Question

1. Write the equations for the reaction of the following Bronsted acids with water:

(a) H2S (b) HC2O4-  (c) HSO3-

2. Write equations for the reactions of the following Bronsted bases with water:

(a) PO4 3- (b) N2H4 (c) H2C6H5O7-

3. In each of the following questions, assume that there is no volume change when HCl is added to water in part (a) or the phosphate buffer in part (c).

(a) Calculate the pH when 0.129 moles of HCl are added to 1.000 liter of water.

(b) What is the difference between the pH of pure water (pH 7.00) and the pH of the solution after HCl was added?

(c) Calculate the pH when 0.129 moles of HCl are added to 1.000 liters of a buffer containing 0.421 M KH2PO4 and 0.443 M K2HPO4.

(d) The pH before the HCl was added is equal to 7.230. What is the difference between the pH before adding the HCl and after adding the HCl?

Answer 1

Bronsted acid is a proton donar in aqueous solution. a Hes (aq) + H2O lag Htay + H5 Cag) 6) HG20qCag) at Heo and Hag) + C204 (a) HSO3 Car & H₂O Cay H@D + Sosa Boonsted base is a proton acceptor in aqueous solution, 3- a Pou AD + Heolag - Holland + ohrago 6) Nell4C99) + H2Ocaq Netts a tortas e He CG Hof (a) theo (aq) + H₂ CG hs of (ag) + OHC