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.
What are the equilibrium concentrations of all the solute species in a 0.99 M solution of...
What are the equilibrium concentrations of all the solute species in a 1.1 M solution of cyanic acid, HOCN? (a) [H30+], M; (b) (OH), M; (c) [HOCN), M; (d) What is the pH of the solution? For HOCN, Ka = 3.5 x 10-4. (a) M (b) M (c) M (d)
What are the concentrations of all the solute species in 1.05 M lactic acid, HC3H5O2? What is the pH of the solution? This acid has a Ka = 1.4 × 10-4.
Calculate the equilibrium concentrations of all chemical species present in a 0.10 M H2CO3(aq) solution. What is the percent ionization of the acid and resulting pH? [H2CO3] = [HCO3-] = [CO32-] = [H3O+] = % ionization = pH = Acid Acetic Ammonium Formula CH:COOH NH4+ H2BO: Boric Carbonic H2CO3 HC1O2 HCOOH Chlorous Formic Hydrocyanic Perchloric 1.8 x 105 5.6 x 10-10 5.4 x 10-10 4.5 x 10-7 4.7 x 10-11 1.1 x 10-2 1.8 x 10-4 5.2 x 10-10 Very...
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...
The Ka of propanoic acid (C2H5COOH) is 1.34 × 10-5. Calculate the pH of the solution and the concentrations of C2H5COOH and C2H5COO– in a 0.421 M propanoic acid solution at equilibrium.
Acetic acid, CH3CO2H, is the solute that gives vinegar its characteristic odor and sour taste. (Ka was not given in this question) Part A: Calculate the pH in 0.840 M CH3CO2H. Part B: Calculate the concentrations of all species present (H3O+, CH3CO2−, CH3CO2H, and OH−) in 0.840 M CH3CO2H. Part C: Calculate the pH in 0.139 M CH3CO2H. Part D: Calculate the concentrations of all species present (H3O+, CH3CO2−, CH3CO2H, and OH−) in 0.139 M CH3CO2H.
5.) Calculate the concentrations of all the species and the pH in 0.25 M hypochlorous acid, HOCL. For HOCL, Ka=3.5x10^-8 6.) the pH of a 0.115M solution of chloroacetic acid, CICH2COOH, is measured to be 1.85. Calculate the Ka for this monoprotic acid Calculate the concentrations of all the species and the pH in 0.25 M hypochlorous acid, HOCI. For HOC, Ka :3.5 x 108. .) The pH of a 0.115M solution of chloroacetic acid, CICH2COOH, is measured to be...
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...
Calculate the equilibrium concentrations of all chemical species present in a 0.10 M H CO.(aq) solution. What is the percent ionization of the acid and resulting pH? Units Units [H2CO3) = Number [HCO3) = Number [CO32) = Number [H30+) = Number Units Units % ionization = Number pH = Number Ka Acid Acetic Ammonium Formula CH3COOH NH4+ H3B03 1.8 x 10-5 5.6 x 10-10 5.4 x 10-10 Boric Carbonic H2CO3 Chlorous Formic Hydrocyanic Perchloric HCIO2 HCOOH HCN HC104 4.5 x...
The Ka of propanoic acid (C2H5COOH) is 1.34 × 10-5. Calculate the pH of the solution AND the concentrations of C2H5COOH AND C2H5COO– in a 0.323 M propanoic acid solution at equilibrium. Please explain each step in detail.