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need help with these 2 questions HCO3 + OH -> H2O + CO32- Acid: Base: Conjugate...
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
(d) Conjugate acid: OH"; conjugate base: H3* (e) None of these 5. Identify the conjugate acid/base pairs in the following equation (10) HASO4 + H2O <H2AsO4 + OH (A). HASO. (acid)HAsO4 (base): H2O (acid)/ OH (base) (B). HASO4 (acid)/HASO. (base): H2O (acid)/ OH (base) (C). H2AsO4 (acid)/ OH (base) ; H2O (acid)/HASO4 (base) (D). H AsO4 and H20 (acids): OH and HASO4(bases) (E). None of these 6. Which is an INCORRECT statement?(10) a) The conjugate base of H2O is OH....
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!
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?
Question 11 (2 points) D Which of the following does not represent a conjugate acid-base pair? HCO3/CO32 H3PO4/HPO42 OH/O-2 NH4 /NH3 Save Question 12 (2 points) D Consider the weak acid HCO3 whose pKa -10.32, which form will pre
1. For each reaction below Classify each acid, base, conjugate acid, and conjugate base as a strong acid, weak acid, strong base, or a weak base. Calculate the value of the equilibrium constant II. I. Determine if these reactions need to be treated as an equilibrium (needing an ICE table) or a stoichiometry problem (assuming the reaction goes essentially to completion) a. F-(aq) H2O() HF(aq) + H3O*(aq) + H2O(1) NH3(aq) + b. NH4 (aq) OH (aq) + H3O*(aq) NH3(aq) +...
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...
In each Reaction identify the Bronsted Lowry acid and base, the conjugate acid and conjugate base: a.H2CO3 + H2O(l) ----- H3O+ + HCO3- b.NH3 + H2O ----- NH4+ + OH-
helpp ConjugatedAB10. Select the conjugate acid of CO32 OH, CO3 HCO3 CO32- O CO3 Acid Strength4. Determine whether the following statement is True or False. 1.0 M HCl solution and 1.0 M acetic acid solution have the same hydronium ion concentration. True False
Question 4 (4 points) Match the acid to its conjugate base pair. - CO32- 1. H2CO3 2. HCO3 3. HCI 4. HNO3