When added to water, ethylamine undergoes the following reaction: C2H5NH2 + H2O C2H5NH3+ + OH- Is ethylamine an acid or a base in this reaction? Strong or weak? How do you know? 6. Name Ca(OH)2 and write its ionization equation.

When added to water, ethylamine undergoes the following reaction: C2H5NH2 + H2O C2H5NH3+ + OH- Is ethylamine an acid or a base in this reaction? Strong or weak? How do you know? 6. Name Ca(OH)2 and write its ionization equation.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter20: Organic Chemistry

Section: Chapter Questions

Problem 76QAP

See similar textbooks

Related questions

Q: Draw the Lewis dot diagram for CH3COOCH3 and CH3COOH. Which of the following compounds is an acid?…

A: Lewis dot structure is a digramatic representation of molecule, in which bonding and non bonding…

Q: a balanced net ionic equation for each of the following acid-base reactions in water

Q: Label acidic basic or neutral: (you will first need to find the pH) 3.9 x 10^-8M NaOH

Q: Propanoic acid, CH3CH2COOH, has a pKa =4.9. Draw the structure of the conjugate base of propanoic…

A: The conjugate base is a species formed when the hydrogen ion (proton) is lost from an acid during…

Q: Label acidic basic or neutral: (you will first need to find the pH) 9.5 x 10^-11 M NH3

A: As per the given data Concentration of NH3=9.5×10-11MpH=?

Q: In the reaction: CH3COOH(aq) + NH2– (aq) CH3COO– (aq) + NH3(aq), the conjugate acid-base pairs…

A: In the reaction : CH3COOH(aq) + NH2- (aq) →CH3COO-(aq) + NH3(aq) Acid loses H+ to form conjugate…

Q: In the laboratory, a general chemistry student measured the pH of a 0.428 M aqueous solution of…

A: pH of a 0.428 M aqueous solution of trimethylamine, (CH3)3N to be 11.731 Kb for this experiment is…

Q: If not, which direction does it need to move (right or left) to reach equilibrium? Explain.

A: For the reaction C6H5NH2(aq)+ H2O (l)------>C6H6NH3+(aq)+OH- Q= reaction coefficient =…

Q: A solution containing .30 M methylamine (CH3NH2) and .33 M methylamonium chloride (CH3NH3Cl) has a…

A: 1. Given that, Concentration of CH3NH2 = 0.33 M Concentration of CH3NH3Cl = 0.30 M pH of the mixed…

Q: Directions: Write the correct Lewis structure and show the step-by-step solution on how you came up…

A: The concept of covalent bond is explained Lewis. The atoms achieve stable octet configuration when…

Q: Calculate the pH of a 0.0470 M aqueous solution of the weak base methylamine (CH3NH2, Kb =…

Q: Label acidic basic or neutral: (you will first need to find the pH) 7.7 x 10^-7 M HNO3

A: Answer is explained below. Concentration of HNO3 is 7.7×10-7 M (Given). Thus, [H3O+] = 7.7×10-7 M.

Q: How does the acidity of hand soap at pH 10 compare to distilled water at pH 7? A. Hand soap is…

Q: Given the reaction: HPO4 2- (aq) + HC2H3O2 (aq) ↔ H2PO4 - (aq) + C2H3O2 - (aq) 1. The acid in…

A: According to Bronsted-Lowry Concept, An Acid is proton (H+) donor and when it is loses the proton it…

Q: Determine the pH and hydrogen ion concentration in a 0.1425M solution of ethylamine, C2H5NH2 at…

A: Here, we have to calculate the pH and hydrogen ion concentration in a 0.1425 M solution of…

Q: Gaseous methylamine, CH3NH2 , can be classified as __________. A Lewis base only…

A: 1- In this question, we will see the class/ nature of this base. You can see details solution…

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: Methyllithium (CH3Li) is often used as a base in organic reactions. What is the…

A: Given reagent, Methyllithium (CH3Li)

Q: Which of the following are acid-base reactions? 1. AGNO3(aq) + HCl(aq) AgCl(s) + HNO3(aq) 2. NH3(aq)…

A: According to Bronsted-Lowry concept of acids and bases Acid is a substance which donates proton…

Q: An aqueous solution of CH3NH3NO3 will be Group of answer choices A. basic, because of the…

A: Since the salt given CH3NH3NO3 is made from the acid HNO3 and base CH3NH2. And we know that the salt…

Q: Label acidic basic or neutral: (you will first need to find the pH) 1.0 x 10-4 M HBr

Q: n of 0.024M. C

A: pH measures the solution that how much solution is acidic and basic when pH is greater than 7 then…

Q: Calculate [OH-] of a 4.40×10-1 M aqueous solution of triethylamine ((C2H5)3N, Kb = 4.0×10-4).…

A: (C2H5)3N is a weak base. Hence it undergoes hydrolysis reaction in solution as, => (C2H5)3N (aq)…

Q: beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for arecoline in…

A: Structure of arecoline:

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: Which of the following acids has the weakest conjugate base? Chlorous acid, Ka = 1.1 x 10-2…

A: The strongest an acid , the weakest is its conjugate base. The acid which has highest Ka value is…

Q: When HBr reacts with equal moles of CH3NH2 is the resulting solution is Neutral Acidic Basic…

A: Substances that can liberate hydronium ions in solution is called an acid and those that release OH-…

Q: Complete the balanced molecular reaction for the following weak base with a strong acid: NaClO2(aq)…

A: Since we know that when sodium chlorite react with sulfuric acid to produce sodium sulfate, chloric…

Q: Complete the reaction by writing the formulas of the products. CH;COOH + NH, = The Ka of CH,COOH…

Q: Show how methanol (CH3OH) can serve as both an acid and a base. Write an equation for the reaction…

A: Those compounds that could acid as well as base is known as amphoteric acid.

Q: Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a solution that is 0.00298 M…

Q: Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer…

A: Given: Concentration of salt= 0.52 M pH of buffer solution = 10.1 Kb of ethylamine = 5.6×10-4

Q: Calculate the concentration of OH-(aq) in a solution in which [H3O+] is 2 × 10-6 M.

A: [H3O+] [OH-] = kw kw = 1 × 10-14

Q: Identify the correct base/conjugate acid pair in this equation: NH4+ + H2O -> NH3 + H3O+ A. H2O…

A: conjugate base is formed when an acid donates a proton. conjugate acid is formed when a base accepts…

Q: Classify K2O strong acid weak acid strong base weak base

A: Acid- The species which is able to donate H+ ion is called as acid. Bade The species which is able…

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

A: Given, a). 0.1 M KClO b). 0.1 M KNO3 c). 0.1 M C2H5NH3Cl d). 0.1 M NaF

Q: Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer…

A: Given: Kb of ethylamine = 5.6×10-4

Q: 2. Write the dissociation equation and equilibrium constant expression for the dissociation of the…

Q: Write a balanced equation showing how the HPO2-4 ion of sodium hydrogen phosphate Na2HPO4 can be a…

Q: Does the pH increase, decrease, or remain the same when each of the following is added? EXPLAIN:…

A: pH = -log[H+] So the concentration of H+ increases pH of the solution decreases while when…

Q: Label acidic basic or neutral: (you will first need to find the pH) 2.0 x 10^-6 M HBr

A: We have given that Molarity of HBr = 2.0×10-6 M We know that The pH of a solution is a measure of…

Q: If the pH of a 0.050 M solution of the acid HX is 2.0 and the pH of a 0.050 M solution of the acid…

A: Given : Concentration of HX = 0.050 M pH of HX solution = 2.0 Concentration of HY = 0.050 M And pH…

Q: Which of the following compounds will form a basic solution when dissolved in water? LiC2H3O2…

A: A salt made from strong base and weak acid give basic aqueous solution.

Q: What is the pH of a 0.10 M solution of ethylamine at 25º C? The pKb of ethylamine at 25º C is 3.25.…

A: Ethylamine is a weak acid so it dissociates partially.

Q: 5. Which of the following is a conjugate acid-base pall? H3PO4 and HPO²- HCO3 and CO2 NaOH and OH…

A: -> Conjugate base of an acid can be formed when hydrogen ion is removed from acid. -> For…

Q: Chemistry beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for…

Q: Calculate the pH of a 0.14 M solution of diethylamine

Q: A certain organic amine acts as a mono acid base in an aqueous solution. A 0.05M solution has a…

Q: Consider the following aqueous equilibrium. CH3CH2NH2(aq) + H20(1) = CH3CH2NH3*(aq) + OH (aq) What…

A: Since in the above reaction, the molecule CH3CH2NH2 is gaining 1 H+ to form CH3CH2NH3+ and H2O is…

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

100%

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 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

Show how methanol (CH3OH) can serve as both an acid and a base. Write an equation for the reaction of methanol with sulfuric acid.
Calculate the pH of a 0.14 M solution of diethylamine.
Consider the molecules R-CH2OH and R-CH2CO2H where R is rest of the hydrocarbon molecule. a) Which has the stronger conjugate base? b) Explain why it is the stronger base. What about the structure helps us to understand why one is stronger than the other? You may use drawings to help explain your answer.
Write the chemical equation for a pentanoate ion acting as base when it reacts with hydrochloric acid (HCI). Which is formula of this rule of reaction?
Write a net ionic equation to show that diethylamine, (C2H3)2NH, behaves as a Bronsted-Lowry base in water. BL base BL acid BL acid BL base H20 +
(HC(CH₂), CO₂) is 9.33 × 106. x Calculate the pH of a 2.8 M solution of trimethylacetic acid. Round your answer to 1 decimal place. The acid dissociation constant K of trimethylacetic acid pH = 0 X 5
Write a net ionic equation to show that piperidine, C5H11N, behaves as a Bronsted-Lowry base in water. BL base BL acid BL acid BL base + H2O +
Draw the Lewis dot diagram for CH3COOCH3 and CH3COOH. Which of the following compounds is an acid? Explain how you determined your answer. For the acid, indicate which of the hydrogen atoms is the acidic hydrogen? Then, explain why the hydrogen atoms in the other structure are not acidic.
Oil of wintergreen, commonly used externally to relieve muscular and joint pain, is the methyl ester of salicylic acid. Write an equation for its preparation from salicylic acid yes.
Write the neutralization reaction occurring between benzoic acid and NaOH. What is the stoichiometry of the reaction?
5. Given the general equation illustrating the reaction of the acid HA in water, HA(aq)+H2O(l)H3O+(aq)+A(aq)explain why water is considered a base in the Brønsted-Lowry model.
Acid-Base Equilibria Many factors contribute to the acidity of organic compounds. Electronegativity, resonance, induction, hybridization, aromaticity, and atomic size, all play a role. In the following comparisons, you are asked to identify the factor(s) that would be most important to analyze when predicting relative acidity, and then to predict the trend in acidity and pKa values. For each of the following pairs of compounds answer the following two multiple-choice questions. 1. What factor(s) are the most important to consider when predicting the relative acidity of the two compounds? a. Electronegativity of the atom possessing the hydrogen. b. Resonance stabilization of the anionic conjugate base. c. Inductive stabilization of the anionic conjugate base. d. Hybridization of the atom possessing the hydrogen. e. The atomic size of the atom possessing the hydrogen.