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-]
Determine the concentrations of the ionic species present in a 0.0340 M solution of the H2CrO4...
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-]
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-]
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 (H2CO3, HCO3 – , CO3 2– , H3O + , and OH– ) in a 0.0037 M M carbonic acid solution. Ka1 = 4.3 × 10–7 ; Ka2 = 5.6 × 10–11
Calculate the molar concentrations of oxalic acid (COOH)2, HOOCCO2-, (CO2)22-, H3O+, and OH- in 0.15 M (COOH)2 (aq). This is a special case of general diprotic acid dissociation. First, we need to find the pKa1 and pKa2 in the water at room temperature, which is available online e.g. Wikipedia (oxalic acid). pKa1 = 1.23, pKa2 = 4.19. Either solve numerically or analytically. Report here [H3O+] = ______ M. 2 sig. figures.
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.
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?
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...