2. Describe how you would go about in the lab making 100 ml of a buffer solution of 0.10 M acetic acid and 0.20 M sodium acetate, if the total acetate concentration (acetate in all forms, as either Ac or HAc, is 0.15M). What would be the pH of your buffer? Ka = 1.8 X 10¹5 for HAC.

2. Describe how you would go about in the lab making 100 ml of a buffer solution of 0.10 M acetic acid and 0.20 M sodium acetate, if the total acetate concentration (acetate in all forms, as either Ac or HAc, is 0.15M). What would be the pH of your buffer? Ka = 1.8 X 10¹5 for HAC.

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: The Ka of formic acid HCOOH is 1.77 x 10-4. A 0.60 M formic acid solution of 40.0 mL is titrated…

Q: for the given alkyl position. Bond Dissociation Energies (for A-BA + B) Bond broken AH (kJ/mol) Bond…

A: Bond dissociation energy - Bond dissociation energy (BDE) is the energy required to break a bond,…

Q: 4. As mentioned, the bicarbonate buffer works to maintain your body at a certain pH level. If a…

A: The objective of this question is to calculate the pH of a bicarbonate buffer solution formed with…

Q: Calculate the pH of a buffer prepared by adding 0.44 moles of acetic acid and 0.25 moles of acetate…

Q: A chemistry graduate student is given 450. mL of a 0.20M ammonia (NH,) solution. Ammonia is a weak…

A: GivenpH = 9.14pOH + pH = 14pOH + 9.14 = 14pOH = 4.86

Q: A buffer solution is made that is 0.450 M in HF and 0.450 M in NaF. If Ka for HF is 7.20 × 10¬4,…

Q: calculate the pH of a solution that is made when 0.10 L of 0.24 M benzoic acid (pKa=4.19) and 3.00 g…

A: Molarity of sodium benzoate can be calculated as follows:

Q: A buffer consists of 0.150 M acid, HA, and 0.200 M of its conjugate base, A. If HA has a K, of 4.84…

Q: A student obtains a sample of 0.02500 M acetic acid (CH3COOH, 60.05 g/mole, Ka =1.8 x 10-5). 50.00…

Q: A chemistry graduate student is given 250.mL of a 0.90M diethylamine ((C_2H_5)_2NH) solution.…

Q: You have 500 mL of a buffer solution conatining 0.154 M acetic acid (CH3COOH) and 0.158 M sodium…

A: we have to calculate the pH after NaOH is added to the buffer solution

Q: 1. Calculate the pH of a solution that is 0.10 M NaClO and 0.10 M HCLO. Ka = 2.8 x 10-8 for HCLO.…

Q: 1. What is the pH of a solution that results from adding 400 mL of 0.40 M NaOH to 600 mL of 0.50 M…

A: Note: As per the guidelines solution of 1st question has been made. For the expert solution of other…

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

Q: If a 31.78 mL sample of hydrocyanic acid (HCN) is titrated to the equivalence point with 42.55 mL of…

A: Ka of HCN = 6.17 x 10-10 pKa = -log(6.17 x 10-10) = 9.21 Let molarity of HCN is M moles/ litre…

Q: An industrial chemist studying bleaching and sterilizing prepares several hypochlorite buffers.…

A: Given : a buffer solution with 1) concentration of weak acid i.e HClO = 0.200 M 2) concentration of…

Q: You have 500.0 mL of a buffer solution containing 0.30 Macetic acid (CH₂COOH) and 0.20 M sodium…

A: Volume of buffer solution = 500 mL = 500 × 10-3 L Molarity of Acetic acid = 0.30 M Molarity of…

Q: Three buffers are prepared using equal concentrations offormic acid (HCOOH) and sodium formate,…

Q: A buffer solution is made that is 0.450 M in HF and 0.450 M in NaF. If Ka for HF is 7.20 × 10-4,…

Q: Part 1: A buffer system is set up with [HA] = 0.550 M and [A-] = 0.460 M in 1.0 L of aqueous…

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: Calculate the pH of a solution that is made when 0.10 L of 0.24 M benzoic acid (pKa = 4.19) and…

A: Mass of sodium benzoate = 3.00 g Molar mass of sodium benzoate = 144.11 g/mol Moles =…

Q: You are required to prepare a buffer (pH = 5.30) using propionic acid and sodium propionate. The…

A: Answer:- This question is answered by using the simple concept of calculation of concentration of…

Q: a Calculate the pH of a solution that is 0.20 M HOCI and 0.88 M KOCI. Ka = 3.5x10-8 pH = 8.1 b In…

Q: 4. You need to make a buffer with pH as close to 10.00 as possible. Two sets of weak acids and…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: How many grams of dry NH4 Cl need to be added to 2.10 L of a 0.100 M solution of ammonia, NH3, to…

A: Given: Volume of ammonia solution = 2.10 L Molarity of ammonia solution = 0.100 M pH of buffer…

Q: A buffer is prepared by mixing 2.50 g of benzoic acid (HC7H5O2) and 3.50 g of sodium benzoate…

A: A Buffer solution is made with a weak acid like benzoic acid and conjugate base of benzoic acid i.e.…

Q: suitable

A: Buffer solution worked at pH = pKa-1 to pKa +1 Here pH = 7.0 then range should be 6 to 8 at this…

Q: Phosphoric acid is a triprotic acid (?a1=6.9×10−3 M, ?a2=6.2×10−8 M, and ?a3=4.8×10−13 M). To find…

Q: When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an…

A: The question is based on the titrations. we are titrating a weak acid acetic acid with a strong…

Q: 2. What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium…

A: Given that: Mass of ammonia = 5.0g Mass of ammonium chloride = 20.0g Kb = 1.76×10-5

Question

2. Describe how you would go about in the lab making 100 ml of a buffer solution of 0.10
M acetic acid and 0.20 M sodium acetate, if the total acetate concentration (acetate in all
forms, as either Ac or HAc, is 0.15M). What would be the pH of your buffer? Ka=1.8
X 105 for HAC.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Defining the buffer solution!

VIEW

Step 2: Calculation for volume of acetic acid and sodium acetate solution required!

VIEW

Step 3: Calculation for pH of buffer!

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 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

You have 0.100 M solutions of acetic acid ( p?a = 4.76 ) and sodium acetate. If you wanted to prepare 1.00 L of 0.100 M acetate buffer of pH 4.00 , how many milliliters of acetic acid and sodium acetate would you add?
A 350-mL buffer solution is 0.500 M in chlorous acid (HClO2, Ka=1.1×10−2) and 0.200 M in sodium chlorite (NaClO2). What is the pH of this solution? Express your answer using two decimal places.pH =
A buffer solution is made that is 0.368 M in HCN and 0.368 M in KCN. If Ka for HCN is 4.00 × 10-¹0, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.088 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + +
Calculate the pH of solution after the addition of 0.010 mol NaOH to 1.00L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10*) What is the neutralization reaction that happens? Is the system still a buffer after neutralization?
What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of a buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. (The Ka for acetic acid is 1.80 ×10-5.)
Consider a buffer made by dissolving 0.140 mol cyanic acid, HCNO, and 0.11 mol potassium cyanate, KCNO, in enough water to make a 1-L solution. Assuming that the volume does not change, what is the pH of the buffer before any acid or base is added? Ka = 3.5 x 10-4 O 3.46 O 3.25 3.36 O None of the above
What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 3.10? (Ka for HF is 6.8 × 10⁻⁴)
When a strong base is added to buffer it will react to become neutralized. Determine the pH after 0.15 mol of OH- is added to a buffer consisting of 2.0 mol of HA and 1.0 mol of A-. (Ka = 5.8 x 10-10) HA + OH- → A- + H2O
Which is true about buffer solutions? -they hold the pH close to the pKa -they contain comparable moles of a weak acid and a strong base - they hold pH constant at pH=7 -they prevent acids and bases from reaching equilibrium -they hold the pH close to the equivalence point pH
To create a buffer solution, 40.00mL of a 0.100M benzoic acid (Bz) solution are mixed with 20.00mL of 0.100M sodium hydroxide solution. What is the pH of the resulting solution if the Ka of benzoic acid 6.5 x10 -5 and the pKa = 4.19? (Use the Henderson Hasselbach Equation with mmol). Reaction: HOBz + OH- ---> H2O + OBz- From the buffer solution above, youo take a 10.00mL portion of the buffer. Using all of the information provided, how much conjugate acid and conjugate base are in the 10.00mL portion that you took out? Group of answer choices 0.167mmol 0.500mmol 0.222mmol 0.333mmol
How many grams of sodium hypochlorite, NaCIO, need to be added to 227 mL of a 0.185 M solution of hypochlorous acid, HCIO, to get a buffer with a pH of 7.92? The Ką for hypochlorous acid is 2.9 × 10-8.