1. Write out the chemical equation for this buffer. Identify which species is the conjugate acid and which is the conjugate base. 2. For buffer 1 calculate the ratio of the base to acid using the Henderson-Hasselbach equation. 3a. Calculate the concentration of the conjugate acid and conjugate base in this buffer. (hint: the total concentration of this buffer is 0.2 M i.e. [acid] + [base] = 0.2 M) 3b. Using the Henderson-Hasselbach equation check that these ratios are correct.
Buffer 1 will be 100 ml of 0.2 M acetate buffer pH = 4.4
1. Write out the chemical equation for this buffer. Identify which species is the conjugate acid and which is the conjugate base.
2. For buffer 1 calculate the ratio of the base to acid using the Henderson-Hasselbach equation.
3a. Calculate the concentration of the conjugate acid and conjugate base in this buffer. (hint: the total concentration of this buffer is 0.2 M i.e. [acid] + [base] = 0.2 M)
3b. Using the Henderson-Hasselbach equation check that these ratios are correct.
4. What volume of 1 M acetic acid would you add to a beaker to get a final concentration of 0.2 M in 100 ml?
5. What volume of 1.0 M NaOH would you add to get the final concentration of the conjugate base that you calculated in part 3a in 100 ml?
6. Explain using chemical equations of the reactions taking place the chemistry behind the preparation of this buffer.
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