BufferDesired pHVolume addedBuffer capacitysolution0.10 M HCI0.10M NaoHAcid addedBase added13.0110.0350.06324.0110.0850.03936.0110.1670.0548.03.870.3879.500.4920.024669.00.08860.0886713.04.990.5Question: What is the most effective buffer against bases?

Buffer solution: A buffer solution is a solution that only changes slightly when an acid or a base…

Answered: Buffer Desired pH Volume added Buffer…

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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Question Completion Status: For Solution A, approximately how many mL of HCI were needed to exceed the buffering capacity of this solution? Enter the number only. Don't enter units as part of your answer and don't use commas or scientific notation. Titration curve of Solution A 14 13 12 11- 10 9 8 pH 7 6 5 4 3 2 1 5 4 3 2 1 HCI added (mL) 0 1 2 3 4 5 NaOH added (mL) 14 13 12- 11 10 9 8 pH 7 6.8 2 65 4 3 2 1 Titration curve of Solution B Click Save and Submit to save and submit. Click Save All Answers to save all answers. 54 32 1 HCI added (mL) 0123 NaOH added (mL)
Design a buffer that has a pH of 4.66 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 × 10-5 4.19 H2PO4- HPO42- 6.2 × 10-8 7.21 HCO3- CO32- 4.8 × 10-11 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams potassium salt of weak acid = grams potassium salt of conjugate base =
Pp
Which of the following will produce a buffer solution when mixed? 50.0 mL 0.500 M HNO3 + 50.0 mL 0.250 M CH3NH3CI 50.0 mL 0.250 M KOH + 50.0 mL 0.500 M CH3NH3CI 50.0 mL 0.500 M KOH + 50.0 mL 0.500 M CH3NH3CI 50.0 mL 0.500 M HNO3 + 50.0 mL 0.500 M CH3NH2
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH.
Interpret pH titration plots. Answer the following about the titration plot shown below, involving a monoprotic acid and base. 20 mL of 0.1M titrand titrated with 0.1M titrant. Data points at 1 mL increments. 14.0 12.0 10.0 5 8.0 6.0 4.0 2.0 0.0 seededood 0 0.0 10.0 مهمه 20.0 30.0 Volume of titrant (mL) (a) Is the species being titrated an acid or a base? (b) Is the species being titrated strong or weak? (c) What is the value of Ka (if a weak acid) or K, (if a weak base) for the species being titrated? If the species is strong (100% dissociated), enter 999. rààààààààà 40.0 50.0
From the following set of titrations choose the three most concordant titres and calculate the average titre value run 1 2 3 4 4 titre (ml) 13.40 13.70 13.85 13.45 13.80
Titration A HCl Titrated with NaOH Volume of NaOH pH 0.0 1.00 5.0 1.18 10.0 1.37 15.0 1.60 20.0 1.95 21.0 2.06 22.0 2.19 23.0 2.38 24.0 2.69 25.0 7.00 26.0 11.29 27.0 11.58 28.0 11.76 29.0 11.87 30.0 11.96 35.0 12.22 40.0 12.36 45.0 12.46 50.0 12.52 Titration B HC2H3O2 Titrated with NaOH Volume of NaOH pH 0.0 2.87 5.0 4.14 10.0 4.56 15.0 4.92 20.0 5.34 21.0 5.46 22.0 5.61 23.0 5.80 24.0 6.12 25.0 8.87 26.0 11.30 27.0 11.56 28.0 11.75 29.0 11.87 30.0 11.96 35.0 12.22 40.0 12.36 45.0 12.46 50.0 12.52 1. Titration A, endpoint pH = Titration B, endpoint pH = 2. pKa or pKb = 3. Ka or…
Determine the Ka value Solution 1 3.98 X 10-3 M Solution 2 6.03 X 10-4 M Solution 3 1.07 X 10-5 M Solution 4 1.05 X 10-5 M Solution 5 4.68 X 10-10 M
Based on the two graphs , draw conclusions regarding the buffer and water solutions ability to resist changes in pH after the addition of NaOH
A student obtains the following data from the Determining the pKa of an Acid-Base Indicator experiment. Using this data, calculate the pKa of the indicator in the fourth solution. Solution Abs. pH 3.4 + HCI 0.054 pH 4.6 + NaOH 0.564 Sample # 1 2 345 actual pH 3.34 3.73 3.96 4.22 4.50 Abs. 0.135 0.214 0.295 0.382 0.460

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Buffer Desired pH Volume added Buffer capacity solution 0.10 M HCI 0.10M NaoH Acid added Base added 1 3.0 1 1 0.035 0.063 2 4.0 1 1 0.085 0.039 3 6.0 1 1 0.167 0.05 4 8.0 3.87 0.387 5 9.50 0.492 0.0246 9.0 0.0886 0.0886 7 13.0 4.99 0.5 Question: What is the most effective buffer against bases?