Given mixture is an example for acidic buffer,
pH=pka+log(moles of salt/moles of acid)
Addition of strong acid reacts with acidic buffer , salt reacts with added acid to form acid
NaC7H5O2 +HA <--> HC7H5O2 + NaA
Added base reacts with acid and forms salt
HC7H5O2 + NaOH <-----> NaC7H5O2 +H2O
pKa=-logka=-log(6.3x10^-5)= 4.20
pH= 4.20+log(0.06x3/0.02x1)
=4.2+log(0.18/0.02)
=4.2+log(9)
=4.2+0.95
pH= 5.15
QUESTION #1 What is the pH of a buffer by mixing 1.00L of 0.020M benzoic acid, HC,H,O2, with 3.00L of 0.060M sodiu...
What is the pH of a buffer solution made by mixing 0.1 M benzoic acid and 0.15 M of its conjugate base, sodium benzoate. Ka = 6.5x10-5 for benzoic acid.
* 2. Calculate the pH of a buffer solution that is 0.050 M in benzoic acid (HC,H,O,) and 0.150 M in sodium benzoate (NaC,H,O,). For benzoic acid, K = 6.5 X10. Use the Henderson-Hasselbalch approach. (6 points) Equation: HC,H,02(aq) + H20(1) = H,0*(aq) + C,H,O, (aq) Hint: pH = pKa + log base] (acid]
A buffered solution with pH of 4.4 is made of 0.1 M Benzoic acid, HC-HOs, and 0.15 M Sodium benzoate, NaC;HO2. After an addition of 1.5 mLs of 6.0 M HCI to 250 mLs of the buffered solution, what is the resulting pH? Ka 6.6 x 10
a buffer solution is 0.050 in benzoic acid and 0.150 M sodium benzoate. For benzoic acid Ka =6.5E-5. a.) the acid and base components of the buffers are_____and_______, respectively. b.) based on the information provided on the previous question, the pH of the buffer solution is given by:
A buffer solution is prepared by dissolving 1.49 g each of benzoic acid, C6H3CO2H, and sodium benzoate, NaC6H; CO2, in 150.0 mL of solution. ( Ka for benzoic acid is 6.3 x 10-5.) a. What is the pH of this buffer solution? pH = b. Which buffer component must be added, and in what quantity, to change the pH to 4.00? e must be added. Quantity = c. What quantity of 2.0 M NaOH or 2.0 M HCI must be...
What mass of sodium benzoate should you add to 150.0 mL of a 0.14 molL−1 benzoic acid solution to obtain a buffer with a pH of 4.25? For benzoic acid, Ka=6.3×10−5.
Consider the buffer system composed of benzoic acid, HC,H,O, and its conjugate base benzoate, CHO HC,H,O, + H2O = H,0+ + C,H,Oz Using Le Châtelier's principle, predict how the concentration of each substance changes by the addition of H,0+. Does the concentration of HC,H,O, increase or decrease when He is added? O decrease O increase Does the concentration of C,H,O, increase or decrease when H, is added? O increase decrease Does the concentration of H, 0* change significantly when H,O+...
I know how to do the question, but at the very end, how do you know if it's a buffer or not? What is the formula or rule to tell if something is a buffer or not? UBC Chem 123 Acid-Base Examples 20: Calculate the pH if 10.0 mL of 0.020 M benzoic acid is added to 40.0 mL of 0.004 M sodium benzoate. The pka of benzoic acid is 4.20. H₂O ² HA + benzoic acil - H₂ot +...
2. What is the pH of a buffer solution that is 0.10 M Benzoic acid, HC.HO, and 0.15 M sodium benzoate. Ka = 6.6 x 10% Page 1
Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONa). (Ka = 6.5 x 10-5 for benzoic acid)