You are working in a lab that studies the psychedelic prodrug, psilocybin. You need to make 1.0 Liter of a 10.0 mM carbonic acid buffer at pH-6. Your lab has a stock solution of 5.0 M NaOH. Describe how you would prepare this buffer solution starting with some amount of carbonic acid, and then adding a strong base (5.0 M NaOH) to get the correct pH. Your answer should explicitly tell me how many moles of carbonic acid you will start with, and how many milliliters of 5.0 M NaOH you will add.

You are working in a lab that studies the psychedelic prodrug, psilocybin. You need to make 1.0 Liter of a 10.0 mM carbonic acid buffer at pH-6. Your lab has a stock solution of 5.0 M NaOH. Describe how you would prepare this buffer solution starting with some amount of carbonic acid, and then adding a strong base (5.0 M NaOH) to get the correct pH. Your answer should explicitly tell me how many moles of carbonic acid you will start with, and how many milliliters of 5.0 M NaOH you will add.

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: I need 30 mL of a buffer solution with a volume ratio of 6:1 acid:base. How do I calculate how much…

A: Given, Volume of buffer = 30mL volume ratio of acid:base = 6:1 Buffer solution: It consists of…

Q: A buffer solution includes a weak acid and its conjugate base. Include states of matter. Write a…

A: A buffer solution is formed by the weak acid and its conjugate base or weak base and its conjugate…

Q: A solution is prepared by combining 3.58 milliliters of 0.3312 M formic acid,128.3 milligrams of…

A: The number of moles of KOH is calculated as shown below.

Q: An analytical chemist is titrating 86.6 mL of a 0.4900M solution of dimethylamine ((CH,) NH) with a…

A: Step 1:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Give a sentence or two on what you would do to complete the preparation of your buffer. You add 0.20…

A: Calculation of pKa of the acid: Calculation of the concentration of the conjugate base (salt):

Q: Describe how would you prepare a buffer solution with pH of 9.50 if you have the following chemicals…

A: Given: pH = 9.50 molar mass of NH4NO3 = 80.043 g/mol List the exact amount of each chemical, 100mL…

Q: Which acid would be best to use when preparing a buffer with a pH of 4.72? A list of Ka values can…

Q: Suppose you want to make 500 mL of a 0.20 M Tris buffer at pH 8.0. On the shelf in your lab, you see…

A: According to the question we have, The pKa of tris is given by = 8.06 The molar concentration of…

Q: 2) What is the pH of a solution that contains 0.10 M hydrocyanic acid and 0.20 M sodium cyanide? 3)…

A: Given,2. Molarity of hydocyanic acid ( HCN ) = 0.10 M Molarity of sodium cyanide ( NaCN ) = 0.20…

Q: 85.0 mL of 0.20M HF (K, = 7.2 x 104)is titrated with 5.0 mL of 0.40 M NAOH. Calculate the pH at this…

Q: How does the buffer solution absorb the added H+ and OH- to make the pH change very small?

A: A buffer can be acidic or basic in nature. A buffer that contains a weak acid with its conjugate…

Q: suppose that the ph of buffer A turned out at ph 5.5 instead of ph 5.0 (100.0 mL of a 0.5 M buffer)…

A: Buffer solution is defined as a solution which resists any change in its pH value even when small…

Q: Buffer 2 will be 150 mL of 0.15 M Tris-HCl buffer with a pH of 8.5 Write out the chemical equation…

A: The objective of the question is to write out the chemical equation for a Tris-HCl buffer and…

Q: what do I need to calculate the theoretical pH if my buffer solution has 0.50 M of a ethyl alcohol…

A: Theoretical pH of a buffer solution is calculated using the Henderson-Hasselbalch Equation written…

Q: Why does buffer capacity increase as the concentration of buffer increases?

A: The solutions which have a nearly constant value of pH or they resist any change in pH value are…

Q: You need to prepare an acetate buffer of pH 5.42 from a 0.774 M acetic acid solution and a 2.96 M…

Q: Briefly explain the most likely reason the student obtained the results of the pH paper turning blue…

A: Explationation of above question is given below.

Q: Calculate the pH of a buffer solution made by mixing a 0.37 M formic acid (HCOOH) with 0.23 M sodium…

A: pH of buffer solution=3.54Explanation:So,pH of buffer solution=3.54

Q: You need to prepare an acetate buffer of pH 5.27 from a 0.895 M acetic acid solution and a 2.71 M…

A: Let volume of KOH = V Liter Molarity of KOH = 2.71 M So, Number of moles of KOH = Molarity of KOH…

Q: Using your knowledge of buffer systems , calculate the pH of the buffer system given the data below:…

Q: Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25…

Q: What must be the minimum concentration of hydrocyanic acid in 1.00L buffer solution of a pH 9.8…

A: Answer: Buffer solution is a type of solution in which on adding small quantity of acid or base, it…

Q: You have prepared a buffer by mixing 20 mL of 0.10 M HOCl with 20 mL of 0.05 M NaOCl, and measured…

A: The given data is as follows: The concentration of HOCl = 0.10 M The volume of HOCl = 20 mL The…

Q: Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 62.9 mL…

Q: Buffer A: Calculate the mass of sodium acetate that must be added to make 100.0 mL of an acetic…

Q: Part A You need to produce a buffer solution that has a pH of 5.21. You already have a solution that…

Q: Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant…

Q: Determine the concentration of CH NH¸* in a buffer solution by constructing an ICE table, writing…

A: Step 1: Given: - Initial [C6H5NH2] = 0.50 M pH = 4.20 [C6H5NH3+] = x Kb = 3.8 × 10-10 The reaction…

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

You are working in a lab that studies the psychedelic prodrug, psilocybin. You need
to make 1.0 Liter of a 10.0 mM carbonic acid buffer at pH-6. Your lab has a stock solution of
5.0 M NaOH. Describe how you would prepare this buffer solution starting with some amount
of carbonic acid, and then adding a strong base (5.0 M NaOH) to get the correct pH. Your answer
should explicitly tell me how many moles of carbonic acid you will start with, and how many
milliliters of 5.0 M NaOH you will add.

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

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

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 make 0.1 L of a buffered solution (pH=9.1) by mixing acetic acid and sodium acetate. You have 1.00 M solutions of each component of the buffered solution. What volume of each solution do you mix to make such a buffered solution? Note that the total ion concentration must be 0.170M.
A buffer solution is prepared by combining 0.848 moles of formic acid and 0.719 moles of sodium formate. What will the solution pH be if 0.126 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places) Type your answer...
The pH of a blood plasma is 7.36. Assuming the principle of buffer system is HCO3-/H2CO3, calculate the ratio HCO3-/H2CO3. Is this buffer solution more effective against an added acid or an added base? (Ka1= 4.2 x 10-7 and Ka2 = 4.8 x 10 -11) (Need to show your calculation.).
Find the ph of a buffer solution that is made by mixing 30ml of 1M NaA and 30ml of 1M HA. Find the ph when 2ml of 1M HCl is added to 30ml of this buffer solution. Given (Ka = 2.11*10^-5)
Calculate change in pH of a buffer solution
A chemist titrates 150.0 mL of a 0.0676M dimethylamine ((CH,) NH) solution with 0.4402M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, of dimethylamine is 3.27. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added. pH = Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibity MacBook Air
Which acid would be best to use when preparing a buffer with a pH of 4.76? A list of Ka values can be found in this table. Ohypoiodous acid O hydrazoic acid Ochloroacetic acid O formic acid
A buffer solution is prepared by combining 0.795 moles of formic acid and 0.898 moles of sodium formate. What will the solution pH be if 0.120 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places)
Please answer
A 1.30 L buffer solution consists of 0.313 M propanoic acid and 0.190 M sodium propanoate. Calculate the pH of the solution following the addition of 0.069 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The K₂ of propanoic acid is 1.34 × 10-5. pH =
Buffer is 200 ml of 0.15 M Tris-HCl buffer with a pH of 8.9 Write out the chemical equation for this buffer. Identify which species is the conjugate acid and conjugate base. What is Pka of this equilibrium? Calculate the ratio of the base to acid using the Henderson-Hasselbach equation.
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