Calculate the weight in grams of the corresponding sodium salt that must be added to 100 ml of the indicated acid solution to obtain the buffer solution at pH 2.68. Molecular Weight of the salt 46.03g/mol Formic acid 0.25M Ka = 1.7x 10-4

Calculate the weight in grams of the corresponding sodium salt that must be added to 100 ml of the indicated acid solution to obtain the buffer solution at pH 2.68. Molecular Weight of the salt 46.03g/mol Formic acid 0.25M Ka = 1.7x 10-4

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: An analytical chemist is titrating 53.0 mL of a 0.3400M solution of propionic acid (HC,H,CO,) with a…

A: Buffer solution not formed

Q: calculate the buffer capacity of a buffer consisiting 0.05 moles each of acetic acid and sodium…

Q: Buffer solution is made by taking 0.404 moles of acid (Pka=5.83) & 0.468 moles of sodium acetate and…

Q: How many moles of sodium hydroxide would have to be added to 250 mL of a 0.385 M hypochlorous acid…

A: The volume of hypochlorous acid = 250 mL The molarity of hypochlorous acid = 0.385 M pH of buffer to…

Q: buffer solution is formed by adding 0.320 moles of solid sodium lactate, NaC₃H₅O₃, to 600.0 ml of…

Q: An analytical chemist is titrating 200.5 mL of a 0.3400M solution of hydrazoic acid (HN,) with a…

A: Here we use the Henderson Hasselbach equation,pH = pKa + log [Salt]/[Acid] Initial Acid = 200.5 x…

Q: a buffer solution consisting of 0.15 moles of ammonia dissolved in half a liter of water. how much…

A: A buffer solution s composed of the weak acid and its conjugate base or weak base and conjugate…

Q: Calculate the mass of the sodium acetate that must be added to to 1.50 L of a 0.450 M acetic acid…

Q: A 1.33 L buffer solution consists of 0.263 M propanoic acid and 0.198 M sodium propanoate. Calculate…

Q: A 1.47 L buffer solution consists of 0.313 M propanoic acid and 0.115 M sodium propanoate. Calculate…

A: According to Hendersen -Hasselbalch equation for propionic acid buffer solution, pH = pka + log…

Q: Calculate the pH of a buffer comprised of 0.10 M hypochlorous acid and 0.080 M sodium hypochlorite.…

A: Formula used:- pH = pKa + log [salt]/[acid]

Q: An analytical chemist is titrating 165.5 mL of a 1.100 M solution of propionic acid (HC,H,CO,) with…

A: Given, 165.5 mL of 1.100 M solution of Propionic acid 497.9 mL of 0.3900 M solution of KOH

Q: Calculate the pH of a buffer solution made by mixing 300 mL of 0.3 M acetic acid, CH;COOH, and…

A: Given, a buffer solution is made by mixing 300 mL of 0.3 M acetic acidand 200 mL of 0.2 M of its…

Q: A buffer solution is made that is 0.357 M in HCN and 0.357 M in KCN. If Ka for HCN is 4.00x10^-10 ,…

A: Given : Concentration of weak acid HCN = 0.357 M Concentration of conjugate base salt of weak acid…

Q: An analytical chemist is titrating 247.0 mL of a 0.6700M solution of propionic acid (HC,H,CO,) with…

Q: A 1.48 L buffer solution consists of 0.100 M butanoic acid and 0.294 M sodium butanoate. Calculate…

A: Given that : The volume of buffer solution = 1.48 L The molarity of butanoic acid = 0.100 M The…

Q: An analytical chemist is titrating 210.3 mL of a 0.4900M Solution of butanoic acid (HC,H,CO,) with a…

Q: A 1.40 L buffer solution consists of 0.256 M propanoic acid and 0.105 M sodium propanoate. Calculate…

A: This is an acidic buffer solution. Moles of propanoic acid = .256*1.4 = 0.3584 Moles of sodium…

Q: If a buffer solution is made from 300.0 mL of 2.2 M pyridine salt mixed with 350.0 mL of 2.0 M…

A: Buffer solution pH is determined using Henderson–Hasselbalch equation. Which relates salt…

Q: A buffer solution consisting of 0.15 moles of ammonia dissolved in half a liter of water. How much…

A: The given solution is NH3/NH4Cl buffer. The pH of the basic buffer solution is to be determined…

Q: An analytical chemist is titrating 56.7 mL of a 0.4900M solution of formic acid (H,CO,) with a…

Q: A 1.41 L buffer solution consists of 0.264 M propanoic acid and 0.131 M sodium propanoate. Calculate…

A: We have to calculate the pH of the solution

Q: An analytical chemist is titrating 88.8 ml. of a 0.4900 M solution of piperidine (C,HNH) with a…

A: When a strong base is added to a weak acid solution or a strong acid is added to a weak base, then…

Q: A buffer solution is prepared by dissolving 1.50 g each of benzoic acid, HC7H5O2, and sodium…

A: The objective of this question is to calculate the pH of a buffer solution prepared by dissolving…

Q: An analytical chemist is titrating 85.5 mL of a 0.4000M solution of formic acid (H₂CO₂) with a…

A: Given A solution is prepared using formic acid = 0.4000M x 85.5 ml = 213.75 mmol NaOH =…

Q: A buffer solution is prepared by dissolving 1.50 g each of benzoic acid, HC7H5O2, and sodium…

A: The objective of this question is to calculate the pH of a buffer solution prepared by dissolving…

Q: Calculate the pH of a buffer formed by mixing 85.0 mL of 0.130 M lactic acid, HC3H5O3, with 95.0 mL…

Q: An analytical chemist is titrating 206.4 mL of a 0.5200 M solution of propionic acid (HC,H,CO,) with…

A: Propionic acid is a weak acid. C2H5COOH + H2O ⇌ H3O+ + C2H5COO- And KOH → K+ + OH-

Q: pH =

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Calculate the pH of a buffer solution that is 2.00 M in phosphoric acid and 1.50 M in potassium…

Q: Calculate the pH of a buffer solution made by mixing 300 mL of 0.3M acetic acid, CH;COOH, and 200-mL…

A: A. 4.4 Given that, Volume of 0.3 M CH3COOH = 300 mL = 0.3 L Moles of CH3COOH = 0.3 M× 0.3 L =…

Q: A 1.49 L buffer solution consists of 0.303 M propanoic acid and 0.148 M sodium propanoate. Calculate…

Q: A buffer solution is prepared by mixing 20.0 mL 0.45 M CH3COOH (acetic acid) with 35.0 mL 0.45 M…

A: The amount, in mL or L, of acetic acid, CH3COOH, that must be added to double the [H3O+] is; 1000…

Q: An analytical chemist is titrating 103.2 mL of a 0.8800M solution of propionic acid (HC,H,CO,) with…

A: Molarity is defined as number of moles of solute divide by volume of solution

Q: A buffer is prepared by adding 35 mL of 0.100 M hypochlorous acid, HOCl, to 65 mL of 0.300 M…

Q: Calculating the pH of a buffer -4 and 0.13M in sodium nitrite α A solution is prepared at 25 °C that…

A: Ph is 3.28Explanation:Step 1:To calculate the pH of the solution, Henderson- Hasselbalch equation,…

Q: What mass (in g) of sodium formate, HCOONA, must be added to 10.0 L of a 0.483 Maqueous solution of…

Q: When a 23.3 mL sample of a 0.379 M aqueous hypochlorous acid solution is titrated with a 0.407 M…

A: Here we have to determine pH at midpoint ,pH at equivalent point when 23.3 ml of a 0.379 M aqueous…

Q: 1.34 L buffer solution consists of 0.128 M butanoic acid and 0.289 M sodium butanoate. Calculate the…

A: When a strong base is added to the buffer solution, then it reacts with the weak acid of the buffer…

Q: A buffer is made by adding 0.300 mol HC:H:O2 and 0.300 mol NaCaH»Oz to enough water to make 1.00 L…

A: Given, Concentration of weak acid that is acetic acid (CH3COOH) of the buffer solution is ----…

Q: A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium…

A: Introduction to Buffer solution- A weak acid and its conjugate base, or vice versa, are combined to…

Q: An analytical chemist is titrating 213.4 mL of a 0.3200M solution of butanoic acid (HC,H,CO, with a…

Q: An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with…

A: Given that: Concentration of butanoic acid = 0.5300 MConcentration of KOH base = 0.8200 MVolume of…

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

Calculate the weight in grams of the corresponding sodium salt that must be
added to 100 ml of the indicated acid solution to obtain the buffer solution at
pH 2.68. Molecular Weight of the salt 46.03g/mol
Formic acid 0.25M Ka = 1.7x 10-4

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

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 2 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

An analytical chemist is titrating 150.6 mL of a 0.4500 M solution of ammonia (NH,) with a 0.6900 M solution of HNO2. The p K, of ammonia is 4.74. 3 Calculate the pH of the base solution after the chemist has added 113.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH %3D
Calculating the pH of a weak base titrated with a strong acid An analytical chemist is titrating 104.1 mL of a 0.1200M solution of propylamine (C,H,NH,) with a 0.2600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 53.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume eguals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility APR 23 MacBook Air O00 000 F4
An analytical chemist is titrating 108.9 mL of a 0.8900 M solution of propionic acid (HC,H,CO,) with a 1.000 M solution of NaOH, The p K of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 73.48 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = Check Explanation rivacy Accessibility Terms 2021 McGravw.Hill Education. All Rights Reserved V I 10: cer
An analytical chemist is titrating 219.9 mL of a 0.5100 M solution of aniline (CH,NH,) with a 0.1800 M solution of HNO,. The p K, of aniline is 9.37. 3 Calculate the pH of the base solution after the chemist has added 360.5 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.
a buffer solution is prepared by dissolving 1 mol of lactic acid C3H6O3, with Ka = 1.4 × 10-⁴ and 1 mol of sodium lactate CH3CH (OH) COONa, in a sufficient amount of water up to a volume of 1 liter .pH of this buffer solution is: a) 5.38 b) 10.15 c) 0.85 d) 4.1
A 1.451.45 L buffer solution consists of 0.1590.159 M butanoic acid and 0.3320.332 M sodium butanoate. Calculate the pH of the solution following the addition of 0.0620.062 moles of NaOHNaOH. Assume that any contribution of the NaOHNaOH to the volume of the solution is negligible. The ?aKa of butanoic acid is 1.52×10−51.52×10−5.
A chemistry student is asked to maked a buffer of pH = 4.0. Which of the following acids would be the best choice? Explain your selection to the best of your ability and in your own words. Formic acid -4 Ka = 1.8 x10 Acetic acid Ka = 1.8 x10-5 -5 Chloropropanoic acid Ka 7.8 x10 Benzoic acid Ka = 6.3 x10-5
You are required to prepare a buffer (pH sodium propionate. The concentration of the propionate must the concentration of the acid be? K, = 1.3 × 105 5.30) using propionic acid and 0.6M. Which one
A 1.50 L buffer solution consists of 0.280 M propanoic acid and 0.139 M sodium propanoate. Calculate the pH of the solution following the addition of 0.065 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The Ka of propanoic acid is 1.34×10^−5.
An analytical chemist is titrating 68.7 ml of a 0.4600 M solution of hydrazoic acid (HN,) with a 0.4100M solution of KOH. The p K, of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 30.6 ml. of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. PH -
A 1.47 L buffer solution consists of 0.173 M butanoic acid and 0.299 M sodium butanoate. Calculate the pH of the solution following the addition of 0.060 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-. pH =
A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)