• The large container marked “DI water” • 1 M CH3COOH Record the pH of this...
• The large container marked “DI water”
• 1 M CH3COOH Record the pH of this solution for later use. (4.76)
• 1 M NaCH3COO
• Two (2) 600-mL beakers
Transfer 20 mL of CH3COOH to one of the empty beakers. Transfer 20 mL of NaCH3COO to the same empty beaker. Add 360 mL of DI water. (400 mL total in the beaker.) Record the pH of this solution for later use (4.76).
a. moles of CH3COOH in the buffer
b. moles of NaCH3COO in the buffer
c. calculation of buffer pH from the Henderson-Hasselbalch equation.
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• The large container marked “DI water”
• 1 M CH3COOH Record the pH of this...
you prepared your initial buffer by mixing 30 mL of CH3COOH, 10 mL of NaCH3COO, and...
you prepared your initial buffer by mixing 30 mL of CH3COOH, 10 mL of NaCH3COO, and 360 mL of DI water concertation is 3M for both. a)Predict pH b) using the Henderson-Hasselbalch equation to determine the pH c. Prediction of whether this new buffer solution have a higher buffering capacity towards HCl, or a lower buffering capacity towards HCl d. Prediction of whether this new buffer solution will have a higher buffering capacity towards NaOH, or a lower buffering capacity...
IV. Comparing Buffering Capacity A. pH of Pure Water i. Measure out 30.0 mL DI H2O...
IV. Comparing Buffering Capacity A. pH of Pure Water i. Measure out 30.0 mL DI H2O into a beaker. 1. Calculate the expected pH of pure water. pH ________ 2. Measured pH of pure water. pH ___3.88______ 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error __________ B. pH of Water and Strong Acid i. Measure out 30.0 mL DI H2O and 2.0...
The buffer solution is made of 50ml of 1.0M CH3COOH and 50ml of 1.0M NaCH3COO. Please...
The buffer solution is made of 50ml of 1.0M CH3COOH and 50ml of
1.0M NaCH3COO.
Please find the expected pH of the buffer after the addition of
the strong base, and the percent error between the expected pH and
the measured pH of the solution.
pH of Buffer after the addition of the Strong Base: ix. Measure out 50.0 mL the buffer in part D and 2.0 mL of 1.0 M NaOH into a clean beaker. X. Rinse the pH...
consider 100.0 ml of a buffer solution that contains [NaCH3COO]=[CH3COOH]=0.250 M a) what is the pH...
consider 100.0 ml of a buffer solution that contains [NaCH3COO]=[CH3COOH]=0.250 M a) what is the pH of this buffer? b) what should the ph of the buffer be after 50.0ml of water is added? explain c) wtite balanced net ionic for the reaction that occurs whrn 1.0 M HCl ir added to this buffer. d) after adding 10.0 ml of 1.0 M HCl what will the ph of the solution be? e) as more 1.0 M HCl is slowly added...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity t...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity to be higher, lower, or the same as the buffer you prepared in Part II of this lab? Be specific and use your data. c. Measure the pH of the Beaker #2 solution, via a pH meter, and record in data sheet. Part II: Dilute Buffer Solution In this section, the pH of a 0.25 M CH3CO2H - 0.25...
3.What happens to the pH of your buffer solution when you dilute it with DI water?...
3.What happens to the pH of your buffer solution when you dilute it with DI water? Why? How does this compare to the dilutions of the solution containing just acid or base? 7.Explain and justify when and why it is NOT appropriate to use the Henderson-Hasselbalch equation to calculate the pH of a solution. You should address both (1) what kinds of components should/should not be present, and (2) their relative concentrations.
Please help, I'm so confused!!!! This is due wednesday night!!! i'm gonna fail :(((( pH of...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
based on instructions please help me fill out chart Use appropriate safety precautions for working with...
based on instructions please help me fill out chart
Use appropriate safety precautions for working with concentrated acids and bases. This includes splash-proof goggles, long pants, and closed-toe shoes. No eating, drinking, or chewing at any time in the laboratory. Part I: Comparing the Behavior of the Buffer with Distilled Water 1. Obtain a pH meter or probe. Make sure beakers are clean and dry. 2. Place 25 mL of distilled, deionized water in a clean dry 100-ml beaker. 3....
check answers please thanks? vom voline SE 5: Buffers o n test effect of acid and...
check answers please thanks?
vom voline SE 5: Buffers o n test effect of acid and bases on the carbonic acid/sodium bicarbonate buffer system. ere will test et ou will need: 4 small beakers balance IM NaOH pH paper baking soda glass stirring rod 100 ml beaker seltzer water graduated cylinder IMHCI Prepare 50 mL of a butter containing 0.1M NaHCO. in carbonic acid. Use a source NaHCO, and seltzer water as a source of carbonic acid How much NaHCO,...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.5? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid Step 1: Rearrange the Henderson Hasselbalch...
The buffer solution is made of 50ml of 1.0M CH3COOH and 50ml of
1.0M NaCH3COO.
Please find the expected pH of the buffer after the addition of
the strong base, and the percent error between the expected pH and
the measured pH of the solution.
pH of Buffer after the addition of the Strong Base: ix. Measure out 50.0 mL the buffer in part D and 2.0 mL of 1.0 M NaOH into a clean beaker. X. Rinse the pH...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity to be higher, lower, or the same as the buffer you prepared in Part II of this lab? Be specific and use your data. c. Measure the pH of the Beaker #2 solution, via a pH meter, and record in data sheet. Part II: Dilute Buffer Solution In this section, the pH of a 0.25 M CH3CO2H - 0.25...
3.What happens to the pH of your buffer solution when you dilute it with DI water? Why? How does this compare to the dilutions of the solution containing just acid or base? 7.Explain and justify when and why it is NOT appropriate to use the Henderson-Hasselbalch equation to calculate the pH of a solution. You should address both (1) what kinds of components should/should not be present, and (2) their relative concentrations.
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
based on instructions please help me fill out chart
Use appropriate safety precautions for working with concentrated acids and bases. This includes splash-proof goggles, long pants, and closed-toe shoes. No eating, drinking, or chewing at any time in the laboratory. Part I: Comparing the Behavior of the Buffer with Distilled Water 1. Obtain a pH meter or probe. Make sure beakers are clean and dry. 2. Place 25 mL of distilled, deionized water in a clean dry 100-ml beaker. 3....
check answers please thanks?
vom voline SE 5: Buffers o n test effect of acid and bases on the carbonic acid/sodium bicarbonate buffer system. ere will test et ou will need: 4 small beakers balance IM NaOH pH paper baking soda glass stirring rod 100 ml beaker seltzer water graduated cylinder IMHCI Prepare 50 mL of a butter containing 0.1M NaHCO. in carbonic acid. Use a source NaHCO, and seltzer water as a source of carbonic acid How much NaHCO,...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.5? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid Step 1: Rearrange the Henderson Hasselbalch...
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