Answered: 38. In the reaction CH3COOH --> CH3COO…

38. In the reaction CH3COOH --> CH3COO + H* 2517 a. CH3COOH is the conjugate acid b. CH3COO is the conjugate acid C. H* is the conjugate acid d. CH3COOH is the conjugate base a

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: What is the pH of 0.055 M KOH solution? What is the pH of 0.55 M KOH solution What is the pH of a…

A: 1. Concentration of KOH = 0.55 M2. Concentration of Chloroacetic acid = 2 M3. Concentration of…

Q: Write the products of the following acid-base reaction. H₂C- OH OH You should include all products.…

A: Bronsted–Lowry acids and bases: According to this theory, an acid is a proton (H⁺) donor, and a base…

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

A: According to Bronsted-Lowry concept Acid is a species which can donate proton and forms its…

Q: Rank the acids shown in decreasing (strongest to weakest) order of acidity. ОН о ОН 7. F ОН НО = Br…

A: Given , Halogen derivative of carboxylic acid .

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

Q: (EA18) which one of the following is the strongest base? Why? TV. FO I. Học? II. NH H3C? III OH very…

A: Strong acid have weak conjugate base. Weak acid have strong conjugate base. Electronegativity or…

Q: For each mixture of acids, find the pH and [A- ] for each conjugate base. a. 0.185 M HCHO2 and 0.225…

A: pH of mixture of any two weak acids(1 and 2) can be determined by the formula- H+=c1k1+ c2k2

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

Q: 4. Give the products from the following acid-base reactions and identify the acid and base on the…

A: The given reactions are represented as follows:

Q: The cation of the salt of a strong acid and a weak base is the O conjugate base of the strong acid.…

A: an acid is a species which donates Proton while a base accepts proton.An acid after donating Protons…

Q: The pH of an aqueous solution that is 2.7 x 103 M HCI is . What is the pOH? Circle one: ACID or BASE…

A: Formulas :

Q: For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than…

A: the correct option are as follows:

Q: Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three…

Q: Consider the following reaction. The conjugate base of H3O' (hydronium ion) is a strong acid, strong…

Q: The Ka of an acid is known to be 1.51 X 10^-5. A solution is made by adding 0.279 mol of the acid to…

A: Hello, we are supposed to answer first three sub-parts of a question as per our solution authoring…

Q: In the following reaction, HCO; (aq) + H20(E)=co;²(aq) + H;0*(aq) Select one: O a. H3O* is an acid…

Q: Consider the weak acid reaction: HA + H2O H3O+ + A-1 and the reaction of its conjugate base: A-1…

A: The weak acid reaction is as follows: HA + H2O <-> H3O+ + A-1 The reaction of its conjugate…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

Q: A solution is found to have a pH of 8.72. What is the hydroxide ion (OH) concentration? s the…

A: If pH is greater than seven than solution is basic in nature.

Q: Consider the following data on some weak acids and weak bases: acid base Ka name formula name…

Q: Determine if the following substances act as an acid or base in the given reaction. 02- + so3 →…

A: Given, The chemical reaction, O2- + SO3 ---------> SO42-

Q: aqueous reaction. Identify the acid, the base, the conjugate acid, and the conjugate base. HOCl +…

A: In the Reaction, left side ( means reactant part ) acid and base are present. HOCl removed H(+) ion…

Q: If the conjugate acid of a pair is chlorous acid, then what is the name of the conjugate base? O…

A: given that, chlorous acid is a conjugate acid.

Q: 2. Suppose a 0.0500M solution of HNO, was created Write the dissociation reaction for this compound.…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: In addition to your recorded pH called make a table showing the corresponding [H3O+]values. Also…

A: We use the below formula to find [H3O+] from pH. [H3O+] = 10-pH

Q: Which of the following is a weak base? a. KOH b. NaOH c. Cd(OH)2 d. Ca(OH)2

Q: a. b. C. For each of the following aqueous reactions, identify the acid, the base, the conjugate…

A: Bronsted-Lowry acid- base theory : According to this theory an acid is a substance which donates H+…

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 × 10~7. Calculate the pH of a 4.0…

Q: a. A solution of HINO, has a pH of 3.57. What is the molarity of the solution? Molarity = M b. A…

A: pH = -log[H+] Log [H+] = -pH [H+] = 10-pH

Q: You have a 0.0100 M solution of a weak base, B. True or False. a. [OH-] = 0.0100 M b. [B] = 0.000…

A: Given : Weak base, B with concentration = 0.0100 M

Q: What is the conjugate base of H2SO4? * SO4 H2S03 O HSO3 HSO4- Which is defined as the loss of…

A: Given Acid = H2SO4 Conjugate base = ? Statement : Loss of electron from species Name of process =…

Q: < Weak Acid HCN HNO HIO HBrO CH₂COOH + K₂ 4.9 x 101⁰ 4.5 x 10 2.3 x 10¹¹ 2.5 x 10¹ 6.3 x 10° Which…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Identify acid, base, conjugate acid, and conjugate base in the following reactio a. H20 + H2CO3 =…

A: We know that acid is a substance that releases H+ ions in an aqueous solution. A base is a substance…

Q: The Ka for a weak acid is 1.2*10^-8. a. What is the equilibrium concentration of OH- in a 0.0020 M…

A: Given, Ka for a weak acid = 1.2 × 10-8 Molarity of its conjugate base = 0.0020 M Let the weak acid…

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

38. In the reaction
CH3COOH --> CH;COO + H*
a. CH3COOH is the conjugate acid
b. CH3COO is the conjugate acid
c. H* is the conjugate acid
d. CH3COOH is the conjugate base
O a
O b

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

Trending now

This is a popular solution!

Step by step

Solved in 2 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 sample of water from a stream has [H3O*]=3.1 × 10-9 M. Which statement below accurately describes this water sample? A. The water sample is acidic. B. The water sample is a basic solution. C. The pOH of the water sample is 8.50. D. pH of the water sample is much les than 7.0. E. The pH of the water sample is 7.5.
Consider the weak acid reaction: HA + H20 H30* + A and the reaction of its conjugate base: A + H20 + H2O HA + OH-1 Add the reaction together and write the net reaction. You do not need to include subscripts or superscripts. use the "=" sign for the arrow. [reaction] weak acid reaction and the conjugate base
1donsify the apid, base , conjugate acid and conjugate base in The follaing reachon HPOU t AzO > HO t Ag PO 4
Which of the following statement best explain why the acidity of carboxylic acids is greater than those of the alcohols? a. Alcohols behave as neutral compounds in aqueous solution. b. Alcohol has the ability to donate proton to becomes a negative ion called an alkoxide ion, RO– c. When a carboxylic acid donates its proton, it becomes a negatively charged ion, RCOO−, called a carboxylate ion which is more stabilized by resonance. d. The OH group in alcohol is less charged and often more difficult to release electron for chemical reactions.
When this reaction occurs H₂O + NH3 -> -OH + NH4+ Which of the following statements are correct? OH₂O is the Bronsted Lowry acid OH₂O is the Bronsted Lowry base ONH3 is the Bronsted Lowry acid ONH3 is the Bronsted Lowry base OOH is the conjugate acid OH is the conjugate base NH4 is the conjugate acid O NH4 is the conjugate base
Identify the correct acid/conjugate base pair in this equation: HCO3- is an acid and OH- is its conjugate base. H2O is an acid and HCO3- is its conjugate base. H2O is an acid and H2CO3 is its conjugate base. HCO3- is an acid and H2CO3 is its conjugate base. H2O is an acid and OH- is its conjugate base.
Calculate the pH of each of these solutions. is the solution acidic, basic, or neutral ?. a. a solution with a OH- concentration of 5.5 x 10-12 M b. a solution with a H3O+ concentration of 3.2 x 10-8 M c. a solution with a pOH of 7.00
Using the following K, values, calculate the pH values for each of these solutions (using 2 significant figures). [K, for acetic acid= 1.78x105; K, for phosphoric acid = 7.52x103K, for H₂CO3 = 4.3x107] A. A solution of 0.3 M acetic acid has a pH of B. A solution of 3 M acetic acid has a pH of i C. A solution of 100 mM phosphoric acid has a pH of D. A solution of 43 mM H₂CO3 has a pH of
Complete the table below. Be sure each of your answer entries has the correct number of significant digits. You may assume the temperature is 25 °C. conjugate acid formula H₂S HSO4 H₂ BO3 Ka 5.55 X 10 0.012 5.8 X 10 -8 -10 formula HS 2- SO 4 conjugate base K₂ B 1.8 × 10 8.33 × 10 -7 - 13 1.72 × 10 -5 × Ś x10
1. A solution of Ba(OH)2 has a [OH-] of 0.40 M. What is the initial molar concentration of the solution? 2. A solution of LiOH has a pH of 13.68. What is the initial concentration of the solution. 3. A solution of Hbr has a [OH-]= 5.0 x 10-12 M. What is the pH of the solution? 4. The [OH-] of CsOH is 0.025 M. What is the pH of the solution? 5. What is the initial concentration of a solution of CsOH with a ph=13.68? 6. A solution of HCl has a pOH=12.08. What is the initial concentration of the solution? 7. The Ka of acetic acid is 1.8x10-5 at 25 degrees C. What is the pH of 0.25 M CH3COOH? 8. The Kb of ammonia is 1.8 x 10-5 at 25 degrees C. What is the pH of 0.25 M NH3?
A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=7.2×10−5[H+]=7.2×10−5 M? B. What is the hydroxide ion concentration, [OH−][OH−], in an aqueous solution with a hydrogen ion concentration of [H+]=7.2×10−5[H+]=7.2×10−5 M? C. A monoprotic weak acid, HAHA, dissociates in water according to the reaction HA(aq)↽−−⇀H+(aq)+A−(aq)HA(aq)↽−−⇀H+(aq)+A−(aq) The equilibrium concentrations of the reactants and products are [HA]=0.120 M[HA]=0.120 M, [H+]=3.00×10−4 M[H+]=3.00×10−4 M, and [A−]=3.00 ×10−4 M[A−]=3.00 ×10−4 M. Calculate the ?aKa value for the acid HA.