How many microliters of 1.000 M NaOH solution must be added to 25.00 mL of a 0.1000 M solution of lactic acid (CH, CH(OH)COOH or HC₂H₂O₂) to produce a buffer with pH=3.70? Express your answer using two significant figures.

How many microliters of 1.000 M NaOH solution must be added to 25.00 mL of a 0.1000 M solution of lactic acid (CH, CH(OH)COOH or HC₂H₂O₂) to produce a buffer with pH=3.70? Express your answer using two significant figures.

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 volume of 500.0 mL of 0.140 M NaOH is added to 615 mL of 0.250 M weak acid (?a=8.47×10−5). What is…

Q: Two solutions of an unknown slightly soluble salt, A(OH)2, were allowed to equilibrate—one at 25 °C…

A: Given: Volume of A(OH)2 =15 mL Concentration of HCl = 0.20 M At 25oC Volume of HCl =6.37 mL At 80oC…

Q: A volume of 500.0 mL of 0.170 M NaOH is added to 625 mL of 0.200 M weak acid (Ka=2.88×10−5). What is…

A: pKa = - log Ka = - log (2.88 * 10-5) = 4.541

Q: A chemistry graduate student is given 300. mL of a 1.10M hydrocyanic acid (HCN) solution.…

Q: A chemistry graduate student is given 250. mL of a 0.70M hydrocyanic acid (HCN) solution.…

Q: A buffer solution of volume 1.0 L contains 0.200 M of a weak acid (pKa 4.37) and 0.100 M sodium salt…

A: Number of moles of weak acid HA = 0.200 M × 1.0 L = 0.200 molNumber of moles of A– = 0.100 M × 1.0 L…

Q: A student does a titration of 86.0 mL of a 0.37 M solution of methylamine (CH3NH2(aq) (pKb =3.36)…

A: PH+Poh=14. This is basic buffer equation Poh=pkb+log[salt]/base Use this equation and get the…

Q: A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated…

A: Given, A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution…

Q: What mass of (CH,) NH,Cl should the student dissolve in

Q: You are asked to prepare a pH = 3.00 buffer solution starting from 1.00 L of a 1.00 M solution of…

A: Given:pH of solution = 3.00Volume of HF solution = 1.00 LConcentration of HF = 1.00 MKa of HF =…

Q: chemistry graduate student is given 450. mL of a 0.50M trimethylamine ((CH3)₂N) N solution.…

Q: A buffer is made by adding 0.68 g of sodium formate, NaHCOO (molar mass = 68.0 g/mol), to 1.00 L of…

A: Given : Mass of sodium formate i.e NaHCOO = 0.68 g Concentration of formic acid i.e HCOOH = 0.015 M…

Q: A 30.00 mL portion of 0.225 M hydrochloric acid is titrated with Ca(OH)2 of unknown concentration.…

A: The given problem can be solved by using the formula given below to reach the endpoint is as…

Q: A buffer is made by mixing 40.00 mL of a 0.100 M solution of the fictitious acid HA (pKa = 5.11)…

A: Given,Molarity of fictitious acid, HA = 0.100 M ( pKa = 5.11 )volume of HA = 40.00 mLMolarity of…

Q: HEPES is commonly used to make physiological buffers and undergoes the following dissociation:…

A: Given: Concentration of buffer = 0.1000 M pH of buffer = 7.20 Volume of buffer = 2.000 L Molar mass…

Q: A buffer solution was prepared by adding 4.92 g of sodium acetate, NaCH3CO2, to 2.50 x 10^2 mL of…

A: The objective of this question is to calculate the pH of a buffer solution after adding a certain…

Q: The pKp values for the dibasic base B are pKbl = 2.10 and pKb2 = 7.65. Calculate the pH at each of…

A: pH is a scale which basically measure the acidity/ basicity of a solution. If PH value is 7 then…

Q: A chemistry graduate student is given 125. mL of a 0.20M chlorous acid (HClO₂) solution. Chlorous…

Q: A buffer is composed of 0.200 M (CH3)2NH (Kb = 5.9 × 10–4) and 0.250 M (CH3)2NH2NO3. What is the pH…

A: The given solution is a buffer solution composed of (CH3)2NH and (CH3)2NH2NO3. Molarity of (CH3)2NH…

Q: A chemistry graduate student is given 500. mL of a 0.40M ammonia (NH,) solution. Ammonia is a weak…

Q: When a 16.0 mL sample of a 0.469 M aqueous nitrous acid solution is titrated with a 0.460 M aqueous…

Q: 1) What is the pH at the equivalence point in the titration of a 29.1 mL sample of a 0.450 M aqueous…

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

Q: What is the pH of the equivalence point?

Q: When a 28.1 mL sample of a 0.465 M aqueous acetic acid solution is titrated with a 0.419 M aqueous…

Q: Consider a titration where 0.215 M potassium hydroxide is added from a burette to 10.00 mL of…

A: Given: Titration of potassium hydroxide with hydrochloric acid.

Q: 1. A 20.0 mL sample of a 0.240 M hydrofluoric acid (HF) solution is titrated with 0.200 M NaOH.…

Q: A chemistry graduate student is given 500. mL of a 0.70M propanoic acid (HC₂H,CO₂) solution.…

Q: 1) A 25.0 ml solution of an unknown concentration of phosphoric acid, H;PO4, is titrated with0.250 M…

Q: How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the…

A: a) Moles of base = Molarity * Volume (L) = 0.1M * 0.025 L = 0.0025 mol At equivalence point- Moles…

Q: == O Acids and Bases Calculating the composition of a buffer of a given pH 0/5 10 A chemistry…

A: Buffers are solutions that can resist the change in the pH of the solution when acid or a base is…

Q: A chemistry graduate student is given 250. mL of a 1.20m benzoic acid (HCH₂CO₂) solution. Benzoic…

Q: ☐ x10 b A chemistry graduate student is given 250. mL of a 0.10M methylamine (CH3NH2) solution.…

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

How many microliters of 1.000 M NaOH solution must be added to 25.00 mL of a 0.1000 M solution of lactic acid (CH, CH(OH)COOH or HC₂H₂O₂) to produce a
buffer with pH=3.70?
Express your answer using two significant figures.
1951 ΑΣΦ
V=
µL

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: Given data and required constants

VIEW

Step 2: Determination of number of moles of lactic acid

VIEW

Step 3: Solving Henderson-Hasselbalch equation

VIEW

Step 4: Determining the number of moles of NaOH required

VIEW

Step 5: Determination of the volume of NaOH required.

VIEW

Solution

VIEW

Step by step

Solved in 6 steps with 10 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

We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.8 mL of the NaOH solution to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the pKa value of HA(aq)? (c) What is the pH at the equivalence point? (d) What is the pH one third along the titration when you still have twice as much HA(aq) as A-(aq)?
A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.
A chemistry graduate student is given 125. mL of a 0.90M benzoic acid (HC,H,CO2) solution. Benzoic acid is a weak acid with K,=6.3 × 10 °. - 5 What mass of NaC,H,CO, should the student dissolve in the HC,H,CO, solution to turn it into a buffer with pH = 3.97? You may assume that the volume of the solution doesn't change when the NaCH,CO, is dissolved in it. Be sure your answer has a unit symbol, and round it 2. to 2 significant digits. x10
7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?
A volume of 500.0 mL of 0.180 M NaOH is added to 545 mL of 0.250 M weak acid (Ka = 6.39 × 10). What is the pH of the resulting buffer? НА(аq) + ОН (aq) - → H, O(1) + A (aq) pH =
A chemistry graduate student is given 500.mL of a 0.80M chloroacetic acid (HCH2ClCO2) solution. Chloroacetic acid is a weak acid with Ka = 1.3x10^−3. What mass of NaCH2ClCO2 should the student dissolve in the HCH2ClCO2 solution to turn it into a buffer with pH = 3.08 ?You may assume that the volume of the solution doesn't change when the NaCH2ClCO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
2. Dr. Dahm has prepared 250 mL of a acetate buffer which contains 0.1 mol of acetic acid (CH₂COOH) and 0.15 moles of acetate (CH₂COO). Determine the initial pH. If he then adds 0.025 moles of H* calculate the new pH. Ka = 1.8 × 10³ CH₂COOH(aq) + H₂O CH₂COO (aq) + HO (aq) 3. Dr. Dahm makes a second acetate buffer exactly the same way as in #2, but he then adds 15 mL of 0.50 M NaOH calculate the new pH.
The curve for the titration of 25.0 mL of 0.100 M C5H5N(aq), pyridine, with 0.100 M HCI(aq) is given below. 12 10 8 4 2 5 10 15 20 25 30 35 Va(mL) (If the image above does not appear, click here.) Estimate the pH at the stoichiometric point. Your answer must contain only one decimal place. 8.8
What is the pH of a buffer solution if you have 250 ml of a 1.56M Acetic Acid and you added 26.56 grams of sodium acetate (NaCH3CO2)? What is the new pH if you now add 1gram of NaOH to the buffer solution?
A chemistry graduate student is given 500. mL of a 1.60M chloroacetic acid (HCH2CICO2) solution. Chloroacetic acid is a weak acid with K = 1.3 × 103. What mass of NaCH2CICO₂ should the student dissolve in the HCH2CICO2 solution to turn it into a buffer with pH =2.37? You may assume that the volume of the solution doesn't change when the NaCH2CICO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. Explanation Check G MacBook Air 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility
(a) Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate in muscles during intense exercise. A chemist prepares a buffer using 225 mL of 85 M lactic acid (Ka = 1.38 x 10-4) and 435 mL of 0.68 M sodium lactate. What is the pH of the buffer? What is the pH of the lactate buffer if 0.25 moles of gaseous HCl is added?
A buffer is made using 100.0 mL of 0.100 M CH3CH2COOH (propanoic acid) and 100.0 mL of 0.100 M NaCH3CH2COO (sodium propanoate). 10.0 mL of 0.100 M HCl is added to the buffer. What is the solution pH after the HCl is added?For CH3CH2COOH K = 1.3 x 10^-5