PART 1. Write net-ionic ic equations for the reaction of the buffer misxture, Na

Question

PART 1. Write net-ionic ic equations for the reaction of the buffer misxture, NaJHPOs with NalH,PO4 for 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 Bronsted base Bronsted acid Buffer (yes, or (capable in reacting with reacting with H ions) present l (capable in no?) OH ions) NH4HSO4 NHj. NE HC1, NaCI NH4CI, NaCI H2CO, KHCO HCI H2C204 KHC KHS NazS 3. Calculate the ph of an equimolar mixture of HS and Nalls. Show the setup. Kal for H2S is 1.1 x10 Setup: Answer

Explanation / Answer

Q1

this is a buffer so there is conjugate acid and conjguate bases

they are amphoteric, so they can act as acid or bases

Na2HPO4 = 2Na+ + HPO4-2

NaH2PO4 = Na+ + H2PO4-

a)

H+ addition:

HPO4-2 + H+ = H2PO4-

b)

OH-

H2PO4- + OH- = H2O + HPO4-

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