The question is attached.
Starting with equation (8.5) show that the maximum buffer capacity occur at pH=pKa.
The units of buffer capacity are mol L^-1. As a consequence of the definitions, buffer capacity is always a positive quantity. For a monoprotic acid the buffer capacity (as a function of pH) is given by: (see attach
What is the effect on pH when a buffer is diluted by a factor of 10?
a. The buffer pH does not change appreciably
b. The buffer pH increases by 1
c. The buffer pH decreases by 1
d. The buffer pH increases by 10
e. The change is dependent on Ka of the acid
A step by step method to prepare a buffer with a specific pH and concentration is given. This includes guidelines to find the conjugate acid/base pair, calculation of the buffer ratio using the Henderson-Hasselbalch equation, and the determination of mass of chemicals reagents required to prepare the buffer.
You want a solution that will buffer the addition of either 10 micromoles of acid or 10 micromoles of base. Total buffer concentration is equal to the concentration of the acid plus the concentration of salt of the acid. Which of the following buffers would you use if you wanted to buffer a solution at pH=6.9?
a) buffer A w
1) A buffer is prepared by adding 0.200 mol of sodium lactate ( NaC3H5O3) to 500ml of 0.5 M lactic acid ( Ka = 1.4 x 10^-4).
A) What is the pH of the buffered solution?
B) What is the pH after 100ml of 0.100 M HCL is added to the buffer?
C) What is the pH after 12 g of NaOH is added to the original solution prepared in
1.00L buffer solution contains 0.100M acetic acid and 0.100M sodium acetate. The ka of acetic acid is 1.8*10^-5. Calculate the pH of this buffer solution after the addition of 0.010 moles of solid sodium hydroxide to the buffer
(a) Calculate the pH of the 0.20 M NH3/0.18 M NH4Cl buffer.
for this part i got the wrong anwser of 9.21 so im not sure how to even begin part b
(b) What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 70.0 mL of the buffer?
Could you please show me in detail how to do this?
1. Choose an appropriate weak acid from the list below to make 0.25 liter of a 0.1M buffer solution that has a pH of 4.7:
AVAILABLE WEAK ACIDS:
Acetic acid (Ka = 1.8 x 10⁻⁵)
Citric acid (Ka = 8.4 x 10⁻⁴)
Benzoic acid (Ka =