Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Use each of the two methods of buffer preparation to make a 1.0 M buffer with a 1:2 conjugate ratio (base:acid). Select the best answer from the dropdown for each method.
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- Method 1: Weak base + conjugate acid.
- How many moles of NH4NO3 should be added to a 100 mL solution of 1.0 M NH3 to achieve the desired concentration and conjugate ratio?
- Method 2: Weak base + strong acid.
- A solution of HCl is added to 100 mL of 2.0 M NH3. What concentration of HCl should be used to achieve the desired concentration and conjugate ratio in the buffer while only using 100 mL of strong acid?
- Method 1: Weak base + conjugate acid.
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- You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa 4.20) and 0.240 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: mL sodium benzoate: mLarrow_forwardA 1.451.45 L buffer solution consists of 0.1590.159 M butanoic acid and 0.3320.332 M sodium butanoate. Calculate the pH of the solution following the addition of 0.0620.062 moles of NaOHNaOH. Assume that any contribution of the NaOHNaOH to the volume of the solution is negligible. The ?aKa of butanoic acid is 1.52×10−51.52×10−5.arrow_forwardYou are in charge of making a Tris buffer at pH 7.5. You could start with solid Tris base as you did in lab, but you found stock solutions of 1.0M Tris base and 1.0M Tris Hydrochloride (the conjugate acid form) in the lab and decided to make the buffer with those. How much of each of the stock solutions would you mix together to make 200.0 mL of 1.0M Tris buffer at pH 7.5?arrow_forward
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