I am not sure how to approach this question I think I have the correct answer...
I am not sure how to approach this question I think I have the correct answer for number 1 but I am not exactly sure how to apply it to number 2 if number 1 is correct.
1. What is the best range of buffering that is provided when a weak acid is present in a water solution?
the best range of buffering that is provided when a weak acid is present in a water solution is a pH of about 5 to 7.
2.* What is the ratio of conjugate base to weak acid at the ends of this range? Use the Henderson-Hasselbach equation to show how you obtained your ratios.
You should be able to calculate this ratio at plus or minus 2, 3, 4 pH units from the pKa value. Remember you are using a log scale (pH) and powers of 10 in concentration as you go up or down the pH scale.
Homework Answers
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I am not sure how to approach this question I think I have the
correct answer...
please help walk me through how to solve these, the questions change everytime. i am not...
please help walk me through how to solve these, the questions
change everytime. i am not even sure where to start. thank
you
HON WILL UNULNEM TULENERAL CHEMISTRY LABE Amber Gloria's Qula History Lab & Quiz Exploring Buffers Background Incorrect Question 3 0/1 pts If you mix a weak acid and a weak base together with concentrations of 0.33 and the acid has apk, -8.58, what is the pH of the buffer? Give your answer to two decimals. pH =...
Hello, I will try this again I am trying to prepare a buffer from a solution...
Hello, I will try this again I am trying to prepare a buffer from a solution of a weak acid. This is for part D. of Experiment 25 - Ph Measurements - buffers and their properties I am to be give an 0.50 M solution of weak acid with a given pKa, and I will preparre a buffer of a desired pH measurement (choose any pH) I must first dilute the acid solution to 0.10 M by adding 10 ml...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...
i need to find the ratio of B- and HB to create a ph level of...
i
need to find the ratio of B- and HB to create a ph level of 11
using the pka found in part 1 and 2 of question c. what equation
would i use to fibd the ratio and the volume?
5. Preparation of Buffer Target pH to be prepared pK, from C.1 and C.2 Show calculation of B)/(HB) ratio needed: Ratio [B]/[HB) needed: Volumes used to create above ratio: ml. HB ml phl of prepared buffer c. Some Properties...
NOTE: I know the answer to this problem is 13.0 but I am unsure how to...
NOTE: I know the answer to this problem is 13.0 but I am unsure how to get the answer. A weak acid has a pKa of 7.3. 30 mL of 1.0 M NaOH is added to 100 mL of a 1.0 M buffer of this acid at pH 8.0. The resulting solution is at pH:
In the titration of 25.0 mL of 0.1 M CH3COOH with 0.1 M NaOH, how is...
In the titration of 25.0 mL of 0.1 M CH3COOH with 0.1 M NaOH, how is the pH calculated before the titrant is added? The pH is calculated by determining the concentration of excess hydroxide ions in the solution, subtracting pOH from 14, and taking the negative log of the result. The pH is 14. The pH is 7. The pH is calculated using the H-H equation for a buffer solution, using the ratio of the concentrations of the base...
Please make sure parts e and f are correct, I have gotten two wrong answers so...
Please make sure parts e and f are correct, I have gotten two
wrong answers so far. Thanks. Will give thumbs up. Please show
work.
Here is a list of hypothetical acids with their pKa's. The pKa values are valid at 25 °C. Acid pK a А 3.44 B 5.12 с 6.40 D 8.52 d. Which of these acids, in combination with its conjugate base, would be the best one to use to create a buffer with a pH of...
I have a chem final next week and I have a question I am stuck on....
I have a chem final next week and I have a question I am stuck on. If you solve, please explain the steps. I will 'like' your response. Thanks in advance! 1. Calculate how many mL of 0.10M KOH must be added to 100.0mL of 0.20M formic acid solution to make a pH = 3.50 buffer. pKa(HCOOH) = 3.74 I keep getting 115mL by plugging in all given info to the equation pH=pka+log(b/a) and solving for x then converting to...
I need help with the problem in the last photo.. I thought I’d post my lab...
I need help with the problem in the last photo.. I thought I’d
post my lab explanation and data if that helps you get a better
understanding, but it’s just the question at the end. I know I need
to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log(
[acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how
do I find the concentrations to put in the log fraction?
Thanks, in advance!
Learning Objectives: 1....
I can't figure out how to find the concentration of the conjugate base. Question 2 If...
I
can't figure out how to find the concentration of the conjugate
base.
Question 2 If a 50.00 mL sample of 0.132 M ammonium chloride is titrated with 21.47 mL of 0.149 M NaOH, what is the pH of the titration mixture? (For NH4CI, Ka = 5.75 x 10-10, Selected Answer: 2 Correct Answer: 9.21 +0.02 Response This is in the buffered region of the titration. Therefore, calculate the moles of weak acid initially present and the Feedback: moles of...
please help walk me through how to solve these, the questions
change everytime. i am not even sure where to start. thank
you
HON WILL UNULNEM TULENERAL CHEMISTRY LABE Amber Gloria's Qula History Lab & Quiz Exploring Buffers Background Incorrect Question 3 0/1 pts If you mix a weak acid and a weak base together with concentrations of 0.33 and the acid has apk, -8.58, what is the pH of the buffer? Give your answer to two decimals. pH =...
i
need to find the ratio of B- and HB to create a ph level of 11
using the pka found in part 1 and 2 of question c. what equation
would i use to fibd the ratio and the volume?
5. Preparation of Buffer Target pH to be prepared pK, from C.1 and C.2 Show calculation of B)/(HB) ratio needed: Ratio [B]/[HB) needed: Volumes used to create above ratio: ml. HB ml phl of prepared buffer c. Some Properties...
Please make sure parts e and f are correct, I have gotten two
wrong answers so far. Thanks. Will give thumbs up. Please show
work.
Here is a list of hypothetical acids with their pKa's. The pKa values are valid at 25 °C. Acid pK a А 3.44 B 5.12 с 6.40 D 8.52 d. Which of these acids, in combination with its conjugate base, would be the best one to use to create a buffer with a pH of...
I need help with the problem in the last photo.. I thought I’d
post my lab explanation and data if that helps you get a better
understanding, but it’s just the question at the end. I know I need
to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log(
[acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how
do I find the concentrations to put in the log fraction?
Thanks, in advance!
Learning Objectives: 1....
I
can't figure out how to find the concentration of the conjugate
base.
Question 2 If a 50.00 mL sample of 0.132 M ammonium chloride is titrated with 21.47 mL of 0.149 M NaOH, what is the pH of the titration mixture? (For NH4CI, Ka = 5.75 x 10-10, Selected Answer: 2 Correct Answer: 9.21 +0.02 Response This is in the buffered region of the titration. Therefore, calculate the moles of weak acid initially present and the Feedback: moles of...
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