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 pH and the concentrations of all species present (H2CO3, HCO3 – , CO3 2–...
Calculate the pH and concentration of species present in a polyprotic acid solution.For a 3.44×10-3 M solution ofH2CO3, calculate both the pH and the CO32- ion concentration.H2CO3 + H2O → H3O+ +HCO3-Ka1 = 4.2×10-7HCO3- + H2O → H3O+ +CO32-Ka2 = 4.8×10-11pH =[CO32-] =
12. Calculate the pH and the concentration of all species in solution of 0.33 M K2CO3. For carbonic acid Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11
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...
Calculate the concentration of all species in a 0.165 M solution of H2CO3 (Ka1 is 4.3×10−7 and Ka2 is 5.6×10−11).
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...
Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11. What is the pH of a 0.47 M solution of carbonic acid?
A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3] = 1.000 M. Determine how much strong acid 1.00M HCI or strong base 1.000 M NaOH must be added to change the pH to 7.40. The step-wise acid dissociation constants for carbonic acid are Ka1= 4.2*10^-7 ; Ka2= 4.8*10^-11.
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×10-7 and Ka2 = 5.6 × 10-11.10)A) 10.44 B) 5.50 C) 4.31 D) 11.00 E) 3.56
Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of CO3 -2. Ka1 = 4.30 x 10-7 Ka2 = 5.59 x 10-11
In waters affected by acid rain the concentrations of the three carbonic acid species (H2CO3, HCO3-, CO32-) are determined by concentration of the strong acid deposited by acid rain, as well as the concentration of H2CO3 which is controlled by the solubility of carbon dioxide . Under these conditions (constant H2CO3 and relatively low pH) the only carbonic acid equilbrium of importance is the conjugate base reaction of HCO3-, which is related to, but not identical to - and not...