Is H2CO3 not an amphiprotic because it can only donate H+? But HCO3- is amphiprotic cause...
My professor explained that Not all polyprotic acids are amphiprotic because for instance, the second H of H2SO4 doesn’t come off strongly like the first H. However, this explanation doesn’t explain the reason why H2SO4 is not amphiprotic to me. To me, H2SO4 cannot accept a H+, but can donate a H, which is the reason why it’s not an amphiprotic. In contrast, H2PO4- is amphiprotic because it can accept a H+ to become H3PO4 and also donate a H...
For the reaction H+(aq) + HCO3-(aq) ↔ H2CO3(aq), if the reaction is at equilibrium, which conditions must be maintained? A. [H2CO3] > [H+][HCO3-] B. [H2CO3] < [H+][HCO3-] C. [H2CO3] = [H+][HCO3-] D. none of the above
What is the conjugate acid of CO3? 2- HC02 . H2CO3 HCO3 Co22- none of the above 2
Consider a solution consisting of the following two buffer systems: H2CO3 HCO3– + H+ pKa = 6.4 H2PO4– HPO42– + H+ pKa = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present? ***Please explain why the right answer is right and why the other ones are wrong. a. [H2CO3] > [HCO3- ] and [H2PO4- ] > [HPO42- ] b. [HCO3- ] > [H2CO3] and [HPO42- ] > [H2PO4-...
The following questions is based on ionization of carbonic acid. [H2CO3 = H+ + HCO3- K1 = 4.7 X 10-7, pK1 = 6.34 ] [HCO3- = H+ CO3-2 K2 = 4.4 X 10-11, pK2 = 10.36] Calculate the pH ofthe solution form by mixing the following: a)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.050 M NaOH . b)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.150 M NaOH . c)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.100 M...
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
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
please answ all questions
The chemical formula for carbonate is H2CO3 нсоз HCO3- CO3- Co2 QUESTION What is the pH of a solution that is 1 molar [H+ -7 7 -3 3 -1 QUESTION 10 The average concentration of C02 in the atmosphere today is approximately. 300 ppm 330 ppm 380 ppm 420 ppm Click Save and Submit to save and submit. Click Save All Answers to save all an
For each of the four, specify whether the substance can act as a/an... (1) acid in aq. solutions, (2) base in aqueous solutions, and (3) amphiprotic species in aqueous solution? Note: An amphiprotic substance can donate protons (act as Bronsted acid) or accept protons (act as Bronsted base). H3SO4+ H2SO4 HSO4- SO42-