justify nh4+is conjugated acid of hco3-
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...
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:
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!
The conjugate acid of NH3 is Select one a. NH21+ b. NH4 Ở c. NH21- Ô d, NH4OH e. There is not conjugate acid of this compound. The conjugate base of NH4+ is Select one: a. NH3 b. NH2 C. NH31+ d. NH3- e. There is no conjugate base of this ion. The formula for the conjugate base of HCO3- is Select one: a. co32 b. H2CO3 OC. CO2 d. C031- The conjugate acid of H20 is Select one: a....
Question 16 Identify which of the following is NOT conjugated acid-base pair: HBr/HBrO ОСІГІНСІ CH3COOH/CH3COO O NH3/ NH4+ Question 20 The isotonic solution of glucose contains 5.0 % (m/v) glucose. If a nurse injects a 4,3 % (m/v) of glucose solution. What will happen to REC (red blood cell swell and burst no change shrink color change A Click Submit to complete this assessment. Question 8 Write correct IUPAC name of H104 Hydro lodo tetraoxide Periodic acid Hydrolodous acid Hydrolodic...
HCO3 + HCO3 = Acid Base 3. Complete the table of values below for the aqueous solutions at 25°C using your calculator. (No need to show your calculation here) [H] [OH-1 PH рон 2.7 x 10-8 M M 8.60
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
8. (4 pts) Give the equations for the hydrolysis of: a. NH4* (as an acid) NHA HO → Nit, , b. HCO3 (as a base) HCO₃ + H2O + H₂ t, that 9. (6 pts) State for each of the following examples if it is acidic, basic, or neutral. a. Na2SO4 b. KFC . FeBrs 10. (6 pts) Determine the pH of a 0.077 M solution of boric acid. Ks of boric acid = 5.4 x 10-10 rH= pka log...
In waters affected by acid rain the concentrations of the three carbonic acid species (H2CO3, HCO3-, CO32-) are determined by concentration of the strong acid deposited by acid rain, as well as the concentration of H2CO3 which is controlled by the solubility of carbon dioxide . Under these conditions (constant H2CO3 and relatively low pH) the only carbonic acid equilbrium of importance is the conjugate base reaction of HCO3-, which is related to, but not identical to - and not...
Identify the products formed in this Brønsted-Lowry reaction. HCO3 + CN = acid + base acid: base: