Use the following data to calculate the Ka of carbonic acid at 253 K. H2CO3 (aq)...
Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <-> HCO3 (aq) + H3O . Ka1= 4.3x10^-7 . Ka2= 4.7x10^-11 a. if you add NaHCO3 to the solution, would the pH of the solution go up, down, or stay the same? b. Calculate the pH of the solution if you added 3.4 x10^-3 M NaHCO3.
A) Calculate the concentration of HCO3- in an aqueous solution of 2.68×10-2 M carbonic acid, H2CO3 (aq). [HCO3-] = ___ M. B) Calculate the concentration of C6H6O62- in an aqueous solution of 0.0818 M ascorbic acid, H2C6H6O6 (aq). [C6H6O62-] = ___ M.
Using the thermodynamic data provided below, calculate Ka2 for H2CO3(aq) at 25° H*(aq) H:CO3(aq) HCO3 (aq) CO3(aq) AH° (kJ/mol S (J/K mol) 0 0 -698.7 191 -691.11 95.0 -676.26 -53.1 Multiple Choice 4.3910-9 459-10-11 459-10-10 None of the above 409-10-11
Using the thermodynamic data provided below, calculate Ka2 for H2CO3(aq) at 25° H*(aq) H:CO3(aq) HCO3 (aq) CO3(aq) AH° (kJ/mol S (J/K mol) 0 0 -698.7 191 -691.11 95.0 -676.26 -53.1 Multiple Choice 4.3910-9 459-10-11 459-10-10 None of the above 409-10-11
Carbonic acid (H2CO3) is unstable in water and rapidly decomposes i to CO2(g) and H2O(l). Consequently, the reaction between Coc-H+(aq) and HCO3-(aq) is better represented as
Calculate the concentration of CO32- in an aqueous solution of 0.249 M carbonic acid, H2CO3 (aq). [CO32-] = M.
Calculate the percent ionization of carbonic acid (H2CO3) in solutions of each of the following concentrations (Ka = 4.3e-07.) (a) 0.193 M (b) 0.371 M (c) 0.783 M
The acid dissociation constant K, of carbonic acid (H2CO3) is 4.5x 10-7. Calculate the pH of a 4.2 M solution of carbonic acid. Round your answer to 1 decimal place. PH = 0 x 5 ?
The pH of a 0.19 M solution of carbonic acid (H2CO3) is measured to be 3.53. Calculate the acid dissociation constant K, of carbonic acid. Round your answer to 2 significant digits. K = 1) x 6 ?
Question 1 (1 marks) Tron (II) sulfide can react with carbonic acid, H2CO3, according to the reaction shown. 2 FeS (s) + H2CO3 (aq) + 2 FeO (s) + 1/n (CH2O)n (aq) + 2 S (s) NO a) Calculate the mass (g) of iron (II) oxide produced when 10.20 g iron (II) sulfide and 1.450 mol carbonic acid are reacted. The reaction results in a 87.5 % yield of product formed. b) If the carbon containing product has a molar...