Determine the concentrations of the ionic species present in a
0.268 M solution of the
NaO2CCOCH2CO2Na.
(pKa1=3.40, pKa2=5.11 for
HO2CCOCH2CO2H). Find the
concentration of:
a) [HO2CCOCH2CO2H]
b)[HO2CCOCH2CO2-]
c) [-O2CCOCH2CO2-]
d) [H3O+]
e) [OH-]
Determine the concentrations of the ionic species present in a 0.268 M solution of the NaO2CCOCH2CO2Na....
Determine the concentrations of the ionic species present in a 0.0340 M solution of the H2CrO4 . (pKa1 = 0.74 , pKa2 = 6.49 ). 1. [ H2CrO4 ] 2. [ HCrO4- ] 3. [ CrO42- ] 4. [H3O+] 5. [OH-]
NEED HELP ASAP Determine the concentrations of the ionic species present in a 0.352 M solution of the H2CrO4 . (pKa1 = 0.74 , pKa2 = 6.49 ). [ H2CrO4 ] [ HCrO4- ] [ CrO42- ] [H3O+] [OH-]
NEED HELP ASAP Determine the concentrations of the ionic species present in a 0.0660 M solution of the NaO2CCH2CO2Na. (pKa1=2.83, pKa2=5.69 for HO2CCH2CO2H) (in M) [HO2CCH2CO2H] [HO2CCH2CO2-] [-O2CCH2CO2-] [H3O+] [OH-]
NEED HELP ASAP Determine the concentrations of the following ionic species present in a 0.305 M solution of the diprotic acid H2SO3. For H2SO3, Ka1 = 1.4E-2, Ka2 = 6.3E-8. What is the H3O+ ion concentration? What is the HSO3- ion concentration? What is the SO32- ion concentration?
NEED HELP ASAP Determine the concentrations of the following ionic species present in a 0.279 M solution of Na2SO3. For H2SO3, Ka1 = 1.4E-2, Ka2 = 6.3E-8 (in M) What is the OH- ion concentration? What is the HSO3- ion concentration? What is the SO32- ion concentration?
Calculate the pH and the concentrations of all species present in 0.11 M ascorbic acid (H2C6H6O6) solution. (Ka1=8.0×10−5), (Ka2=1.6×10−12) Part A: Calculate the pHpH of a 0.11 MM solution of ascorbic acid. Part B: Calculate the concentration of H2C6H6O6 in a 0.11 MM solution of ascorbic acid. Part C: Calculate the concentration of HC6H6O6−HC6H6O6− in a 0.11 MM solution of ascorbic acid. Part D: Calculate the concentration of C6H6O62−C6H6O62− in a 0.11 MM solution of ascorbic acid Part E: Calculate...
Use two concentration tables to calculate the concentrations of all species present in a 0.0641 M solution of KBrO. The Ka for HBrO is 2.8E-9. What is the concentration of K+? What is the concentration of BrO-? What is the concentration of the conjugate species formed from the reaction of aqueous KBrO? What is the hydronium ion (H3O+) concentration? What is the hydroxide ion (OH-) concentration?
What are the equilibrium concentrations of all the solute species in a 0.99 M solution of propanoic acid, HC3H5O2? (a) [H3O+], M; (b) [OH-], M; (c) [CH3CH2COOH], M; (d) What is the pH of the solution? For CH3CH2COOH, Ka = 1.34 x 10-5.
3) Determine the pH and the concentration of all species at equilibrium of a 0.045 M solution of the diprotic acid salicylic acid. pKa1 = 3.98 and pKa2 7.65. -
Calculate the concentrations of the molecular and ionic species and the pH in aqueous solution that has a formal composition of 0.2350 M KH2PO4 + 0.4300 M K2HPO4. ph of 7.46 What is the concentration of the molecular species H3PO4?