How would you create a buffer solution at a pH of your choosing (between pH 4-6) by adding solid sodium acetate to 50mL of 0.1M acetic acid? Use the Henderson-Hasselbalch equation to calculate the mass of sodium acetate that you will need to produce this acetate buffer (K, = 1.75 x 10-5). Make a note of your chosen pH and the mass of sodium acetate that you will need in part 4 in the "procedure and data" section before turning in your pre-lab assignment. %3D

How would you create a buffer solution at a pH of your choosing (between pH 4-6) by adding solid sodium acetate to 50mL of 0.1M acetic acid? Use the Henderson-Hasselbalch equation to calculate the mass of sodium acetate that you will need to produce this acetate buffer (K, = 1.75 x 10-5). Make a note of your chosen pH and the mass of sodium acetate that you will need in part 4 in the "procedure and data" section before turning in your pre-lab assignment. %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Answer the following questions about a titration between 25.0 mL of a weak base (Kb= 6.9*10-5) and 0.100 M hydrochloric acid). A.What is the concentration of the weak base solution if it requires 37.50 mL of the HCl solution to reach the equivalence point (assume 1:1 stoichiometry)? B.What is the initial pH of the weak base solution before any HCl is added? C.What is the pH of the titration at the equivalence point? D.The pKa of ethyl red is ~ 5.4 and the pKa of thymol ~ 8.4. Which indicator would be best to use in the titration?
Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of 1 M sodium acetate added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.
11) A 520 ml solution contains 0.130 M formic acid (K, = 1.80 x 10) and 0.130 M sodium formate. First determine the pH of this initial solution. Next, determine the pH if 1 mL of 5.5 M of HCI was added to this solution. Finally, determine if rather than HCI, 1 mL of 5.5 M NaOH was added to the solution.
The pH of a saturated solution of metal hydroxide, Me(OH)2, is 12.4 at room temperature. Calculate the Ksp for the compound. Round off your answer to 3 sig. figs. Reaction: Me(OH)2 ↔ Me2+ + 2 OH-.
MISSED THIS? Read Section 18.4 (Page); Watch KCV 18.4B. Consider the curve shown here for the titration of a weak monoprotic acid with a strong base. Hd 14 12 10 8 6420 80 120 160 40 Volume of base added (mL) The figure shows pH as a function of volume of base added. The pH is measured from 0 to 14 on the y-axis, while the volume of base added is measured from 0 to 160 milliliters on the x-axis. The curve of the plot goes up gradually from pH 2.3 at 0 milliliters to pH 5.8 at 49 milliliters, next the plot goes up steeply to pH 11.8 at 51 milliliters, and finally the plot goes up gradually to pH 12.2 at 160 milliliters. ✓ Correct An equilibrium problem based on the initial concentration and Ka of a weak acid should be solved for aqueous solution of the weak acid. This is true for the initial state of titration, when no base has been addition of a small amount of a strong base turns this solution into a buffer whose pH is calculated in way. Part D At what volume of added base does pH =…
8. Often, the solubility of organic molecules can be influenced by changing the pH of a solution. Below are drawings of two dyes, Sudan Blue and Sudan Orange, at different pHs. Fill in the table to indicate if the dye will be soluble in dichloromethane (DCM) or water under each condition. pH = 12 pH = 7 `ΝΗ Ο Sudan Blue ΝΗ pH = 2 `ΝΗ Ο ΝΗ Sudan Blue NH, O NH₂ Sudan Blue Sudan Orange OH Sudan Orange OH Sudan Orange OH OH pH = 12 pH = 7 pH = 2 Sudan Blue Sudan Orange
What is the effective pH range for a sodium acetate/acetic acid buffer? Ka = 1.80 x 105. %3D Enter your answer to three decimals. to
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 5 pH = 6 pH = 8 O yes Ba(OH), O no do O yes CuBr O no O yes AgCN O no Explanation Check Rights Reserved Terms of Use Privacy Accessibility O 10:00 O oo o0
24. How many moles of NH,Br must be added to 2 L of 0.1 M NH,OH to form a buffer whose pH is 9.00? (K, of NH,OH = 1.76 x 0*)
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 2 pH = 3 pH = 5 O yes BaCO, dlo O no O yes Cal, O no O yes Ni(OH), O no Check Terms of Use Privacy Explanation 2021 McGraw-Hill Education. All R V 1 10: Ocer