The pK₂ value for HF is 3.14. Would a buffer prepared from HF and KF with a pH of 2.64 be considered to be an effective buffer? A buffer in which the mole ratio of KF to HF is 0.41 has a pH of 2.75. Would this buffer solution have a greater capacity for added acid ( H3O+) or added base ( OH)?

The pK₂ value for HF is 3.14. Would a buffer prepared from HF and KF with a pH of 2.64 be considered to be an effective buffer? A buffer in which the mole ratio of KF to HF is 0.41 has a pH of 2.75. Would this buffer solution have a greater capacity for added acid ( H3O+) or added base ( OH)?

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: 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: What is the pH of the buffer solution that contains 2.0 g of NH4Cl in 250 mL of 0.050 M NH3? Is the…

A: Buffer solutions are designated as alkaline buffer solutions and acidic buffer solutions. Given…

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: A chemistry graduate student is given 300. mL of a 1.10M dimethylamine ((CH3)2NH) solution.…

Q: What is the pH of a buffer system that contains 0.200 M hydrocyanic acid (HCN) and 0.150 M sodium…

A: Given : Concentration of hydrogen cyanide (HCN) = 0.200 M Concentration of sodium…

Q: nate (Na2CO3)corresponds to the following values: 0.53 M. (Ka for HCO3− is 5.6 ×10−11.) Report…

A: Ka = 5.6×10-11 pKa = -log(Ka) = -log(5.6×10-11) = 10.25 1) As it is Acidic buffer, pH = pKa +…

Q: The pK value for HF is 3.14. Would a buffer prepared from HF and KF with a pH of 4.94 be considered…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base. It…

Q: A buffer can be prepared from a weak acid, HA, and it's conjugate base, A⁻. A 1L solution is…

A: Given data,[HA]=0.2M[A-]=0.1MpKa=7.5Molarity of KOH=1MVolume of KOH=50mL0.05LVolume of buffer=1L

Q: Calculating the composition of a buffer of a given pH A chemistry graduate student is given 500. mL…

Q: A benzoic acid-sodium benzoate buffer is prepared by dissolving a certain amount of sodium benzoate,…

A: A buffer solution is an aqueous solution. It consist of a mixture of a weak acid and its conjugate…

Q: A buffer solution contains formic acid and a salt solution containing sodium formate. What is the pH…

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

Q: A buffer solution is prepared by dissolving 1.00 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: Given: The concentration of acetic acid is 0.100M. The volume of acetic acid is 100 mL. The…

Q: Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid…

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

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

Q: IS IS If Kal for H2S is 1.00 x 10, what is the pH of the buffer solution? pH = Write the net ionic…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: 6. A buffer solution contains 0.1OM benzoic acid (C,H5COOH, Ka = 6.3 x 10) and 0.10M potassium…

A: pH can be calculated by using henderson equation pH = pka + log (salt/ acid) Pka = - log 6.3 x10-5…

Q: What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml…

A: Given -> Volume of formic acid = 300 ml Molarity of formic acid = 1.65 M = M1 Volume of sodium…

Q: A chemistry graduate student is given 125. mL of a 0.30M pyridine (CHN) solution. Pyridine is a weak…

A: The concentration of pyridine = 0.30 MThe Kb for pyridine = Mass of = ?

Q: You prepare a buffer by mixing 0.15 mol propanoic acid (pKa = 4.87) and 0.25 mol sodium propionate.…

A: Mole of propanoic acid = 0.15 molMole of sodium propionate = 0.25 molpKa = 4.87 Mole of NaOH = 0.025…

Q: A chemistry graduate student is given 250. mL of a 1.70M nitrous acid (HNO₂) solution. Nitrous acid…

Q: Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of…

A: Given that, Ka for CH₃COOH is 1.8 × 10-5

Q: A hydrofluoric acid buffer is commonly used for systems that require a pH of about 3.00. Calculate…

A: The volume of buffer solution V = 100 mL Concentration of HF CHF = 0.14 M Concentration of KF CKF =…

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

Q: A buffer solution is made that is 0.402 M in HF and 0.402 M in KF. If Ka for HF is 7.20 x 10-4 what…

Q: A chemistry graduate student is given 250. mL of a 0.30M chloroacetic acid (HCH,CICO,) solution.…

A: We have to calculate the mass of salt added.

Q: A chemistry graduate student is given 450. mL of a 0.40M acetic acid (HCH3CO2) solution. Acetic acid…

Q: Which acid, along with it's corresponding salt, would be best to make a buffer of pH 7? hydrofluoric…

A: Given pKa = -log KaHydrofluoric Acid = Ka = 6.8 × 10-4pKa = 3.2Hypochlorous Acid = Ka = 3.5 ×…

Q: What quantity in moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb…

A: The objective of this question is to find out the quantity in moles of CH3NH3Cl that needs to be…

Q: A buffer is composed of 0.200 M HC2H3O2 (Ka = 1.8 × 10–5) and 0.250 M NaC2H3O2. What is the pH of…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

Q: A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) 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

The
pK₂ value for
HF is 3.14. Would a buffer prepared from
HF and
KF with a pH of 2.64 be considered to be an effective
buffer?
A buffer in which the mole ratio of
KF to
HF is 0.41 has a pH of 2.75. Would this buffer solution
have a greater capacity for added acid (
H3O+) or added base (
OH)?

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

Step 2

Step 3

Final answer

Step 5

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

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.
The pK₂ value for HCN is 9.40. Would a buffer prepared from HCN and NaCN with a pH of 7.60 be considered to be an effective buffer? A buffer in which the mole ratio of NaCN to HCN is 2.0 has a pH of 9.71. Would this buffer solution have a greater capacity for added acid ( H3O+) or added base (OH)?
A buffer is formed by adding 1.0 mol of dimethylamine, (CH3)2NH, and 1.0 mol of dimethylammonium, (CH3)2NH2+, in a 1.0 L container. If a 10.0 mL sample of this buffer is diluted to 1000 mL with water, what is the pH of the diluted buffer?For dimethylamine, Kb = 5.4 × 10-4Insert your answer in decimal notation rounded to 2 decimal digits.
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
What quantity in moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) to make a buffer with a pH of 11.50?
A buffer solution is made that is 0.323 M in НаСОз and 0.323 м in NaHCOз. If Kal for H2CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.089 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +
A chemistry graduate student is given 250.mL of a 0.30M propanoic acid HC2H5CO2 solution. Propanoic acid is a weak acid with Ka=1.3x10^−5. What mass of KC2H5CO2 should the student dissolve in the HC2H5CO2 solution to turn it into a buffer with pH=4.30? You may assume that the volume of the solution doesn't change when the KC2H5CO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
9 If the dissociation constant of a weak acid is 1.4 x 10-5, at what ratio should you adjust the concentration of the weak acid and its conjugate base in order to prepare a buffer that has a pH of 4.85? a) 0.100 M weak acid with 0.0100 M conjugate base b) 0.0100 M weak acid with 0.100 M conjugate base c) 0.100 M weak acid with 0.200 M conjugate base d) 0.300 M weak acid with 0.300 M conjugate base e) 0.500 M weak acid with 0.250 M conjugate base
-4 = A chemistry graduate student is given 500. mL of a 0.20M nitrous acid (HNO₂) solution. Nitrous acid is a weak acid with K = 4.5 × 10 What mass of NaNO₂ should the student dissolve in the HNO₂ solution to turn it into a buffer with pH = 3.46? You may assume that the volume of the solution doesn't change when the NaNO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. [] x10 Ś
An analytical chemist is titrating 74.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 1.200 M solution of KOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 36.1 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.
Calculate the pH of a buffer when 0.010 moles of NaOH is added to 100. mL solution that is 0.20 M sodium pentanoate (C HCOONa) and 0.20 M pentanoic acid (CH₂COOH). PK (CH₂ a COOH) = 4.82.
Calcium carbonate (limestone) is not very soluble in water. This low solubility is reflected in its small Ksp value (4.6 x 10-9). Ksp is the product of the equilibrium concentrations of the ions in a saturated solution of a salt. Calculate the solubility Ca2+ (in units of mg/L), assuming simple dissociation into the two ions for the dissolved CaCO3(s). Calculate the pH.