You are interested in making a buffer with a pH of 7.30. Which of the following weakacid/conjugate base pairs would be most suitable to use?acidH3PO4HCO₂HCH3CO₂HH₂PO4NH4HCO3HPO4²-conjugate baseH₂PO4HCO₂CH3CO₂HPO4²-NH32-CO3²-PO4³-OHCO₂H/HCO₂OCH3CO₂H/CH3CO₂H₂PO4/HPO42-NH4 /NH32-HCO3 / CO3²-pka2.163.754.757.219.2510.3312.32

You are interested in making a buffer with a pH of 7.30. Which of the following weak acid/conjugate base pairs would be most suitable to use? acid H3PO4 HCO₂H CH3CO₂H CH3CO₂ HPO4²- H₂PO4 + NHA HCO3 HPO4²- conjugate base H₂PO4 HCO₂ NH3 CO32- 3- PO4³- HCO₂H/HCO₂ OCH3CO₂H/CH3CO₂ H₂PO4/HPO42- NHA/NH3 OHCO3/ CO3²- pka 2.16 3.75 4.75 7.21 9.25 10.33 12.32

You are interested in making a buffer with a pH of 7.30. Which of the following weak acid/conjugate base pairs would be most suitable to use? acid H3PO4 HCO₂H CH3CO₂H CH3CO₂ HPO4²- H₂PO4 + NHA HCO3 HPO4²- conjugate base H₂PO4 HCO₂ NH3 CO32- 3- PO4³- HCO₂H/HCO₂ OCH3CO₂H/CH3CO₂ H₂PO4/HPO42- NHA/NH3 OHCO3/ CO3²- pka 2.16 3.75 4.75 7.21 9.25 10.33 12.32

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: determine the pH of the resulting solutions when the 2 reagents are mixed together. 15.00mL of…

A: Given - 1. Molarity of NH3 = 0.1000 M Volume of NH3 = 15.00 mL Molarity of HCl = 0.10000 M Volume of…

Q: Ka = [H3O*] when the concentration of the acid equals the concentration of its conjugate base in a…

A: For an acidic buffer, using the Henderson-hasselbalch equation, pH= pKa + logA-HA

Q: You are given three unknown solutions. One is strongly acidic (pH below 1), one is neutral, and one…

A: pH indicators are added in small amount to solutions so that they can indicate their pH by showing…

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

A: pH + pOH = 14 pH = -log[H+] pOH = -log[OH-] For a weak base solution: [OH-] = (kb × C)1/2 Given…

Q: A solution is made by adding 52.0 mL of 0.230 - M acetic acid (Ka = 1.8 times10^-5) to 52.0 mL of…

Q: Which makes a buffer solution? a weak acid + a weak base b weak base + the salt of the weak base…

A: Buffer solution- buffer solutioh is chemial solution is a chemical solution which consists of a…

Q: Salts are composed of both cations and anions, both of which can potentially affect pH. Which of the…

A: When a salt is added to water it breaks into cations and anions or nothing and gives hydroxide…

Q: pH = 6.9 small can be neutralized can not be neutralized is not dissolved large Reset Help When…

A: Buffer solution — A solution which prevents change in pH on adding small amount of any acid or base…

Q: What is the effect on the concentration of ammonia, hydroxide ion, and ammonium ion when the…

A: Le chatelier's principle states that if a reaction at equilibrium is disturbed by changing…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: Consider a buffer solution comprised of HF and F-. The Ka of HF is 6.3 x 10-4. If the pH of the…

A: Weak acid are those acid which does not dissociate completely in aqueous solution. Here HF is weak…

Q: When mixed in equal molar amounts, which of the following pairs of substances would create a buffer?…

A: The objective of the question is to identify which pair of substances, when mixed in equal molar…

Q: Which of the following are considered buffer solutions Group of answer choices NH3/NH4+ HF/F-…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: One of the buffers that contributes to pH stability in human blood is carbonic acid (H2CO3).…

A: If the pH of the blood increases the buffer will act in such a way that reduces the pH. It is the…

Q: What is the concentration of conjugate base in a buffer that has a pH=6.39 and a Ka=4.66×10−5.…

A: Given that, Concentration of [H+] in a buffer =4.07×10-7 M Ka value of weak acid = 4.66×10−5. Then,…

Q: Each of the systems below has a total volume of 100 mL. Which of the systems would be able to…

A: A buffer is a solution that cannot change the even after the addition of an acid or a base.To find…

Q: Buffer 2 will be 150 mL of 0.15 M Tris-HCl buffer with a pH of 8.5 Write out the chemical equation…

A: The objective of the question is to write out the chemical equation for a Tris-HCl buffer and…

Q: You plan to make a buffer solution with sulfurous acid (H₂SO) and it undergoes dissociation reaction…

A: Henderson-Hasselbalch equation is used to prepare a buffer solution of desired pH: Desired pH is…

Q: What

A: Dear student I have given answer to your question in the image format.

Q: Consider the weak acid H2A and its Conjugate base HA-. Which diagram below represents a buffer…

Q: Identify each of the following substances as a strong acid, a weak acid, a strong base, a weak base,…

Q: Each of the systems below has a total volume of 100 mL. Which of the systems would be able to…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Use only species chosen from those listed below: NH4+ NH3 H2O H3O+ OH− (a)…

Q: If one mole of each of the following are dissolved in one liter of water which solution would have…

A: Given: Number of moles of given acids and bases= 1 mole The volume of the solution= 1 L To find: The…

Q: When mixed in equal molar amounts, which of the following pairs of substances would create a buffer?…

A: The objective of the question is to identify which pair of substances, when mixed in equal molar…

Q: Calculate the pH of the solution that results following addition of 10 mL of 1 M NaOH to 40 mL of 1…

A: Given: The objective is to calculate the pH of the solution 1M NaOH to 40mL of 1M NH4 Cl Formula…

Q: A prepared buffer solution contains a mixture of H2PO4 and HPO ions. Which species will react with…

A: The objective of the question is to identify which species in a buffer solution will react with any…

Q: Classify the following salts as acidic/basic/pH neutral and write a hydrolysis equation for them…

A: The salts given are NaNO3 CsF NH4Cl KCl Ba(CH3COO)2 CH3NH3I

Q: What component do you need to add to H2CO3 to make a buffer? H2O OH- H3O+ HCO3-

A: Buffer is a solution which resists the change in pH of a solution by the addition of small amount of…

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

You are interested in making a buffer with a pH of 7.30. Which of the following weak
acid/conjugate base pairs would be most suitable to use?
acid
H3PO4
HCO₂H
CH3CO₂H
H₂PO4
NH4
HCO3
HPO4²-
conjugate base
H₂PO4
HCO₂
CH3CO₂
HPO4²-
NH3
2-
CO3²-
PO4³-
OHCO₂H/HCO₂
OCH3CO₂H/CH3CO₂
H₂PO4/HPO42-
NH4 /NH3
2-
HCO3 / CO3²-
pka
2.16
3.75
4.75
7.21
9.25
10.33
12.32

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 :

VIEW

Step 2: Explanation :

VIEW

Solution

VIEW

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

n 5 of 20 > Attemp Calculate the pH of the solution that results from mixing 74.0 mL of 0.061 MHCN(aq) with 26.0 mL of 0.022 M NaCN(aq). The K₂ value for HCN is 4.9 x 10-10 pH = Incorrect Calculate the pH of the solution that results from mixing 28.0 mL of 0.024 M HCN(aq) with 72.0 mL of 0.053 M NaCN(aq). pH = I Incorrect Calculate the pH of the solution that results from mixing 44.0 mL of 0.101 M HCN(aq) with 44.0 mL of 0.101 M NaCN(aq). pH = Question Source: Atkins 7e-Chemical Principles | Publisher: W.H. 60°F 9 40 Is . a 9:41 PM 5/27/2022 PgDn Ins F3 m 4 R F $ O B 16x F4 Incorrect 10 % 5 T G F5 10 A 6 F6 Y H PrtScn F7 & 7 U Home F8 * 00 8 End K F9 ( 9 PgUp F10 ) 0 P F11 F12 =
Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base? The pH will always be greater than 7, regardless of the acid and conjugate base. The pH of the solution will be equal to the pKa of the acid. The pH of the solution will be equal to Kw. The pH will be equal to the concentration of the conjugate base. The pH will be equal to the concentration of the acid.
Buffer 2 will be 150 mL of 0.15 M Tris-HCl buffer with a pH of 8.5 Write out the chemical equation for this buffer. Identify which species is the conjugate acid and conjugate base.
Calculate the pH of each of the following buffered solutions: a) 0.25 M acetic acid CH3COOH (Ka = 1.8 x 10-5) and 0.10 M sodium acetate CH3COONa b) 0.50 M C₂H5NH2 (Kb = 5.6 x 104) and 0.50 M C₂H5NH3C1
Calculate the pH of a solution that is prepared by mixing 25.0 g HC2H3O2 and 25.0 g NaC2H3O2 in 800.0 mL solution (Ka HC2H3O2 = 1.8 x 10-5)
A 14.3 mL solution of 0.100 mol L-1 HF is titrated using 0.150 mol L-1 NaOH. What is the pH of the solution after 5.98 mL of the NaOH solution is added? Express your answer to 2 decimal places. ka of HF is 6.3x10-4
What is the pH of a buffer solution that is 0.26 M propionic acid and 0.54 M sodium propionate? Ka(propionic acid)=1.3*10^-5 pH = ?
What is a description of the salt that is used in a buffer solution? from the conjugate base from a weak acid O from the conjugate base of a weak base from the conjugate acid of a weak acid O from the conjugate acid of a strong base
Which of the following titrations is the MOST feasible? O NAOH versus NaHCO3 O NH4CI versus HCI O HI versus KOH O acetic acid versus ammonia
by the addition of strong base in a buffer, pH of the solution is maintained by? 1- Shifting equilibrium toward right side 2- Shifting equilibrium toward left side 3- by producing weak acid and more H ions 4- by producing conjugate base and more OH ions
Describe how you would prepare a 250.0 mL buffer solution that has a pH of 7.40 and has a H2PO4 − concentration of 1.0 M. You only have the following materials available. Materials/Chemicals: 1 L jug of deionized water 250.0 mL volumetric flask 500 mL bottle of 1.0 M H3PO4 500 g bottle of NaH2PO4 500 g bottle of Na2HPO4 500 g bottle of Na3PO4 500 g bottle of HF
Which of the following combinations of substances, when combined in roughly equal amounts, will create a buffer solution? NaC₂H3O2 and NaCl HF HNO2 HCIO4 and KCIO4 HNO3 and NaNO3 HNO3 H2O LICIO and HCIO