This question concerns part 1 of this lab. You need to make a buffer solution by mixing both a weak acid and its conjugate base in the right proportions to achieve the desired pH. Your desired target pH is 4.20. You have been provided with 5.00 mL of 0.100 M sodium acetate solution. How many moles of acetic acid do you need to add to this solution to obtain a buffer solution at the desired pH? The pKa of acetic acid is 4.74.
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This question concerns part 1 of this lab.
You need to make a buffer solution by mixing both a weak acid and its conjugate base in the right proportions to achieve the desired pH.
Your desired target pH is 4.20. You have been provided with 5.00 mL of 0.100 M sodium acetate solution.
How many moles of acetic acid do you need to add to this solution to obtain a buffer solution at the desired pH? The pKa of acetic acid is 4.74.
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- 7 of 21 I Review | Constants | Periodic Table Part A You need to produce a buffer solution that has a pH of 5.21. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74. Express your answer numerically in millimoles. • View Available Hint(s) ΑΣφ mmol acetateFor this one, need the acid/ base tables in the book (Appendix E & F). Match each buffer system with the correct pH range the buffer maintains. Prompts Submitted Answers hypochlorous acid + sodium hypochlorite Choose a match formic acid + potassium formate 6.46-8.76 propionic acid + sodium propionate 2.77-4.77 4.76-6.76 3.89-5.89Compare the results of two experiments: First, a small amount of base is added to an unbuffered solution with a pH of 7. Second, the same amount of base is added to a buffered solution with a pH of 7.
- In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict the pH of the sample.c) Using…In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data. Method 1-TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint. Method 2 - pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8. A. Calculate the molarity of the acid using the titration data. B. If we assume that the titrated unknown is a strong acid, predict the pH of the sample. C.…In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 d) Based on your answer in a) and c), do you think the unknown is really a strong acid or is it a weak acid instead? Defend your answer in one sentence.e)…
- Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases 車 Conjugate Acid Name Formula 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 Ammonia NH3 CH;NH2 CH§NH2 CH;NH2 C;H;N NH,+ Methylamine Ethylamine Aniline Pyridine CH;NH;* CH$NH;* CH;NH;* C;H;NH 1.7 x 10-9 1. Compute the pOH of the buffer solution. (Write your answer in 1 decimal place).Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Name Formula Kb 1.8 x 10-5 Ammonia Methylamine NH3 CHÍNH, 4.38 x 10-4 C₂H5NH₂ 5.6 x 10-4 Ethylamine Aniline CHẠNH, 3.8 x 10-10 Pyridine CsHsN 1.7 x 10-⁹ 2. Compute for pKb Conjugate Acid NH4+ CH;NH * C₂H5NH3+ CH,NH,* CH,NH*3. You discovered a new diprotic acid (acid X). You want to characterize the pka's of acid X, so you perform a titration experiment. Your data are summarized in the table below. Your titration sample contains 150.0 mmol of acid X. Total amount NaOH added (mmol) 120.0 220.0 Determine the pka's of acid X. pH 2.905 7.055
- A buffer solution is prepared by combining 0.848 moles of formic acid and 0.719 moles of sodium formate. What will the solution pH be if 0.126 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places) Type your answer...A buffer solution is prepared by combining 0.795 moles of formic acid and 0.898 moles of sodium formate. What will the solution pH be if 0.120 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places)The pH of a solution made from a 0.75 M acetic acid solution and a 0.54 M sodium acetate solution is (K, = 1.8 x 10-5) Your Answer: Answer Question 7 1) Listen The pH of 300 mL solution made of 1.10 M acetic acid and 0.80 M potassium acetate is (Ka = 1.8 x 105) after the addition of 0.03 moles HCI Your Answer: Answer Question 8 1) Listen The pH of 300 mL solution made of 0.97 M acetic acid and 1.19 M potassium acetate is (Ką = 1.8 x 10-5) after the addition of 0.010 moles NaOH Your Answer: Answer