2. A buffer solution is prepared by mixing 15.00 mL of 0.12 M CH₃COOH with 9.00 mL of 0.080 M NaOH. a. Calculate the moles of CH₃COOH and NaOH before mixing. b. Assuming the reaction goes to completion, calculate the moles of CH₃COOH and CH₃COO⁻ present in the buffer solution. c. Calculate the concentration of CH₃COOH and CH₃COO⁻ in the buffer solution. d. Use the Henderson-Hasselbalch equation to calculate the expected pH of this buffer solution. CH₃COOH Kₐ = 1.8 x 10⁻⁵.

Answered: Image /qna-images/answer/e9cd9ce4-500c-433b-bad8-c5d7505ed6e9.jpg

2. A buffer solution is prepared by mixing 15.00 mL of 0.12 M CH COOH with 9.00 mL of 0.080 M NaOH. a. Calculate the moles of CH COOH and NaOH before mixing. b. Assuming the reaction goes to completion, calculate the moles of CH.COOH and CH COO present in the buffer solution. c. Calculate the concentration of CH.COOH and CH COO in the buffer solution. d. Use the Henderson-Hasselbalch equation to calculate the expected pH of this buffer solution. CH.COOH K. = 1.8 x 10³.

2. A buffer solution is prepared by mixing 15.00 mL of 0.12 M CH COOH with 9.00 mL of 0.080 M NaOH. a. Calculate the moles of CH COOH and NaOH before mixing. b. Assuming the reaction goes to completion, calculate the moles of CH.COOH and CH COO present in the buffer solution. c. Calculate the concentration of CH.COOH and CH COO in the buffer solution. d. Use the Henderson-Hasselbalch equation to calculate the expected pH of this buffer solution. CH.COOH K. = 1.8 x 10³.

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: A 1.00 liter solution contains 0.45 M hydrocyanic acid and 0.58 M sodium cyanide. If 0.15 moles of…

A: Explanation:Don't forget to leave a helpful rate.Thank you and happy learning on Course Hero!

Q: A 25.00 mL sample of magnesium hydroxide solution is titrated with 0.00500 M HCl and 2 drops of…

Q: An aqueous solution of Ca(OH)2with a concentration of 0.146 M was used to titrate 25.00 mL of…

A: Answer:- This question is answered by using the simple concept of chemical reaction between acid and…

Q: A buffer solution is one which a. contains the maximum amount of solute possible for a…

A: Buffer solutions are those solutions that resist the change in pH on the addition of a small amount…

Q: A 22.2 mL sample of 0.357 M ammonia, NH3, is titrated with 0.352 M hydroiodic acid. The pH before…

A: Since you have posted unrelated question as per guidelines we can solve only one per session . If…

Q: [Review Topics] [References] Use the References to access important values if needed for this…

A: The question is based on the concept of solubility product Principle. it states that a weak…

Q: + For the reaction NH3 + H₂O → NHÂ* + OH¯, if 0.010 M of NH3 is added, what is the concentration of…

A: Here the dissociation reaction of NH3 is given in the H 2 O.Now here do not give any other…

Q: Consider the solubility of BaSO4. If Ba(NO3)2 is added to the solution, the solubility of the barium…

A: Due to presence of common ion Solubility of BaSO4 is decreases

Q: What is the common ion in a solution prepared by mixing Ca(OH)2 adnd Ca(NO3)2? a. OH-…

A: Ca(OH)2 will dissociate into solution as Ca(OH)2 --> Ca2+ + 2 OH-

Q: vi. What species are present in each of these substances? Species Present NaCl(ag) NaCI(s) i. Write…

Q: A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.023 M HCl, and the equivalence…

A: A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.023 M HCl, and the equivalence…

Q: In an experiment, 1.000 mol H2 and 1.000 mol l2 are mixed in a 1.00-L container, and the reaction…

A: Equilibrium constant can be defined as number that represents the relationship between the amounts…

Q: Use the solubility rules listed in Section 8.3B to predict whether each of the following ionic…

A: Since you have posted multiple sub-parts, the answer for first three sub-parts are given below.…

Q: A 0.2071-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized…

Q: A 25.0 mL sample of lithium hydroxide is completely neutralized by adding 30.0 mL of 0.100 mol/L…

A: Given: Concentration of H3PO4 is 0.100 mol/L Volume of phosphoric acid is 30.0 mL or 0.03 L Volume…

Q: a. A 1.0 L solution that is 0.60 M in ammonia is mixed with 75.8 g of ammonium sulfate. What is the…

A: The addition of any small quantity of acids/base in a buffered solution (solution of weak base plus…

Q: Consider these compounds: A. NICO3 B. Zn(OH)2 C. Cus D. Fe(OH) 2 Complete the following statements…

A: Answer:Ionic compound that has low solubility in water is called as sparingly soluble compound and…

Q: a. Calculate the solubility of PbBr, if the Ksp=6.6 x 106 b. Calculate the solubility of PbBr, if…

Q: A solution of sulfuric acid (25.00 mL) was titrated to the second equivalence point with 36.55mL of…

Q: Write the reaction that takes place when OHa) is added to a basic buffer solution containing…

A: Given: Buffer solution of HONH2 and HONH3+. And OH- is added in the solution.

Q: A solution contains 9.15x10-³ M sodium sulfide and 9.79×10- 3 M potassium hydroxide. Solid…

A: The question is based on the concept of solubility product principle. It that states that when a…

Q: solution contains 6.88×10-3 M ammonium carbonate and 1.16×10-2 M potassium fluoride. Solid magnesium…

A: The question is based on the concept of solubility product Principle. it states that a weak…

Q: A solution contains 1.08×10-2 M lead nitrate and 1.24x10-2 M silver acetate. Solid ammonium bromide…

A: Given: Concentration of silver acetate i.e. AgCH3COO = 1.24 × 10-2 M Concentration of lead nitrate…

Q: A solution contains 1.30×102 M lead acetate and 7.48×103 M calcium nitrate. Solid potassium sulfate…

A: Precipitation reaction occurs when two ionic compounds interact in an aqueous solution to form an…

Q: A solution contains 1.26x102 M manganese(II) acetate and 1.03x10² M nickel(II) nitrate. Solid sodium…

Q: A solution contains 1.20x10-2 M lead nitrate and 1.07x10-2 M calcium acetate. Solid sodium sulfate…

A: Concentration of lead nitrate = 1.20 x 10-2 M Concentration of calcium acetate = 1.07 x 10-2 M Solid…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: We have to write the balanced equation for the reaction and calculate :- moles of HNO₃ moles of…

Q: Which of the following compounds is SOLUBLE? A. SrSO4 B. CaCO3 C. BaS D. CaCl2

A: Among all the given compounds SrSO4, CaCO3, BaS and CaCl2, calcium chloride (CaCl2) is highly…

Q: Which compound will dissolve in water in large amounts

A: Greater lattice energy (energy which is required to dissociate 1 mole of an ionic compound into its…

Q: A 10.00 mL sample of H3PO4 is titrated with 0.100 M Ca(OH)2. The equivalence point is reached after…

A: Equivalent =molarity×volume×n factor n factor is no of replace H+ ion or OH- ion for acid and base…

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

2. A buffer solution is prepared by mixing 15.00 mL of 0.12 M CH₃COOH with 9.00 mL of 0.080 M NaOH.

a. Calculate the moles of CH₃COOH and NaOH before mixing.

b. Assuming the reaction goes to completion, calculate the moles of CH₃COOH and CH₃COO⁻ present in the buffer solution.

c. Calculate the concentration of CH₃COOH and CH₃COO⁻ in the buffer solution.

d. Use the Henderson-Hasselbalch equation to calculate the expected pH of this buffer solution. CH₃COOH Kₐ = 1.8 x 10⁻⁵.

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: Determine the given values

VIEW

Step 2: Determine the moles of CH3COOH and NaOH before mixing

VIEW

Step 3: Determine the moles of CH3COOH and CH3COO- present in the buffer solution.

VIEW

Step 4: Determine the concentration of CH3COOH and CH3COO- present in the buffer solution.

VIEW

Step 5: Determine the pH of the buffer solution

VIEW

Solution

VIEW

Step by step

Solved in 6 steps with 9 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 solution contains 1.42×10-2 M manganese(II) nitrate and 1.47×10-2 M magnesium acetate.Solid sodium hydroxide is added slowly to this mixture.A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of hydroxide ion when this precipitation first begins?[OH-] = M
A solution contains 1.13×10-2 M chromium(III) nitrate and 1.16×10-2 M nickel(II) acetate. Solid potassium hydroxide is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of hydroxide ion when this precipitation first begins? [OH-] = ____M
1. For the reaction: 2NH3(g) + CO2(g) (NH2)2CO(s) + H2O(g) AH = - 330 kJ Predict how each of the following changes would impact a reaction that is currently at equilibrium. That is, which way would the reaction progress in order to respond to the change in the system to regain equilibrium (use arrows to show the direction of change that would occur to return back to equilibrium). Explain your reasoning for each part.
Consider the titration of H2SO4 with NaOH. A 30.0 L sample of H2SO4 requires 0.090L of 0.100 M NaOH. What are the moles ofacid? Number of molecules of the acid? Molarity of Acid? what is the grams of Acid present?A. Moles of Acid?B. Molecules of AcidC. Molarity of AcidD. grams of Acid?
a. You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution of nitrous acid, HNO2, and an 0.68 M solution of NaOH. What volume of each of these solutions must be mixed in order to get the desired buffer solution? Use the simultaneous equations method to solve this problem. b)If the acid used in a. was nitric acid, HNO3, could the same buffer solution be made? Briefly explain. c) If the buffer solution prepared in a. also contained ~10–6M Ni2+ and ~10–6 M Pb2+ , could those metal ions be separated from each other by saturating the solution with H2S? Explain your answer by showing the necessary calculations.
9. Which of the following materials is Not Soluble ( insoluble ) in water ? a) AgCl c) KCl b) AgNO3 d) (NH4)2CO3
A 0.1240 M NaOH(aq) solution was used to titrate 20.00 mL of an acetic acid (CH3COOH) solution that has an unknown concentration. The equivalence point is reached after adding 15.34 mL of NaOH(aq). a. Write out the complete balanced equation for the reaction that occurs in this titration. b. How many moles of NaOH were added to the acetic acid solution? c. How many moles of acetic acid were in the original 20.00 mL solution? d. What was the concentration of acetic acidic in the original 20.0 mL solution?
7. Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2. a. calcium sulfate. c. calcium oxide d. calcium phosphate. b. calcium hydroxide
A solution contains 1.47x102 M zinc nitrate and 1.37x102 M cobalt(II) acetate. Solid potassium carbonate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula B. What is the concentration of carbonate ion when this precipitation first begins? [Co,?] = M
Consider this reaction H2SO4(aq) +2KOH(aq) ---> H2SO4(aq) ---->K2SO4(aq) +2H2O(l) Determine the volume of 0.205 M KOH solution require to neutralize each sampe of sulfuric acid. a. 35mL of 0.205 M H2SO4 b. 205mL of 0.135 M H2SO4 C. 80 ml of 0.100 M H2SO4
A solution contains 1.37×102 M lead nitrate and 7.70×10³ M magnesium acetate. Solid ammonium fluoride is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula B. What is the concentration of fluoride ion when this precipitation first begins? [F] = M
A 1 liter solution contains 0.514 M hydrocyanic acid and 0.386 M potassium cyanide. What will the addition of 0.193 moles of hydrobromic acid do? (Assume that the volume does not change upon the addition of hydrobromic acid.) *More than one answer is accepted. A. Raise the pH slightly B. Lower the pH slightly C. Raise the pH by several units D. Lower the pH by several units E. Not change the pH F. Exceed the buffer capacity