What are the equilibrium concentrations of all the solute species in a 1.1 M solution of...
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 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.
What is the pH of a solution that is 0.18 M KOCN and 0.14 M HOCN (cyanic acid)? (Ka for HOCN is 3.5 x 10^-4) pH=
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...
Question 10 1 pts What hazard classification would you expect a 90% ethyl acetate/10% hexane mixture to have? Flammable liquid Corrosive Toxic Flammable solid Question 16 1 pts The TLC diagram shown represents the analysis of three different compounds. Which of the three columns is/are likely to represent a pure compound, and why? 0 0 2 * 3 Columns 1 and 3, because there is only one spot in each. Column 2 only, because there are two spots present Columns...
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 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...
Calculate the concentrations of all species in a 1.02 M Na.SO, (sodium sulfite) solution. The ionization constants for sulfurous acid are K1 = 1.4 x 10-2 and Ka = 6,3 x 10- (Nat] = M (S01 (HSO;] MH,80] = (OH) = M (H+) =
Chem II Common Assignment: Equilibrium and Buffers 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...