Suppose you want to make a buffer with a pH of 6.90. Which of the following acid/conjugate base pairs should you choose? O HOCI and OCI- (K3 = 3.5 x 10-8) O HF and F- (K, = 6.6 x 10-4) %3D HSO4 and SO,2 (K, = 1.2 x 10-2) %3D O CH5CO2H and C,H5CO2" (K, = 6.5 x 10-5) %3D

Suppose you want to make a buffer with a pH of 6.90. Which of the following acid/conjugate base pairs should you choose? O HOCI and OCI- (K3 = 3.5 x 10-8) O HF and F- (K, = 6.6 x 10-4) %3D HSO4 and SO,2 (K, = 1.2 x 10-2) %3D O CH5CO2H and C,H5CO2" (K, = 6.5 x 10-5) %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: Calculate the pH of a buffer system containing 3.0 M NH3 and 2.0 M NH CI. (K, of NH4, the acid in…

A: Check the formula to calculate the pH of the buffer system and use it to calculate the pH of the…

Q: A certain indicator, HA, has a K₂ value of 4.0 x 10-7. The protonated form of the indicator is blue…

Q: You have a buffer solution containing an acid, HA. The pKa of HA is 7.20 and its conjugate base is…

A: Here we are required to find the pH of the buffer solution.

Q: A certain weak base has a Kp of 7.30 x 10-7. What concentration of this base will produce a pH of…

A: We need to calculate the concentration of the weak base that has pH = 10.27

Q: An organic acid (HA) has a molecular weight of 100g/mol, a Kow = 5.6 and a K, = 2.7 x 10-2. If…

Q: Which of the following acids should be used to prepare a buffer with a pH of 3.4? CH3COОН, Ка - 1.8…

Q: i. First, identify the acid. It's either H2PO41 or HPO42. The acid is because it has the most acidic…

A: Answer-1 H2PO4- H2PO4- because it has more number of acidic hydrogens, that's why it will lose it…

Q: What concentration of sodium benzoate must be used to create a buffer solution with a pH of 5.63 if…

A: Use a udic buffer equation to get MOLARITY of sodium benzoate. Buffer mixture is defined as an…

Q: What concentration of NaF do you need to add to a 0.15M HF solution to get a buffer solution pH of…

Q: You want to prepare 100.0 mL of a buffer solution with a pH of 4.95 by mixing appropriate volumes of…

A: Given : pH of buffer solution = 4.95 Concentration of CH3CO2H = 0.10 M Concentration of CH3CO2Na =…

Q: 3-Calculate pH of a buffer solution made from 0.15 M formic acid and 0.12 M sodium formate. The Ka…

A: Formic acid solution is a weak acid. Sodium ion are neutral but formate ion is basic in nature so it…

Q: A buffer solution is prepared in which the concentration of pyruvic acid, HC;H3O3, is 0.300 M and…

A: The solution given is a buffer solution of monoprotic pyruvic acid and its conjugate base pyruvate.

Q: The values of Ka for hydrozoic acid (HN3) and hypobromous acid (HBrO) are given below. HN3 Ka = 1.9…

A: Given: HN3 Ka = 1.9 × 10-5 HBrO Ka = 2.0 × 10-9

Q: A certain weak base has a Kp of 7.40X . What concentration of this base will produce a pH of 10.18?…

Q: What is the pH of a buffer solution that is 0.34 M methylamine and 0.44 M methylammonium chloride?…

A: Given: The concentration of methylamine is 0.34 M. The concentration of methylammonium chloride is…

Q: |Ka for formic acid is 1.7 x 10-4 at 25°C. A buffer is made by mixing 425 mL of 0.428 M formic acid,…

A: Given: Ka of formic acid = 1.7×10-4 Concentration of formic acid (M1) = 0.428 M Concentration of…

Q: 4. Formic acid, HFor, has a K value of 1.8 x 104. You need to prepare 125 mL of a buffer hav- ing a…

Q: Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH…

Q: If a buffer solution is 0.290 M in a weak base (K, = 1.4 × 10-5) and 0.580 M in its conjugate acid,…

A: pH of the buffer solution is determined by the Henderson-Hasselbalch equation as shown below: pH =…

Q: What is the pH of a solution that is 0.75 M HF and 0.15 M NaF? The Ka of HF is 6.6 x 10-4

A: Given: Concentration of HF [HF]= 0.75 M Concentration of NaF [NaF]= 0.15 M Ka of HF is 6.6 x 10-4 To…

Q: The H2CO3/HCO3- buffer system is the major system used to control the pH of blood. What is the pH of…

Q: What ratio of CH₂NH₂ to CH₂NH₂* is needed to prepare a pH 10.10 buffer? (Kb for CH₂NH₂ is 4.4 × 104)…

A: Given :- pH of buffer = 10.10 Kb for CH₃NH₂ = 4.4 × 10⁻⁴ To calculate :- ratio of CH₃NH₂ to…

Q: Which of the following combinations would be the best to buffer the pH of a solution at…

A: pH range or buffer capacity of a buffer = pKa±1.

Q: How much solid sodium acetate (CH3COONa) is needed to prepare a buffer solution at ph 5 if you have…

Q: Which weak acid would be best to use when preparing a buffer solution with a pH of 8.40? an acid…

A: Buffer solutions resist any changes in pH upon the addition of an acid or base to the solution. The…

Q: Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or…

A: Henderson-Hasselbalch equation, Is an equation which shows the relationship between the pH and pOH…

Q: What is the pH of a solution made by adding 23.5 g of KC2H302 to 400 mL of 0.80 M HC2H302? (Ka for…

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: Calculate the pH of a buffer solution prepared by dissolving 0,48 mole of sodium fluoride (NaF) and…

A: Buffer solution is a type of solution which resist the pH change when small amount of acid or base…

Q: For 490.0 mL of a buffer solution that is 0.185 M in CH3CH₂NH₂ and 0.135 Min CH3CH₂NH3C1, calculate…

A: This is an basic buffer solution with amonium ion salt and amonia base

Q: Classify the following solutions as one of these types AND calculate the pH: strong acid, strong…

A: Given,a) 0.040 M NaF (Ka for HF = 7.2 x 10-4)b) 10 M HClO4c) A solution made by mixing 10.0 mL of…

Q: You are making a buffer solution in the lab by combining the weak acid H2PO4- with its conjugate…

Q: What is the pH of a buffer solution prepared by dissolving 0.10 mol of sodium acetate (NaC2H3O2) and…

A: Ka = 1.8 × 10-5 pKa = - log Ka = - log (1.8 × 10-5) = 4.745.

Q: What are the [H₃O⁺] and the pH of a propanoic acid–propanoate buffer that consists of 0.35 M…

A: First of all write the equation for given compound: CH3CH2COONa→CH3CH2COO-+Na+ CH3CH2OOH=0.15…

Q: n acid with K, n acid with K, = 3.2 × 10-7 n acid with K, = 2.5 × 10"* n acid with K, = 1.7 × 10-10…

A: As we know, buffer is the mixture of weak Acid/base with its conjugate base/acid. And pH range of…

Q: A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is…

Q: Calculate the pH of a buffer made by adding HCO2H (formic acid) and NaCO2H to water if at…

A: Given: At equilibrium, CO2H-=8.00×10-3 MHCO2H=2.50×10-4 M Ka = 1.77×10-4

Q: A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the…

A: We have to find pH of given buffer on addition of KOH

Q: What is the pH of a buffer solution that is 0.21 M methylamine and 0.20 M methylammonium chloride?…

A: The solution can be easily determined using the Handerson HasselBach equation- pOH = pKb + log…

Q: Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO₂H) and 0.15 M sodium…

Q: What is the pH of a buffer solution that is 0.13 M methylamine and 0.21 M methylammonium chloride?…

Q: At 22 ˚C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The…

A: Answer: For any sparingly soluble salt it is considered that all its dissolved quantity is in…

Q: The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood is HCO, /H2CO3,…

A: Given, pH of blood plasma = 7.40

Q: A certain weak base has a Kp of 8.60 × 10-'. What concentration of this base will produce a pH of…

A: Kb = 8.40x10-7 pH= 10.37 Concentration of base=?

Q: What is the pH of a 75.0 mL of a 0.1 M NH3 solution (Kb= 1.8 x 10- 5) when 100.0 mL of a 0.0.75 M…

A: Hello. There are multiple subparts in the question. The first three subparts have been solved. To…

Q: Calculate the pH of a buffer solution prepared by dissolving 0.78 mole of sodium fluoride (NaF) and…

Q: If you mix 125.0 mL of 0.50 M CH3CO2H with 75.0 mL of 0.83 M NaOH, what is the pH of the resulting…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Suppose you want to make a buffer with a pH of 6.90. Which of the following acid/conjugate base
pairs should you choose?
O HOCI and OCI- (K3 = 3.5 x 10-8)
O HF and F- (K, = 6.6 x 10-4)
%3D
HSO4 and SO,2 (K, = 1.2 x 10-2)
%3D
O CH5CO2H and C,H5CO2" (K, = 6.5 x 10-5)
%3D

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

Write the buffer equilibrium reaction, then write the neutralization reaction. What isthe pH of the 0.20M NH3/NH4CL buffer after the addition of 10.0 mL of 0.10 HCl to65.0 mL of buffer? The Ka for NH3 is 5.6 x 10-10
Which weak acid would be best to use when preparing a buffer solution with a pH of 9.80? an acid with K₂ = 2.5 x 10-5 a an acid with K₂ = 2.0 x 10-6 a an acid with K₂ = 1.0 × 10-¹1 an acid with K₁ = 1.7 x 10-10 a an acid with Ka = 2.5 × 10-8 an acid with K₂ = 3.2 x 10-7 a
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.7
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.).
What is the pH of the buffer that results when 2.3 g of NH3 and 6.46 g of NH4Cl are dissolved in 250 mL water? (Ka for NH4+ = 5.60 × 10-10) Please give the answer to 2 decimal places.
Maps [References] Suppose you want to make a CH3 COOH/CH;COO¯ buffer solution with a pH of 5.11. The acetic acid concentration is to be 0.27 M. What should the acetate ion concentration be? (pK,(CH3 COOH) = 4.74.) %3D Concentration %3D
The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.
A buffer solution is made that is 0.415 M in CH3COOH and 0.415 M in CH3COO- . (1) If Ka for CH3COOH is 1.80×10-5 , what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.103 mol HI is added to 1.00 L of the buffer solution. Use H3O+ instead of H+ .
For 250.0 mL of a buffer solution that is 0.290 M in CH3CH2NH2 and 0.210 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 0.022 mol of NaOH . ( Kb(CH3CH2NH2)=5.6×10−4 .) What is the initial and final pH?
Formic acid, HFor, has a K, value of 1.8 x 104. You need to prepare 125 mL of a buffer hav- ing a pH of 3.25 from 0.10 M HFor solution and a 0.10 M NaFor solution. How many mL of NaFor and HFor should be mixed to make the desired buffer?
What is the pH of a buffer solution consistig of 0.035 M NH3 and 0.050 M NH4 + ? (Ka for HN4+ = 5.6 x 10-10)
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