Question

Submit for Grading Current Tº Close Problem Tutored Practice Problem 17-24 Use the Henderson-Hasselbalch equation to calculate ph of a buffer solution. Using the Henderson-Hasselbalch equation, calculate the ph of a buffer solution that is 0.345 Min HCO,' and 0.300 M in co, Check Submit Auer Show Approach Adding Acid or Base to Buffer It is a common misconception that buffer pll remains constant when some strong acid or base is added. This is not the case. As shows in the following emple problem, a buffer is the pll change upon addition of a strong acid or base because only the weak acid conjugate base ratio of the buffer is affected. The pH changes, but only by a small amount MacBook Air

Answer 1

Concentration of HCO3- = 0.345M

concentration of CO3-2 = 0.300M

Ka of HCO3- = 4.8 x10^-11

Ka= 4.8x10^-11

-log(Ka) = -log(4.8x10^-11)

PKa = 10.32

PH = PKa + log[salt]/[acid]

PH = 10.32 + log( 0.300/0.345)

PH = 10.26