The value of Ka for phenol,
C6H5OH, is 1.00 x 10-10. Which of
the equations below illustrates this reaction for phenol?
A) C6H5OH (aq) +
H2O (l) -------C6H5O-
(aq) + H3O+ (aq)
B) C6H5OH (aq) +
H2O (l)
------C6H5OH2+ (aq) +
OH- (aq)
C) C6H5OH (aq) +
OH- (l) -----C6H5O-
(aq) + H2O (l)
D) C6H5OH (aq) +
H2O (l)
-----C6H5OH2+ (aq) +
H2O (l)
E) C6H5O- (aq) +
H2O (l) -------C6H5OH (aq) +
H2O (l)
Reaction D | |
Reaction E | |
Reaction B | |
Reaction A | |
Reaction C |
The value of Ka for phenol, C6H5OH, is 1.00 x 10-10. Which of the equations below...
1.) The organic solvent phenol, C6H5OH dissociates to a small extent in water according to the following equilibrium equation: C6H5OH(aq) ⇄ C6H5O - (aq) + H + (aq) Use Le Chatelier’s principle to predict which form of phenol (C6H5OH or C6H5O - ) will increase in concentration as a result of the addition of HCl. 2) Oxalic acid forms a stable transition metal complex with Fe3+(aq). Use Le Chatelier’s principle to explain why the addition of oxalic acid to a...
Phenol (C6H3OH), commonly called carbolic acid, is a weak organic acid. C6H5OH(aq) + H2O(l) # C6H50- (aq) + H30+ (aq) Ka = 1.3 x 10-10 If you dissolve 0.300 g of the acid in enough water to make 856 mL of solution, what is the equilibrium hydronium ion concentration? [H30+1=C M What is the pH of the solution? pH = 0
A mixture of 0.0500 moles of each of the following is prepared in 1.000 L of DI water: HCl (large Ka) CH3COOH, acetic acid (Ka = 1.8x10-5) C6H5OH, phenol (Ka = 1.6x10-10) 1. Account for all activity coefficients and for the changes caused by the solution having an ionic strength that should not be neglected by including the appropriate activity coefficients, determine the concentrations of the species listed below at equilibrium in the solution: HCl, Cl-, H3O+, CH3COOH, CH3COO-, C6H5OH,...
How to solve
tions of 16.122 The equilibrium equations and Ka values for three reaction systems are given below. NH (aq)H2O H3O + NH(aq); Ka= 5.6 x 10-10 H2CO3(aq) + H2O H.O (aq) + HCO3 (aq); Ka= 4.3 x 10-7 H2PO4 (aq) +H2O H2O (aq)+ HPO4 (aq); Ka 6.2 X 10 a Which conjugate pair would be best for preparing a buffer with a pH of 6.96? Why? ranare 100 mlof a buffer with
Answer ASAP please!!!
8. Calculate the percent ionization in a 0.56 M aqueous solution of phenol (C6H5OH), if the pH is 5.07 at 25°C (Ka = 1.3 x 10-10). A. 1.5 x 10-3 % B. 1.1 x 10-1 % C. 1.5 x 10-5% D. 2.5 % E. 3.5 x 10-3% [Ni(en)]2+ (aq) + 6 NH3 (aq) 9. What is Keq for the following reaction? [Ni(NH3)]2+ (aq) + 3 en (aq) = Ký [Ni(NH3)4]2+ = 1.2 x 109 K [Ni(en)]2+ =...
Use the two given equations to determine the K3 value for the desired equilibrium equation. Given 1: 2H2O(l)= H3O+(aq)+OH-(aq) K1=1.00X10^-14 Given 2: HCN(aq)+H2O(l)=H3O+(aq)+CN-(aq) K2=4.90X10^-10 Given 3: CN-(aq)+H2O(l)=HCN(aq)+OH-(aq) K3=??? What is the K3 value?
A student makes a solution of 1.00 X 10^-7 M NaOH at 298K. Which of the following is NOT true for this solution at 25C? a) [OH-] > 1.0 X 10^-7 b) [OH-][H3O+] = 1.0 X 10^-14 c) [OH-] > [H3O] d) [OH-] = 1.0 X 10^-7 e) [OH-]/[H3O+]>1 Explain why!! Please
9) What is the H+ ion concentration in a 4.8 x 10–2 M KOH solution? A) 4.8 x 10–2 M B) 1.0x 10–7 M C) 2.1 x10–13 M D) 4.8 x 10–11 M 10) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-? A) HA (aq) + H2O (l) H2A+ (aq) + OH-(aq) B) A- (aq) + H3O+ (aq) C) HA (aq) + OH- (aq) H2O (l) + H+ (aq) HA (aq) + H2O...
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O (l) A 1.0 L buffer solution is 0.280 M in HC2H302 (acetic acid) and 0.320 M in NaC2H302 (sodium acetate). Calculate the pH of the budder and he Ka for HC2H3O2 IS 1.8 X 10-5 Calculate the pH of te solution above after the addition of 0.0400 moles of solid NaOH. Assume no volume change upon the addition of base.
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?