Answered: 25) Which one of the following is not a…

25) Which one of the following is not a conjugate acid-base pair? a) NH, and NH, c) HS and H,S b) Н.о-and OH d) NH, and NH;

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter17: Acid-base(proton Transfer) Reactions

Section: Chapter Questions

Problem 16E

See similar textbooks

Related questions

Q: From the following compounds identify the bases and explain, with the aid of diagrams, why they…

Q: 2. Illustrate using an equation, the meaning of the terms: conjugate acid and conjugate base. Give…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: We can ignore the contribution of water to the concentration of OH− in a solution of the following…

A: Concept introduction: A weak base can ionize partially to form OH- ions and respective anion. The…

Q: Derive equations that define a0, a1, a2 and a3 for the triprotic acid H3X

A: In the titration of acid H3X, changes in the concentration of various species can be visualized from…

Q: The weak acid, HA, has a Ka of 1.60 x 10-10. What is the Kb of its conjugate base, A™?

A: Given :- Ka for weak acid (HA) = 1.60 × 10-10 To determine : Kb of its conjugate base (A-)

Q: dissociated H+H+ ions

Q: Choose the correct answers from among the alternatives; For the sentence to be true: weak bases A)…

A: Applying concept of strength of bases with the help of electron pair donating capacity.

Q: CH3NH2 is a weak base (?b=5.0×10^−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a…

A: CH3NH3NO3 → NO3- + CH3NH3+ Kb for the above reaction is 5x10-4 CH3NH3 can donate a proton and…

Q: below B. For each acid above, write the balanced chemical reaction for the dissociation of a proton…

A: Dissociation of acids asked in question is shown below-

Q: 1. Identify the following as acidic or basic, and write the corresponding Ka or Kb reactions and…

A: Acid is a substance which release H+ ions and base is substance which release OH- ions

Q: What is the pH of a solution that has [OH"] = 8.31 x 10I M? Enter your answer with the correct…

A: Given that : [OH-] = 8.31 × 10-11 M To find: pH of the solution. It is known that pOH = -…

Q: Phosphoric acid, H3PO4 is a triprotic acid. pKaj= 2.16 pКа237.21 pКаз-12.32 2- Calculate the pH of a…

A: Phosphoric acid will ionize in aqueous solution as--

Q: The pOH of ammonium hydroxide at 25 C is 5.55. What is the pH and the [H ], [OH ] in mol/L for…

A: At constant temperature, the pH of a solution remains constant. For 250 C, the pH of the solution…

Q: Which of the following is a conjugate pair of acids and bases involved in the below reaction?…

A: Given reaction HCN + ClO- → HClO + CN-Conjugate pair of acids and bases = To be determined Acid…

Q: Which of the following would be considered a weak base? Solution A B C D % Dissociation 95 30 85 45…

A: Acids have pH level less than 7 and bases have pH more tha 7. Higher the pH stronger is the base…

Q: [H*] pH [OH'] pOH Acid or Base 1. 1х 106 2. 9 3. 4 x 10-6 4. 2.6

Q: Write complete Lewis structures of the molecules in the following reactions. Which is the Lewis acid…

A: Lewis structures of the molecules: a). In this reaction, NH3 acts as a Lewis base because, the…

Q: If the pH of a 25 °C NaOH solution is 9.00, what is the molarity of NaOH in that solution?

Q: 25. (a) What is a Brønsted-Lowry acid? (b) What is a Brønsted-Lowry base? (c) Use the following…

A: 25. (a) According to Brønsted-Lowry theory, an acid is a proton (H⁺) donor. (b) According to…

Q: 22. The conjugate base of CH3COOH is: A) H3O* B) CH3COO" C) OH D) H2O 23. The conjugate acid to NH3…

A: The correct answer about acid Base system is given below

Q: Identify the acids and bases in the following reactions: le) H (a) CHyCH, + TICI, HyC-č-CH, + BHy…

A: Lewis acids are species that accept lone pair of electrons whereas base are the species that can…

Q: What is the pH of a soluti on prepared by dissolving 3.00 g of the weak acid HA (molar mass = 138.12…

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the…

Q: Which of the following species cannot act as a Lewis acid?

A: A Lewis acid is an electron pair acceptor. Lewis base is an electron pair donator. A comparison of…

Q: The pH of aqueous 0.10 M pyridine (C5H5N) ion is 9.29. What is the Kb of this base

A: Given , Concentration of pyridine (C) = 0.10 M pH of pyridine solution = 9.29 Dissociation constant…

Q: A weak base has K, = 2.2 × 10¬11. What is the value of K, for the conjugate acid? %3D K, =

Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…

Q: . The pH of a solution is 6.7. From this statement alone, can you conclude that the solution is…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Kb for ammonia (NH3) is 1.76 x 10-5 What is Ka for ammonium, its conjugate acid. (NH4+)

Q: The pH of a 0.501 M solution of the conjugate base, A-, of a weak acid, HA, is 11.10. What is the…

A: Given: pH = 11.10 [A-] = 0.501 M As pH = -log[H+] Thus, [H+] = 10-pH = 1011.10 = 7.9 x 10-12 M…

Q: dissociated H+H+ ions

Q: (a) Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-. (b) Give…

Q: For the reaction H2CO3 + H2O ↔ H3O+ + HCO3-, H3O+ is the conjugate base. true or false?

A: A conjugate base is formed when an acid loses a proton/ hydrogen ion.

Q: 5. For the following acids: i. Name the following acids. ii. Identify if it is strong or weak acid.…

A: Acid is a substance that is capable of donating a proton or hydrogen ion to the base.

Q: Of these shown molecules, identify the non-lewis base HO H20 SH

Q: Clearly indicate the acid and the conjugate acid in each of the following reactions and determine…

A: Equilibrium is favoured on the side where more stable product is formed. Positive charge is more…

Q: Calculate the pH at 25 °C of a 0.15M solution of lidocaine HCl (C14H2, NONH,CI). Note that lidocaine…

A: In this question, we want to determine the pH of the solution. You can see the calculation steps…

Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…

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

Q: Identify the molecules or ions below as Lewis acids, Lewis bases, or neither. If there is more than…

Q: Which one of the following cannot act as a Lewis base? A. Cr3+ B. CN- C. Cl- D. NH3 E. F-

A: According to Lewis theory of acids and bases, the bases are the species that donate lone pair of…

Q: The Kb for aniline (C6H5NH2) is 4.3 x 10-10. What is the pH of a 0.15 M solution of aniline?

A: From the ICE table, we have

Q: At 25 °C, how many dissociated OH ions are there in 1245 mL of an aqueous solution whose pH is 1.61?…

Q: At pH = 3.9, a weak acid has a concentration of 0.75 M. If the pKa = 4.5, what is the concentration…

Q: The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the…

A: Since for any acid and its conjugate base, the Ka and Kb respectively are related to each other as…

Q: 3. Designate the Lewis acid and Lewis base in each of the following reactions: ÇI CH, CH,-C-OH, ČH,…

A: Anything that occupies space and has mass is called matter. The matter may be classified into acids…

Q: The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature. What is the initial…

A: Weak acid or base are those substance which does not dissociate 100%. The value of degree of…

Q: The base protonation constant K, of ammonia (NH,) is 1.8 × 10¯³. Calculate the pH of a 1.1 M…

Q: What is the pH of a solution containing 0.055 mol L-1 HCOOH and 0.141 mol L-1 HCOO- ?

Q: The pH of 0.55 M aqueous solution ammonia HN3 at 25.0 degree C is 11.50. What is the value of Kb for…

A: NOTE : You have given HN3 instead of NH3. Since the pH is in basic zone, hence the specie will be…

Q: Caffeine (CHiON O2) is a weak base with a pKof 10.4. Calculate the pH of a solution containing a…

Q: If the pH of a 1.00-in. rainfall over 1800 miles^2 is 3.90, how many kilograms of sulfuric acid,…

A: Given: pH = 3.90Area= 1800 miles2Ka2 = 0.012.

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

25) Which one of the following is not a conjugate acid-base pair?
a) NH, and NH,
c) HS and H,S
b) H,O' and OH-
d) NH; and NH;

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

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

The following reactions illustrate Brnsted acid-base behavior. Complete each equation. a.HI(aq)+?H3O+(aq)+I(aq) b.NH3(l)+?NH4++NH2 c.H2C2O4(aq)+H2O(l)?+HC2O4(aq) d.H2N2O2(aq)+H2O(l)H3O+(aq)+? e.?+H2O(l)H3O+(aq)+CO32(aq)
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
Following is a structural formula for imidazole, a building block of the essential amino acid histidine (Chapter 27). It is also a building block of histamine, a compound all too familiar to people with allergies and takers of antihistamines. When imidazole is dissolved in water, proton transfer to it gives a cation. Is this cation better represented by structure A or B? Explain.
White vinegar is a 5.0% by mass solution of acetic acid in water. If the density of white vinegar is 1.007 g/cm3, what is the pH?
. Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?