Exercise Write net-ionic equations for the reaction of the buffer mixture, Na,HP

Question

Exercise Write net-ionic equations for the reaction of the buffer mixture, Na,HPO4 with NaH PO4 1. a. with added H' ions: b. with added OH ions: 2. Write the formulas of the particles present in each of the following solutions. Then classify these particles as Bronsted-Lowry acids or bases. If more than one Bronsted-Lowry acid is present, list the strongest one first. Decide on which of the solutions below would show a buffer action. (A buffer must be able to react with both H and OH ions. Solute Particles present Bronsted base Bronsted acid Buffer (yes, or (capable in (capable in no?) reacting with reacting with H ions) OH ions) NHHSO4 NH3, NH CI HCL, NaCl NH CI, NaCl KHCO HC2H302 HCI H C204 KHS, Na2S 3. Show the setup. Calculate the pH of an equimolar mixture of H2S and NaHS. Kal for HS is 1.1 x107 Setup: Answer

Explanation / Answer

ANSWER:

In the buffer mixture of NaH2PO4 and Na2HPO4,  NaH2PO4 acts as acid and reacts with OH- and Na2HPO4 acts as base and reacts witt H+. Na2HPO4 dissociates as:

Na2HPO4 -------> 2 Na+ + HPO42-

(i) Reaction of 2 Na+ + HPO42- (Na2HPO4) with H+

2 Na+ + HPO42- + H+ --------------> 2Na+ + H2PO4-

Net ionic equation :   HPO42- + H+ -------------->   H2PO4-

(ii) Similarly NaH2PO4 react with OH-

NaH2PO4 dissociates as:

NaH2PO4 ------------ Na+ + H2PO4-

Na+ + H2PO4- + OH- ---------> Na+ + HPO42- + H2O

Net ionic equation:  H2PO4- + OH- --------->  HPO42- + H2O

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