Question

Calculate the pH if 10.00mL of 2.00M HBr was added to the buffer from question 1.

leg(4.ox Io-) 1. . Determine the pH of 100.0mL, of a buffer costaining 0.200M HNO: and 0 200M KNO.. K, for HNOr is 4010 3, 398 CA H-3.398 log ~ 3,4 o.zoom 2. Calculate the pH if 30.00mL. of 0.150M NaOlHl was added to he teffe ftem O, 300L b 0.004500 0.00o 003 PH: 3.5 a 0.0255 o.oys 3. Calculate the pH if 10.00mL of 2.00M HBr was added to the buffer from question 1. b 0.0100 o, ooo 4-0.020o -.0o t 0.0100 4. Calculate the pH if 15.00mL of 2.00M HBr was added to the buffer from question 1

Answer 1

Here Henderson Hasselbalch equation is used to determine the pH of the reaction. HNO3 and KNO3 have NO3- ion and due to common ion effect the pH does not change much on addition of acid or base. Thus they act as Buffer solutions . Here, the change in numbet of moles at equilibrium is determinrd with the help of ICE table. I- initial C-change E- equilibrium. Here the concentration of acid and conjugate base is the same, so pH= pka

2. and 0 2 M KNO aj 乙一3.398 .