Q7. Given the following Ka values for the weak acids and bases:CH;COOH/CH3CO0HCO3/CO32-H2PO4 /HPO,2Ка 1.8 х 105Ka = 5.6 x 10:11Ka = 6.2 x 108Which of the pair(s) would be appropriate as a buffer at pH = 7.0? Explain your answer.

To find the pair that will be appropriate as buffer of given range we use the buffer range of each…

Q7. Given the following Ka values for the weak acids and bases: CH;COOH/CH3CO0 HCO3/CO,2- H2PO4 /HPO,2- Ка 1.8 х 105 Ka = 5.6 x 10:11 Ka = 6.2 x 108 Which of the pair(s) would be appropriate as a buffer at pH = 7.0? Explain your answer.

Q7. Given the following Ka values for the weak acids and bases: CH;COOH/CH3CO0 HCO3/CO,2- H2PO4 /HPO,2- Ка 1.8 х 105 Ka = 5.6 x 10:11 Ka = 6.2 x 108 Which of the pair(s) would be appropriate as a buffer at pH = 7.0? Explain your answer.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 5ALQ: Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong...

See similar textbooks

Related questions

Q: Fill in the blanks: Aldosterone is the main mineralocorticoid steroid hormone produced by the zona…

A: Carbon has valency 4 so it can form four bonds with other atom. The degree of substitution can be…

Q: 2. Balance the following redox reactions in acidic solution a Fe2* + Cr,0,2- + H* → Fe* + Cr** + H,O…

Q: How momy grame of amimmium oxalate 'must be added to 500g of water to 7owver. the freezing point of…

Q: A solution is made by mixing 44.0 mL of ethanol, C, H,O, and 56.0 mL of water. Assuming ideal…

A: mass of substance = volume of substance x density of substance According to the Raoult's law Vapor…

Q: Calculating 12.49 mg. KI in 104.5mL of solution

A: Molarity is the ratio of moles of solute to volume of solution in litres.

Q: 1. In the chromatography plate there are three solutes that move forward: 2cm, 2.5cm and 3cm Which…

Q: You are given 2 stock solutions of 1M acetic acid and 1M sodium acetate. You are asked to prepare…

A: We will use dilution formula, Mi Vi = Mf Vf Mi & Mf -- Intial and final Molarity Vi &…

Q: 7. Decide whether each of the following will cause an aqueous solution to be acidic, basic, or…

Q: The reagent is incorrect to produce the product below. LINH3 CH;C=CCH, H CH3 A) True B) False…

A: ->Li/NH3 is reducing agent which can reduce internal alkyne to trans alkene. ->NaNH2 is base…

Q: D. Draw and name all the isomeric trichlorobenzenes (molecular formula C6H3CI3). If your answer is…

Q: Indicate the hybridization number of the numbered carbon atom. 1-10

A: Indicate the hybridization number of the numbered carbon atom. 1-10

Q: The oxidation of nitrogen oxide produces nitrogen dioxide, as shown below: 2NO (g) + O2 (g) → 2NO2…

Q: 4. What is the concentration of the solution prepared by diluting 250µl of ampicillin (5mg/ml) to a…

Q: How many moles are in 78.9g of HCl?

Q: 15. How many minutes would a current of 20.0 amps need to run through a solution containing Au*3 to…

A: Given that: Current = 20.0 A = 20.0C/s Mass of Au = 10.0g

Q: give two position isomers of the molecule that has the following molecular formula:C5 H10

Q: What is 3-tert-butyldecane structural formula?

Q: 1. In combination with molybdenum, the cobalt(II) sulfide is used as a catalyst in the industrial…

A: Given, Solubility of cobalt(ll) sulfide = 0.38 gL

Q: 7. Calculate the specific heat of gold if it required 48.0 joules of heat to warm 25.0 grams of gold…

Q: 2. Balance the following redox reactions in acidic solution a Fe2* + Cr,0,2- + H* → Fe* + Cr* + H,O…

Q: the symbol for the state its in

A: Recall the given reaction, 3 Cl2 g + 2 Cr3+ aq + 14 OH- aq → 6 Cl- aq +…

Q: I tried question #4 of answer of covlent bond it was incorrrect. For #1 I tried of covlent and got…

A: 1. The bond strength of a covalent bond is measured by the bond energy. The bond energy is the…

Q: 5. Calculate the heat release when 266 grams of white phosphorus P4 burns in air according to the…

A: Here we have to convert the gram of P4 to mole. And we have to multiply the number of mole of P4…

Q: Description The graph below shows how the mass of copper deposited during electrolysis varies…

A: A question based on tools in analytical chemistry that is to be accomplished.

Q: Select the INCORRECT statement. Select one: O a. All matter exhibits properties of both particles…

Q: Deoxyadenosine monophosphate (dAMP) and guanosine monophosphate (GMP) are nucleotides. The…

Q: Without performing detailed calculations, determine the hydrate of Na2SO3 that contains almost…

A: Given that, Na2SO3 that contains almost exactly 50% H2O by mass Determine the hydrate compound

Q: Consider the titration of 40.0 mL of 0.200 mol/L HCOONa (aq) with 0.300 mol/L HCl (aq). Ka for HCOOH…

Q: is the new concentration of the solution? 2. You start with 2.5L of a KNO3 stock solution and…

A: As per our guidelines, we are supposed to answer only one question with three sub parts. Kindly…

Q: Give the reaction mechanism (showing curly arrows) for the bromination of methane in the presence of…

A: Organic reactions are those in which organic reactant react to form organic products.

Q: DMF (solvent) Br + Cs F H20 acetone + KI Br A H3C-I + : P(Ph)3

Q: 1. Determine the oxidation number of each element in these substances: a. S203 b. O2 c. Al:(SO.)3

A: The overall oxidation number of a neutral compound is equal to zero. The oxidation number of oxygen…

Q: Can you please help me draw all the isomers?

A: Isomer are compound which have same molecular formula but different structural formula Here we are…

Q: QUESTION 23 What is the sum of the coefficients (including implied 1's) after balancing the chemical…

Q: . The equation for the synthesis of ammonia is N 2 + 3H 2 à 2NH 3 . How many moles of H 2 are needed…

Q: [1] CH3OH, H* е. CH30 HO, [2] MgBr (2 equiv) [3] H20 HO [1] SOCI2 [2] CH3CH,CH,CH,NH, [3] LIAIH4 [4]…

A: The reactions has been answered below

Q: Which of the following solids has the highest melting point? O Cao O CaF2 O Mgo O MgCl2

A: Given, Which of the following solids has the highest melting point ? a). CaO b. CaF2 c. MgO d.…

Q: 5. In the system 2A + B > 2C K=4.25 x 106, the initial concentrations are A = 2.25 M, B = 3.50 M,…

A: Concept: For a general reaction aA +bB ==== cC +dD The equilibrium constant can be given that K…

Q: O Give the IUPAC names of the following alkyl halides: Br (b) çI ÇH3 (c) CH3 CH;CHCH;CH;CI…

A: Detail description is given below

Q: Given incomplete reaction is : CH4 + Cl2, hv ------------> (a). Predict products and write…

A: The given reaction is the photochlorination of methane, which is a free radical substitution…

Q: A 0.030 M aqueous solution of a sodium salt (NaA) has a pH of 8.23. What is the value of K, for the…

A: The correct answer is given below

Q: 1) 12, NaOH, H20 2 OH + ICH3 2 2) Hо* Draw a detailed mechanism with arrows showing the movement of…

A: Here we are required to show the mechanism for formation of benzoic acid from1,3 diphenyl…

Q: Why is there a need to specify regioselectivity and stereospecificity when dealing with products…

Q: What is the pH afte

Q: considering the following peptides: Phe-Tyr-Ala-Lys-Glu-Asp the amino acid constituents that will…

A: Phe: 1 protonable group NH3 at pKa = 9.24 Tyr: 1 protonable group R at pKa = 10.07 Ala: 0 protonable…

Q: 16. For Nis) + 2H* (? M) H2 (1 atm) Ni*2 (1 M) E = .01v Calculate the pH of the solution.

A: Given reaction: Ni(s) + 2H+(aq) → H2(1 atm) + Ni2+(1 M) E = 0.01 V We have to calculate the pH of…

Q: PROBLEM 2: Find the percent of each component in a 0.4740g of propanediiodic acid and aniline…

Q: Applying the Bronsted Theory, complete the reaction and label each substance an acid or pase: HCO31…

A: According to Bronsted theory, A species that accepts a hydrogen is called Bronsted acid and a…

Q: Match the following terms with their definitions amorphous [ Choose ] [ Choose ] solid material that…

A: Amorphous : solid material that does not have a regular repeating…

Q: Is the answer only one for this problem?

A: Three membered rings formed by two carbon and one oxygen atom is known as epoxide ring. The…

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

Q7. Given the following Ka values for the weak acids and bases:
CH;COOH/CH3CO0
HCO3/CO32-
H2PO4 /HPO,2
Ка 1.8 х 105
Ka = 5.6 x 10:11
Ka = 6.2 x 108
Which of the pair(s) would be appropriate as a buffer at pH = 7.0? Explain your answer.

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 by step

Solved in 2 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

Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.