Answered: Which of the following is not a…

Science

Chemistry

Which of the following is not a conjugate acid/base pair? a. HCN b. H₂SO4 C NHÀ d. H₂O+ CN SO₂² NH3 H₂O

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.52EP: Classify each of the following substances as an acid, a base, or a salt. a. AlPO4 b. KOH c. HNO3 d....

See similar textbooks

Related questions

Q: Which of the following is a strong acid? A. HNO3 B. H₂S C. HNO2 D. HOCI B O A C OD

A: Which of the following is strong acid ?

Q: Determine whether each salt forms an acidic, basic, or neutral solution when it dissolves in water.…

A: I am instructed to answer only three subparts please to repost for the rest.

Q: CH3COO- (aq) + H+ (aq) ⇔ CH3COOH (aq), is an example of ________. Bronsted base…

A: Acid base concept is given by Bronsted as well as Arrhenius . Arrhenius acid is that which…

Q: Which of the following is the formula for a weak acid? О А. НF B. HCIO4 C. H2SO4 O D. HNO3

A: Weak acid is partially dissociate into its ion in aqeous solution (I.e. water) . And strong…

Q: Select the pair of substances which is not a conjugate acid-ba O C. H2SO4, HSO4 O A. H3O*, H2O O E.…

A: The question is based on conjugate acid base principle. a strong acid has a weak conjugate base…

Q: 4. Which of the following is a strong acid? * O A. HNO3 Ов. Н2S O C. HNO2 O D. HCO3-

A: The strongest acid among the following has to be given,

Q: Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an…

A: In order to determine which species is acidic, basic or neutral, we must know the Bronsted Lowry…

Q: Based on their molecular structure, pick the stronger acid from each pair of oxyacids. Explain your…

Q: 22. A solution for which [OH-] = 3.0 x 10-10 is classified as a. acidic b. basic c. neutral

A: Given, [OH-] = 3.0 x 10-10 pOH = -log [OH-] pOH = -log[3.0 x 10-10] pOH = 9.52

Q: Which of the following ions will act as a weak acid in water? WHY? a. K+ b. Na+ c. H2PO42- d. NH4+

Q: Suggest the conjugate base of nitric acid, HNO₃. *

A: As HNO3 is a acid, therefore it will easily release H+ ion as this is the property of acids. To…

Q: 8. Which of these is a weak base? A. NaOH В. НРО C. CH3COOH D. NaHCO3 E. NH&NO3

A: A base is a compound which produces hydroxide ion in water. A weak base is that base which on…

Q: Which of the following is a strong base? a. CH3NH2 b. Ba(OH)2c. Cr(OH)3d. CH3COOH

A: A Base is a substance that can accept hydrogen ions (H+) or, more generally, donate a pair of…

Q: Determine if each anion acts as a weak base in solution. For those anions that are basic, write an…

A: Determine if each anion acts as a weak base in the solution. For those anions that are basic, write…

Q: 2. Write the acid-dissociation reaction for each of the acids below. a. HCOOH b. HSO4 c. H3PO3

Q: Identify each substance as an acid or a base and write a chemi- cal equation showing how it is an…

A: According to Arrhenius concept, an acid can be defined as an species which have the tendency to…

Q: Which acid is the strongest? a. HNO2 b. NH3 c. HF d. HClO4

A: Introduction : Strong acid is defined as which can donate H+ ions easily .

Q: Which of the following is NOT a conjugate acid-base pair? a. H2SO3/HSO3⁻ b. H3O⁺/H2O c. CO32-…

Q: Complete the reaction when ammonia is dissolved into water NH3 + H20 a. NH4*1 b. Он1 C. H30*1 d. H20…

A: Given, NH3 + H2O ------>

Q: Calculate the H3O+ and pH of each polyprotic acid solution. a. 0.350 M H3PO4 b. 0.350 M H2C2O4

Q: Identify each substance as an acid or a base and write a chemical equation showing how it is an acid…

A: Given-> (a) -> HClO4 (b)->Mg(OH)2 (c)->CH3COOH

Q: Write the formula for the conjugate base of each acid.a. HCl b. H2SO3 c. HCHO2 d. HF

A: A conjugate base is formed when a proton is removed from an acid.

Q: What is one set of conjugate acid-base pairs in this reaction? NH3(aq) + H2O(1) NH4"(aq) + OH (aq) O…

A: Conjugate acid-base pair Conjugate acid-base pair is determined based on Bronsted-Lawry theory.…

Q: Fill in the missing information in the following table. pH POH Solution a 9.69 a. b. с. d. Solution…

A: Given,a. pH = 9.69b. [ OH- ] = 3.3 x 10-6 Mc. [ H+ ] = 0.021 Md. pOH = 1.24

Q: In the reaction H2PO4- + H2O -> H3PO4 + OH-, Which pair represents an acid and its conjugate base?…

A: Within the Bronsted–Lowry acid–base theory, a conjugate acid is a chemical molecule generated when…

Q: . If 153.5 mL of CO2 are collected at 14°C, 723.0 torr, what will its volume be at STP? In a…

Q: HCO3– + H2O -> CO3–2 + H3O+ What role is water playing in the…

A: This question is based on the concept of acid-base reactions

Q: true

A: Given-The Conjugate base of a weak acid is stronger base than H2O

Q: Give the formula of the compound which will be dissolved in HNO3? STRONG ACIDS…

A: Solubility

Q: 4.The same number of moles of acetic acid and hydrogen chloride are placed in beakers containing…

A: Concentration of hydronium ion H3O+ present in the solution is known as pH of the solution.

Q: Give a possible value of [OH-] and [H3O+] in a acidic solution. A B [H,0] 107 [H,0]> 107 and…

A: ONE QUESTION TO BE ANSWERED AS PER BARTLEBY ANSWERING GUIDELINES, THANK YOU

Q: What is the H3O+ ion concentration in a solution with an OH– ion concentration of 4.2 × 10–3 M? Is…

A: [OH–] = 4.2 × 10–3 M [H3O+] = ..............? [H3O+][OH-] = 1.0 x 10-14 [H3O+] 4.2 X 10-3 M = 1.0…

Q: Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an…

A: a. Sr2+ + 2H2O -------> Sr(OH)2 + 2H+ It releases hydronium ion in aqueous solution , so…

Q: Calculate the [H3O+] and pH of each polyprotic acid solution.a. 0.350 M H3PO4 b. 0.350 M H2C2O4

Q: When each compound below is added to water, is the resulting solution acidic, neutral, or basic?…

A: Given compounds, a. CH3CH2OHb. Mg(OH)2c. C6H5CO2Hd. LiOHe. C3H7CO2Hf. H2SO4

Q: Classify each as a strong acid, weak acid, strong base, or weak base. a. HASO, b. Sr (OH)2 C. HIO d.…

A: The species that increase the concentration of hydrogen ions or hydronium in an aqueous solution act…

Q: Match the substance to its classification in aqueous solution. NH3 NH4Br 1. Weak acid HC,H5 2.…

A: Different type of compounds have different nature on dissolving them in water. Some of 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

Which of the following is not a conjugate acid/base pair?
a. HCN
b. H₂SO4
C. NHĩ
d. H₂O+
CN
SO₂²
NH3
H₂O

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: The main aim of the question

VIEW

Step 2: Analysing the each given options

VIEW

Solution

VIEW

Step by step

Solved in 3 steps with 23 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

Write a formula for the conjugate base formed when each of the following behaves as a Brnsted acid: a. HSO3 b. HPO42 c. HClO3 d. CH3NH3+ e. H2C2O4
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. HC3H3O3 b. HCN c. H2SO4 d. H2SO3
Which of the following substances are acids in terms of the Arrhenius concept? Which are bases? Show the acid or base character by using chemical equations. a P4O10 b Na2O c N2H4 d H2Te
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) HCO2H(aq) + H2O() HCO2(aq) + H3O+(aq) (b) NH3(aq) + H2S(aq) NH4+(aq) + HS(aq) (c) HSO4(aq) + OH(aq) SO42(aq) + H2O+()
Aluminum chloride, AlCl3, reacts with trimethyl-amine, N(CH3)3. What would you guess to be the product of this reaction? Explain why you think so. Describe the reaction in terms of one of the acid base concepts. Write an appropriate equation to go with this description. Which substance is the acid according to this acidbase concept? Explain.
2. The cyanide ion, CN−, accepts a proton from water to form HCN. Is CN− a Bronsted acid or base or is it amphiprotic? acid base amphiprotic
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Pure liquid ammonia ionizes in a manner similar to that of water. (a) Write the equilibrium for the autoionization of liquid ammonia. (b) Identify the conjugate acid form and the base form of the solvent. (c) Is NaNH2 an acid or a base in this solvent? (d) Is ammonium bromide an acid or a base in this solvent?
Classify each of the following substances as an acid, a base, or a salt. a. AlPO4 b. KOH c. HNO3 d. HC2H3O2
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. H3PO4 b. H3PO3 c. HBr d. HC2H3O2
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
Ethanol (ethyl alcohol), CH3CH2OH, can act as a BrnstedLowry acid. Write the chemical equation for the reaction of ethanol as an acid with hydroxide ion, OH. Ethanol can also react as a BrnstedLowry base. Write the chemical equation for the reaction of ethanol as a base with hydronium ion, H3O+. Explain how you arrived at these chemical equations. Both of these reactions can also be considered Lewis acid base reactions. Explain this.