Determine the conjugate acid/base pair in each reaction
1) HS- + OH- -->
2) H2PO4- (acid) / (CB)
3) HS- (Base) / (acid)
1. H2O + HS- <-> OH - + H2S
H2O acid ( donates H+)
HS- base (accepts H+)
For reverse reaction
OH- conjugate base (accepts H+)
H2S cojugate acid (donates H+)
2. HPO42- is the conjugate base of H2PO4-. The conjugate base of an acid, even a polyprotic one, always has one less H than the acid.
3.HS- is conjugate base and H2S is conjugate acid
Determine the conjugate acid/base pair in each reaction 1) HS- + OH- --> 2) H2PO4- (acid) / (CB)...
Identify the conjugate base for each acid. conjugate base of H,SO, conjugate base of HS": conjugate base of NH : Identify the conjugate acid for each base. conjugate acid of HS: conjugate acid of HPOZ: conjugate acid of NH,: Identify the products formed in this Brønsted-Lowry reaction. HPO4 + BrO acid + base acid: base: A monoprotic weak acid, HA, dissociates in water according to the reaction HA (aq) + H2O(1) = H, 0+ (aq) + A-(aq) The equilibrium concentrations...
1. Identify the acid (A), base (B), conjugate acid (CA) and the conjugate base (CB) in the following equation (5) NH3(aq) + H2O + NH(aq) + OH(aq) B CB CA 2. Determine the pH of a solution at 25°C in which the hydronium ion [H3O+] is 3.5 X 10 - log 3.5x10-4 - pH = 3.45 M. C 3. Calculate the [H3O+] in a solution at 25°C in which the pH is 4.76. (5)
Which of the following is a conjugate acid/ base pair? A) H3PO4, PO43- B) H2PO4 , PO43- C) HPO42-, PO43- D) H3PO4, HPO42-
1. Identify the acid, base, conjugate acid and conjugate base in the following reaction: HPO42+ H20 OH H2PO4 2. Calculate the following a) pH of a [H30*] = 2.76 x 104 M b) pH of a [OH] - 8.5 x 10-6 M c) [H30*] and [OH] for a soln pH 5.73 3. Show how an incoming acid [H30*] is neutralized by the buffer system HCO3 /CO32 system. You should also be able to show the neutralization of incoming base [OH']...
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) +...
H2S + NH3 = NH4+ + HS- OH- + H2PO4- = H2O + HPO42- In the above reactions, NH3 and H2PO4- are: A. Acid and Base B. Base and Acid. C. Acid and acid D. Base and base
7. a) Identify the conjugate acid-base pairs in the following reaction: NH3(aq) + H O(l) + NHa*(aq) + OH (aq) b) The conjugate acid of HCO3 ? c) The conjugate base of H2PO4? d) Which of the following is not a conjugate acid-base pair? A) NH4+/NH3; B) H30*70H; C) H2SO3/HSO3; D) C2H3027HC2H302; E) All of the above are conjugate acid-base pairs.
(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....
Given: H2PO4 + HS =HPO42- + H2S In the forward reaction, HS is acting as a Bronsted acid In the forward reaction, H2PO4 is acting as a Bronsted acid In the reverse reaction, HPO4 is acting as a Bronsted acid In the reverse reaction, H2S is a Bronsted base
1) Write equations for the following Brønsted-Lowry acid-base reactions and indicate each conjugate acid-base pair. a) HClO3 + H2O b) H2SO4 + H2O c) OH- + HPO4 -2