You have a 1M solution of the buffer Tris-HCI. You need to use the buffer in the lab at a final concentration of 200 mM. You need to make 250 ml of this buffer. How would you make this solution? Express your answer in ml. (HINT: 1000 mM = 1 M %3D

You have a 1M solution of the buffer Tris-HCI. You need to use the buffer in the lab at a final concentration of 200 mM. You need to make 250 ml of this buffer. How would you make this solution? Express your answer in ml. (HINT: 1000 mM = 1 M %3D

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 525-mL buffer solution is 0.367 M in acetic acid (CH3COOH) and 0.367 M in sodium acetate…

A: We have to calculate the initial pH and pH after adding given amount of acids and bases.

Q: HA 0.05 L buffer solution (pH = 11.00) was prepared from 0.02 L, 0.2 M NaHCO3 and bottle of sodium…

A: Given the volume of the buffer solution prepared = 0.05 L pH of the buffer = 11.00 NaHCO3 and…

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

Q: # 65 of 214 A2 equivalence 25.00 mL of a solution containing 0.1333 M ammonia (K = 1.76 x 10-5) is…

A: Concept based on buffer solutions.

Q: A 22.0 mL solution of 0.120 M CH3COOH is titrated with a 0.240 M KOH solution. Calculate the pH…

A: In the given question, we are tasked with calculating the pH of a solution at two different points…

Q: A 1.0-LL buffer solution initially contains 0.30 molmol of NH3NH3 (Kb=1.76×10−5)(Kb=1.76×10−5) and…

Q: A student was titrating a solution of HC,H,O, with a Sr(OH)2 solution. Determine the pH at a…

Q: Consider the titration of a 25.4 - mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the…

A: The given information is The titration of 25.4 mL sample of 0.125 M RbOH with 0.110 M HCl. The pH at…

Q: A student prepared a 1:1 buffer, for which [HAc] = [Ac-] = 0.05120 M. Using their 1:1 buffer and a…

A: The question revolves around the preparation of a solution (Solution C) by a student using a 1:1…

Q: A buffer is made by dissolving 12.4 g of sodium dihydrogen phosphate, NaH,P04, and 21.8 g of…

A: pH means the negative logarithm of hydronium ions. By using Henderson - Hasselblach equation: A is…

Q: A Calculating the pH of a Buffer: pH-pk +log HA the Henderson-Hasselbalch equation. This applies…

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

Q: A 252.03 mL, 0.654M weak base solution was titrated with a 0.276 M hydrochloric acid. What is the pH…

A: We have to calculate the pH of solution

Q: A student prepared a 1:1 buffer, for which [HAc] = [Ac-] = 0.05182 M. Using their 1:1 buffer and a…

A: Given that,a student prepared a 1:1 buffer, for which[HAc] = [Ac-] = 0.05182 Mmolarity of HCl…

Q: I just need assistance with part B 5a) Calculate the pH of a buffer solution that contains 0.79 M…

A: The solution containing NaH2PO4 and Na2HPO4 act as a buffer solution because the solution contains a…

Q: What is the pH of the mixture after 45.00 mL 0.102 M NaOH base are added to a 30.00 mL solution of…

A: Molarity = Number of moles of soluteVolume of solution (in L) Number of moles of NaOH in mixture =…

Q: You are instructed to create 100 mL of a 0.05 M Acetate buffer with a pH of 3.8. You have Glacial…

A: A buffer system is a solution that resists changes in pH when small amounts of an acid or a base are…

Q: The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid…

A: For a buffer, buffer capacity is the pH range = pKa ± 1

Q: Question: Determine the [H3O+] of the eight buffer solutions made by mixing 1.10 M acetic acid and…

A: "Since you have asked multiple subpart question, we will solve the first three subpart question for…

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 contains 0.237 M C6H5NH3 Cl and 0.366 M C6H5NH₂ (aniline). Determine the pH change…

A: Volume of buffer solution V = 1.00 L Number of moles of HCl added = 0.090 mole Concentration of…

Q: A student prepared a 1:1 buffer, for which [HAc] = [Ac-] = 0.05491 M. Using their 1:1 buffer and a…

A: Given:The preparation of a solution (Solution C) by a student using a 1:1 buffer system consisting…

Q: ated Find the pH at the end point in the titration of 0.2 M potassium acid maleate, KHM. with 0.2 M…

A: The reaction between KHM and NaOH: KHM+NaOH→NaKM+H2O

Q: 5. a) Calculate the pH of a buffer solution which is 0.1 mol/L with respect to HCN (K₁ = 4.9 x 10-¹0…

A: Note: Since you have posted a question with multiple sub-parts, we will solve the first three…

Q: A student prepared a 1:1 buffer, for which [HAc] = [Ac-] = 0.05096 M. Using their 1:1 buffer and a…

A: The objective of the question is to calculate the moles of .

Q: A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kb (C2H5NH2) =…

A: Calculation of pKb: pKb=-log Kb=-log 4.3×10-4=3.37 Calculation of initial pOH:…

Q: A student was titrating a solution of HC,H,O with a Sr(OH), solution. Determine the pH at a…

A: The objective of this question is to determine the pH of a solution at a particular point during the…

Q: You find 425.0 mLof 0.350 M sodium oxalate in the lab, and you want to use it to make a buffer with…

A: Volume of sodium oxalate = 425 mL or 0.425 L Molarity of sodium oxalate = 0.350 M Moles of sodium…

Q: How many grams of sodium acetate (CH3CO2Na, Mw =82.0 g/mole) should be present in 1.0 L of 0.65 mole…

A: Given that Acidic Buffer solution of sodium acetate and acetic acid pH for buffer = 4.47 Ka for…

Q: A beaker with 165 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total…

Q: Determine [Zn2 ], [CN–], and [HCN] in a saturated solution of Zn(CN)2 with a fixed pH of 3.610. The…

A: Given:The pH of the solution is 3.610 The solubility product (Ksp) of Zn(CN)2 is .The Ka of HCN is .

Q: titration between 25.0 mL of a weak base (Kb= 6.9*10-5) and 0.100 M hydrochloric acid). A.What is…

Q: An oxalic acid/oxalate buffer has a final volume of 3.0L and pH of 4.8 What is the effective…

A: We can solve this problem using Henderson-Hasselbalch equation.

Q: A chemistry graduate student is given 450. mL of a 0.70M pyridine (C,H,N) solution. Pyridine is a…

A: The volume of the pyridine solution = 450 mLThe concentration of the pyridine solution = 0.70 MThe…

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 have a 1M solution of the buffer Tris-HCI. You need to use the buffer in
the lab at a final concentration of 200 mM. You need to make 250 ml of this
buffer. How would you make this solution? Express your answer in ml. (HINT:
1000 mM
1 M

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

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

Answer the following questions about a titration between 20.0 mL of a weak base (Kb= 4.7*10-6) and 0.150 M hydrochloric acid. A.What is the concentration of the weak base solution if it requires 26.67 mL of the HCl solution to reach the equivalence point (assume 1:1 stoichiometry)? B.What is the initial pH of the weak base solution before any HCl is added? C.What is the pH of the titration at the equivalence point? D.The pKa of bruhmophenol is ~ 4.9 and the pKa of thymol blue ~ 9.2. Which indicator would be best to use in the titration
Hello, I don't know where I'm going wrong. I'm using the Henderson-Hasselbalch equation. I've attempted three time with no success. Could you break down this problem so I can spot where I am going wrong? Thank you. Screenshot of problem is attached.
Calculate the pH of a solution that is 0.200 M in NH3 and 0.300 M in NH4Cl. Calculate the pH change that takes place when a 100-mL portion of (A) 0.0500 M NaOH and (B) 0.0500 M HCl is added to 400 mL of the buffer solution. Kb = 1.75 x 10-5 show your solution in picture
What is the effective pH range for a sodium acetate/acetic acid buffer? Ka = 1.80 x 105. %3D Enter your answer to three decimals. to
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 5 pH = 6 pH = 8 O yes Ba(OH), O no do O yes CuBr O no O yes AgCN O no Explanation Check Rights Reserved Terms of Use Privacy Accessibility O 10:00 O oo o0
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 2 pH = 3 pH = 5 O yes BaCO, dlo O no O yes Cal, O no O yes Ni(OH), O no Check Terms of Use Privacy Explanation 2021 McGraw-Hill Education. All R V 1 10: Ocer