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Henderson Hasselbalch Equation: Buffer Calculations

Related Topics

Wize High School Grade 12 Chemistry Textbook > Acids and Bases

Buffers

2 Activities

Consider 500 mL of a sodium acetate/acetic acid buffer in which the concentration of sodium acetate is 0.50 M and that of acetic acid is 0.10 M. (Ka acetic acid= 1.8×10-5)

(a) What is the initial pH of the buffer?

(b) What is the pH after 100 mL of 0.10 M NaOH is added?

(c) What is the pH after 100 mL of 0.10 M HCl is added?

More Buffers Questions:
Consider the following diagrams representing different buffer solutions:
Which of these buffer solutions has the highest acid AND base buffer capacities?
Buffer Problem
What is the pH of the buffer that has 0.81M of CH3COOH and 0.21M CH3COO-? KCH3COOH=1.8x10^-5
Now if we added 0.14M of HCl what is the new pH of the buffer? (ICE table since we need to consider the values at EQUILIBRIUM to find the pH)
Buffer Solutions
Which of the following solutions can rightfully be called a buffer solution?
Let us compare two buffer solutions that you could make from an aqueous solution of the weak acid, HA (aq). In both cases, you start from an identical initial solution. In both buffers, the target buffer ratio is 1A–: 2HA.