In which of the following cases is water acting as a base under the Lewis definitions but not underthe Brønsted-Lowry definitions?O H2O + CN2 OH° + HCNO H2O + HF = H3O* + F°O H20 + PO,3= 20H¯ + H2PO4O H2O + Cu²* 2 Cu(H2O)2+

As per the definition, a Lewis base is the one that is capable of donating a lone pair of electrons…

In which of the following cases is water acting as a base under the Lewis defınitions but not under the Brønsted-Lowry definitions? O H20 + CN' 2 OH° + HCN O H20 + HF= H3O* + F° O H20 + PO,3-= 20H° + H2PO4 O H2O + Cu²* = Cu(H2O)²+

In which of the following cases is water acting as a base under the Lewis defınitions but not under the Brønsted-Lowry definitions? O H20 + CN' 2 OH° + HCN O H20 + HF= H3O* + F° O H20 + PO,3-= 20H° + H2PO4 O H2O + Cu²* = Cu(H2O)²+

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.108QE

See similar textbooks

Related questions

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: Acid : An acid is a chemical species that donates hydrogen ion H+ in aqueous solution. Based on the…

Q: Ką for phenol (a weak acid), CH5OH, is 1.00×10-10.

A: Weak acids acidic strength can be measured by Ka value When a weak acid HA dissolved in water…

Q: Identify the acid and the base in the following reactions. (Type your answer using the format CO2…

A: Concept: Acid: a chemical substance which can give proton(H+) in a chemical reaction known as acid.…

Q: Ką for acetic acid, CH3COOH, is 1.80×10°. Ką for nitrous acid, HNO2, is 4.50×104. Ką for hydrocyanic…

A: Given: Ka for acetic acid, CH3COOH = 1.80×10-5 Ka for nitrous acid, HNO2 = 4.50×10-4 Ka for…

Q: Identify the Bronsted-Lowry acid (A), base (B), the conjugate acid (CA), and conjugate base (CB) in…

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

Q: What is the ionization constant at 25 ∞C for the weak acid CH3NH3+ , the conjugate acid of the weak…

Q: From the following chemical reactions determine the relative Brønsted-Lowry base strengths…

A: According to Bronsted-Lowry concept base is any species that can accept a proton from another…

Q: Calculate the pH of 0.10 M NaOH at this temperature

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

A: In this question we will be dealing with salts of strong acid + weak base and salts of weak acid +…

Q: H,0 + HCN = H,0* + "CN a. Identify each species as a Brønsted acid or base. Select the correct…

A: The given reaction is : The specie which can donate a proton (or H+) is known as a Bronsted acid…

Q: What is the ionization constant at 25 °C for the weak acid (CH3)2 NH2 +, the conjugate acid of the…

A: The weak base given is (CH3)2NH. Conjugate acid of any weak base is produced when the base accepts a…

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

Q: 1) A conjugate acid is defined as 2) In the general ionization reaction: HX(aq) + H,0(1) H,0* +…

Q: In the reaction SnCl4 + 2Cl- = (SnCl6)2- which acts as the Lewis base?

A: We have to identify the Lewis base for the following given reaction SnCl4 + 2Cl- = (SnCl6)2- as…

Q: conjugate acid conjugate base K K.

Q: Ka for nitrous acid, HNO2, is 4.50 × 10-4. Ka for hydrofluoric acid, HF, is 7.20 × 10-4. Ka for…

Q: The following aqueous species constitute two conjugateacid-base pairs. Use them to write one…

Q: Ka for acetylsalicylic acid (aspirin), HC9 H7O4, is 3.00 × 10-4. Ka for hydrofluoric acid, HF, is…

A: According to Bronsted-Lowry acid base theory, an acid is a compound which liberates proton (H+) to…

Q: The base protonation constant K₁ of lidocaine (C14H21 NONH) is 1.15 × 10 Calculate the pH of a 0.88…

A: Step 1: The base lidocaine (C14H21NONH) is a weak base, which is obvious from its small value of the…

Q: Which of the following can be classified as a Lewis base? BH3 O I only II, III, and IV O I and II O…

A: Lewis bases are those compounds which has lone pair of electrons to donate. Lewis acids are those…

Q: Ka for acetic acid, CH3COOH, is 1.80x105. Ką for benzoic acid, CgH3COOH, is 6.30×105. Ka for…

A: Acid dissociation constant: Ka, CH3COOH is 1.8 * 10-5 Ka, C6H5COOH is 6.3 * 10-5 Ka, HClO is 3.5*…

Q: The base protonation constant K, of morpholine (C¸H,ONH) is 2.14 × 10 °. Calculate the pH of a 1.0 M…

Q: Arrange the following acids in order of decreasing strength: 1. NH4+ , Ka-5 .6 x 10^-10 2. HCI02, Ka…

Q: The base protonation constant K, of lidocaine (C4H, NONH) is 1.15 x 10 °. Calculate the pH of a 0.55…

A: Given, kb = 1.15 * 10-8 Concentration of solution = 0.55 M Temperature = 25◦c

Q: Carbon dioxide (CO2) will react with an oxide ion (O2-) to form CO32- CO2 + O2- --> CO3^2- whixh…

A: The species which can accept a pair of electrons is known as Lewis acid. The species which can…

Q: Calculate the pH of a 0.218 M solution of NaNO₂. The ionization constant, K,, for the acid, HNO₂, is…

A: Molarity of NaNO2 = 0.218 M Ka for HNO2 = 4.60×10-4 pH of NaNO2 solution = ?…

Q: Calculate the percent ionization of a 0.437 M solution of hypochlorous acid. (Assume that Ka (HClO)…

Q: The base protonation constant K,, of allantoin (C H₂N₂O₂NH₂) is 9.12 x 10 Calculate the pH of a 0.25…

Q: Write the conjugate base of the two acids below and identify which base is stronger. C6O2H8, Ka =…

A: Interpretation- conjugate base. Concept introduction- Equilibrium constant (K) is ratio of…

Q: The base protonation constant K, of lidocaine (C14H„NONH) is 1.15 × 10°. Calculate the pH of a 0.86…

A: Given, Kb of lidocaine, C14H21NONH = 1.15 × 10-8 Concentration of lidocaine = 0.86 M

Q: Ka for 8 K, for nitrous acid, HNO₂, is 4.50 x 10. K, for benzoic acid, C6H5COOH. is 6.30 × 10-5. 4…

A: For a simple dissociation of a acid HA: The equation of equilibrium constant or, acid dissociation…

Q: Balance the following equations FeBr3 + H2SO4 Fe2(SO4)3 + HBr C2H4 + O2 CO2 + H2O Identify each…

Q: Which would you expect to be the better Lewis base, C^4- or Si^4-? Explain.

A: Species which can donate electron/s or electron density is called lewis base. And electron donation…

Q: The base protonation constant K, of lidocaine (C4H2]NONH) is 1.15 × 10 °. Calculate the pH of a 1.3…

A: Kb - It is the base dissociation constant. It tells us up to how much extent a base dissociates and…

Q: Suppose the pH of a neutral aqueous solution is not equal to 7. What must be true? The tempeature of…

A: Any aqueous solution has two competing ions ( H3O+ & OH- ions ) which indicate acidity &…

Q: [H+] = .0001 [H+] = 0.0030 [ОН-]— 8.6 е -8 РОН %3D 4.9 pH = 7.3 II At 37 degrees C, which of these…

A: We have to predict the solution that is nearly neutral.

Q: In the laboratory, a general chemistry student measured the pH of a 0.532 M aqueous solution of…

Q: K₂ for benzoic acid, C6H5COOH, is 6.30 × 10-5. K₂ for nitrous acid, HNO2, is 4.50 × 10-4. Ka for…

A: Acidic strength = An acid is said to be strong if it's Ka value is high i. e. more is the Ka value…

Q: Assuming identical concentrations and temperatures, which of the following weak bases would be…

A: Approach to solving the question: Detailed explanation: Examples: Key references:

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

In which of the following cases is water acting as a base under the Lewis definitions but not under
the Brønsted-Lowry definitions?
O H2O + CN2 OH° + HCN
O H2O + HF = H3O* + F°
O H20 + PO,3= 20H¯ + H2PO4
O H2O + Cu²* 2 Cu(H2O)2+

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 3

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

Follow the directions of Question 65 for the following bases: (a) SO32- (b) CHO2- (c) NO2-
12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’
Write equations that show H2PO4- acting both as an acid and as a base.
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.
Using the BrĂ¸nsted-Lowry model, write equations to show why the following species behave as weak acids in water. (a) Ni(H2O)5OH+(b) Al(H2O)63+(c) H2S (d) HPO42-(e) HClO2 (e) Cr(H2O)5(OH)+
To measure the relative strengths of bases stronger than OH, it is necessary to choose a solvent that is a weaker acid than water. One such solvent is liquid ammonia. (a) Write a chemical equation for the autoionization of ammonia. (b) What is the strongest acid and base that can exist in liquid ammonia? (c) Will a solution of HCI in liquid ammonia be a strong electrical conductor, a weak conductor, or a nonconductor? (d) Oxide ion (O2) is a stronger base than the amide ion (NH2). Write an equation for the reaction of O2 with NH3 in liquid ammonia. Will the equilibrium favor products or reactants?
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?
Using your results from Exercise 133, place the species in each of the following groups in order of increasing base strength. a. OH, SH, SeH b. NH3, PH3 c. NH3, HONH2
Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
For solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesnt change). a. [H+] b. pH c. [OH] d. pOH e. Ka
Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. Li2O b. CO2 c. SrO
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