄NH4+(aq)+Cl-(aq) Part B: Adding acid to the buffer, NH3-NH4+, will produce this (net ionic) reaction: a. H+(aq)+OH-(aq)⇄H2O(l) b. H+(aq)+NH4+(aq)⇄NH3(aq)+H2(g) c. H+(aq)+NH4+(aq)⇄NH52+(aq) d. H+(aq)+NH3(aq)⇄NH4+(aq)
Which of the following is a Brønsted-Lowry acid-base reaction? CH3CH2NH2(aq)+C6H5COOH(aq)⇄CH3CH2NH3+(aq)+C6H5COO-(aq) H2O(l)+CO2(aq)⇄HCO3-(aq)+H+(aq) Fe3+(aq)+H2O(l)⇄FeOH2+(aq)+H+(aq) HCl(aq)+Zn(s)⇄ZnCl2(aq)+H2(g)