The 100. mL of buffer solution contains 0.08 M benzonic acid and 0.06 M sodium benzoate. What is the resulting pH when 15.0 mL of 0.2 M NaOH is added to the buffer? Кас н соон = 6.46 x 10-5 pH after strong base added = [?]

The 100. mL of buffer solution contains 0.08 M benzonic acid and 0.06 M sodium benzoate. What is the resulting pH when 15.0 mL of 0.2 M NaOH is added to the buffer? Кас н соон = 6.46 x 10-5 pH after strong base added = [?]

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...

See similar textbooks

Related questions

Q: Which of the following aqueous solutions are good buffer systems? O0.28 M ammonia + 0.32 M ammonium…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: A buffer solution contains 0.205 M NaHSO3 and 0.405 M K₂SO3. If 0.0321 moles of nitric acid are…

Q: A buffer solution contains 0.347 M C6H5NH3 Br and 0.336 M C6H5NH2 (aniline). Determine the pH change…

A: Pkb = -log(kb) = - log(7.4×10-10 ) Pkb = 9.13

Q: A 0.7026 g sample of an unknown acid requires 40.96 mL of 0.1158 M NaOH for neutralization to a…

A: Answer: To find out the molar mass of unknown acid it is being titrated against certain quantity of…

Q: 10) You make a solution that has a final concentration of 0.400 M acetic acid and 0.350 M sodium…

Q: in an experiment, the molecular formula for calcium hydroxide was determined to be Ca(OH)2. In this…

A: Given that : The mass of Ca = 0.050 g The volume of DI water = 150 mL The molarity of HCl = 0.30 M

Q: How many grams of solid potassium acetate should be added to 1.50 L of a 0.283 M acetic acid…

Q: What are the molar concentrations of acetic acid (CH,COOH) and sodium acetate (CH, COONA) in an…

Q: The second buffer you will make in lab, Buffer B, will be made by combining the appropriate amounts…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Which of the following aqueous solutions are good buffer systems? . 0.10 M hydrocyanic acid + 0.13 M…

A: A good buffer is prepared by dissolving or mixing a weak acid with its conjugate base or a weak base…

Q: Part C For 260.0 mL of a buffer solution that is 0.2922 M in CH3 CH,NH, and 0.2677 Min CH3CH2NH3CI,…

A: The buffer solution contains C2H5NH2 (weak base) and C2H5NH3Cl (salt of strong acid and weak base).…

Q: A chemistry graduate student is given 100. mL of a 1.20M ammonia (NH solution. Ammonia is a weak…

A: 31 gm of NH4Br added to NH3 to make a buffer solution of desired pH.

Q: A student must make a buffer solution with a pH of 4.50. Determine which weak acid is the best…

A: Concept: Buffer solution: A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is…

Q: Solutions Solution A: Solution B: Solution C: Solution D: 0.565 M HOCI 0.376 M HC1O4 0.817 M HCO₂H…

A: Buffer solution: It is a solution that can resist changes in pH when small amounts of acid or base…

Q: 1. 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: Since you have posted multiple questions, we are entitled to answer the first only. 1) Given:…

Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and…

A: Let y mL benzoic acid and (100 – y) mL sodium benzoate are mixed. For acidic buffer solution, pH =…

Q: Consider the titration of a 26.0 -mL sample of 0.180 M CH,NH2 with 0.150 M HBr. Determine each of…

A: pH is used to identify acidity and basicity of an aqueous solution. It is the negative logarithm of…

Q: Which of the following aqueous solutions are good buffer systems? 0.26 M ammonia + 0.37 M calcium…

Q: What is the pH of the buffered created by dissolving 60.0g HCN (MM= 27.0253 g/mol) and 60.0g KCN…

A: The PH can be calculated as follows

Q: A buffer solution contains 0.236 M C6H5 NH3 Br and 0.470 M C6 H5NH2 (aniline). Determine the pH…

A: The objective of the question is to determine the pH change.The value of for aniline is .The is…

Q: Consider the titration of 50.0 mL of 0.326 M weak base B (Kb = 7.5 x 10⁻⁶) with 0.340 M HNO₃. What…

A: we have to calculate the pH and identify the primary species in solution

Q: Calculate pH of a weak acid/conjugate base buffer solution. Calculate the pH of 550. mL of a 0.394-M…

A: The acid (say HA) dissociates in water to produce corresponding ion and hydronium ions. HA…

Q: A buffer system is prepared by combining 0.506 moles of ammonium chloride (NH4CI) and 0.720 moles of…

A: we have to calculate the pH of the buffer solution

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH),…

Q: 2. You wish to prepare a buffer containing acetic acid and sodium acetate with a total acetic acid…

A: pH of the buffer solution = 5.5 Concentration of the buffer = 450 mM = 0.450 M Volume = 1.5 L Ka of…

Q: A buffer solution contains 0.294 M NH4Cl and 0.388 M NH3 (ammonia). Determine the pH change when…

A: pH of a buffer is calculated using Henderson-Hasselbach equation which is expressed as pH = pKb…

Q: A buffer solution contains 0.327 M NH4Cl and 0.318 M NH3 (ammonia). Determine the pH change when…

Q: The pH of a bicarbonate-carbonic acid buffer is 5.52. Calculate the ratio of the concentration of…

A: The pH of the bicarbonate-carbonic acid buffer = The of carbonic acid at…

Q: Benzoic acid (let’s call it HA) has Ka = 6.3 × 10−5 and pKa = 4.20. A buffer with [HA] = 0.100 M and…

A: Given data,pKa=4.20[HA]=0.10M[A-]=0.063MMolarity of NaOH=0.10MVolume of NaOH=20.0mL=0.02LVolume of…

Q: A buffer solution is prepared which is 0.160 M both in acetic acid and in sodium acetate. Ka = 1.8 x…

A: Given, Molarity of acetic acid and sodium acetate = 0.160 M. Volume of buffer = 14.0 mL Ka (acetic…

Q: Which of the following aqueous solutions are good buffer systems? 0.30 M ammonia- 0.39 M ammonium…

A: The buffer system is a solution that resists the change in pH when acids or bases are added. This…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

The 100. mL of buffer solution contains
0.08 M benzonic acid and 0.06 M sodium
benzoate.
What is the resulting pH when 15.0 mL of
0.2 M NaOH is added to the buffer?
KaCH₂COOH = 6.46 x 10-5
pH after strong base added = [?]
pH of Soln w/ Base
Enter

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step by step

Solved in 4 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A buffer solution contains 0.332 M NH Br and 0.437 M NH3 (ammonia). Determine the pH change when 0.128 mol HC1O4 is added to 1.00 L of the buffer. (Assume K, (NH3) = 1.8 x 10-5.) pH after addition - pH before addition - pH change=
A buffer solution contains 0.396MCH, NH, Br and 0.266MCH, NH, (methylamine). Determine the pH change when 0.063mol NaOH is added to 1.00% of the buffer. pH after addition -pH before addition pH change = A buffer solution contains 0.396 M CH3NH3Br and 0.266 M CH3NH2 (methylamine). Determine the pH change when 0.063 mol NaOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change: =
A chemistry graduate student is given 250, ml, of a 1.30 M pyridine (C5H5N) solution, Pyridine is a weak base with Kg = 1.7 x10^-9. What mass of C5H5NHBr should the student dissolve in the C5H5N solution to turn it into a buffer with pH = 5.227 You may assume that the volume of the solution doesn't change when the C5H5NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A buffer solution contains 0.316 M CH3NH3 C1 and 0.315 M CH3NH2 (methylamine). Determine the pH change when 0.069 mol HBr is added to 1.00 L of the buffer. (Assume Kb (CH3NH2) = 4.2 × 10-4.) pH after addition - pH before addition = pH change
Write the titration reaction of 100 mL of 0.100 M anilinium bromide (“aminobenzene . HBr”) +.100 M NaOH.
5. A buffer is made by mixing 1.250 mol formic acid, HCOOH, with 0.750 mol sodium formate, HCOONa in enough water for a total volume of 1.00L. The Ka of formic acid is 1.87 x 10-4 a. What is the pH of this buffer? b. If 0.075 mol HCI is added to this buffer, what is the pH of the resulting buffer? (assume no volume changes) c. If 0.055 mol NaOH is added to this buffer, what is the pH of the resulting buffer? (Assume no volume changes)
How do I complete problem 1 in a step by step?
6. Which of the following processes will increase the pH of a buffer solution prepared by mixing 0.89 mol HCOOH (formic acid) and 0.76 mol HCOONa (sodium formate) into a 1-L solution? Ka (HCOOH) = 1.8 x 104. %3D a) add some NaCl into the buffer solution. b) add some HCl into the buffer solution. c) add some NaOH into the buffer solution. d) add more water into the buffer solution. e) None of the above.
All boxes please
You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?
Calculate the pH of a buffer solution that is 0.750 M CH3NH2 and 0.200 M CH3NH3Cl. For CH3NH2, Kb = 4.4*10-4
do both please as they are the part of the same question..