1. Based on the given ionization constants, arrange the following solutions from leastbasic to most basic: (a) aniline Kb = 3.8 x 10-10(b) methylamine Kb = 4.4 x 104(c) caffeine Kb = 5.3 x 10-142. Which of the ff. oxoacids is weaker? HNO3 or HNO23. Consider the following acids and their ionization constant, determine which conjugatebase is stronger.(а) НСООН Ка %3D 1.7 х 104(b) HCN Ka %3D 4.9х 10-10

As we know, 1) higher the value of Kb , more is the basic strength. Increasing order C < A…

3.8 basic to most basic: (a) anline Kb (b) methylamine Kb = 4.4 x 104 (c) caffeine Kb = 5.3 x 10-14 ch of the ff. oxoacids is weaker? HNO3 or HNO2 sider the following acids and their ionization constant, base is stronger. (а) НСООН Ка%3D 1.7 х 10+ (b) НСN Ка- 4 0 10-10

3.8 basic to most basic: (a) anline Kb (b) methylamine Kb = 4.4 x 104 (c) caffeine Kb = 5.3 x 10-14 ch of the ff. oxoacids is weaker? HNO3 or HNO2 sider the following acids and their ionization constant, base is stronger. (а) НСООН Ка%3D 1.7 х 10+ (b) НСN Ка- 4 0 10-10

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 10RQ: For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen...

See similar textbooks

Related questions

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

A: NaClO is weak acid and H2SO4 is strong acid. So, it is acid base neutralisation reaction.

Q: 2. (a) For the following reaction equation, draw complete Lewis structures for both reactants and…

A: Note; "Since there are multiple sub-parts in this question and it is not mentioned that which one…

Q: 5. Identify the acid-base conjugate pairs in each of the following reactions: (а) СНЗСОО- + HCN…

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

A: The given incomplete reaction is NaClO aq+H2SO4 aq→. To write the complete balanced molecular…

Q: A:(-) + H₂O(+). For the following named acids: 1a) Consider the reaction AH+ + H₂O a) draw the…

A: Acidity is defined as the ability of a molecule to release protons.If a compound easily donates…

Q: Write the acid dissociation expression (kb) for the following reaction below: a) NH3 (aq) +…

Q: BH(+) + H₂O. For the following named bases: Consider the reaction B: + H3O+ draw the structure of…

A: Basicity is defined as the electron donation ability of a molecule. If it is able to donate…

Q: 2.40 As we will see in later chapters, many steps in key reaction sequences involve acid-base…

Q: Identify the acid and conjugate base pair in the following equation: (AKS 14b) HCIO4 + H2O → H3O* +…

A: In the given reaction HClO4 + H2O ------> H3O+ + ClO4- HClO4 is a strong acid which…

Q: Which of the following is an acid/conjugate base pair? (A) H3PO4/H2PO32- (B) H2SO4/SO42- (C)…

Q: Identify which of the acids below will yield the stronger conjugate base and why. а) НОСI (К, — 3.5…

Q: Which of the following is a hydrolysis reaction? F (aq) + H,O (1) S OH" (aq) + HF (aq) 2 None of…

A: In a hydrolysis reaction, the anion or cation or both of a salt reacts with water and gives hydrogen…

Q: 1. Identify the acid on the left and its conjugate base on the right in the following equations: (a)…

Q: Which one of the following correctly shows the weak acid equilibrium for formic acid, HCOOH? А)…

Q: CH3 „Ph Ph. „CH3 H-SO4 > (А), HSO4 (B) 9. OH Product (A) & (B) respectively in the above reaction…

Q: Asteltoxin, isolated from cultures of Aspergillus stellatus, exhibits a potent inhibitor on E. coli…

A: Most acidic proton is a proton which has the higher degree of positive character and the negative…

Q: Identify the Lewis acid and base in the following reaction. Using curved arrow formalism, show the…

A: Lewis acid is a species which is electron deficient in nature and therefore will accept a pair of…

Q: 18 Lổ -H 8. H-SO4 →(A). Product (A) of the reaction is : 018 (a) Ph – NH –C-Ph (b) Ph – NH –C -Ph OH…

A: This reaction is type of carbocationic rearrangement i.e. Beckmann reaction. Let see the reaction…

Q: HA has a pK₂= 9 and HB has a pKb = 11. Which acid is the stronger acid? (a) HA (b) HB b 3

A: We have been given that HA has pkb = 9 and HB has pkb = 11. We have to tell which acid is stronger…

Q: What is the relationship between Ka of the acid and Kb of its conjugate base?

Q: Write the formula of the conjugate acid of CH₂CO₂.

A: Answer:- This question is answered by using the simple concept of conjugate acid and conjugate base.…

Q: NH; (aq) + Hә0 () +—> NH} (ag) +он (ад)

Q: 4. A weak acid HA has Ka = 4.3 x 10-6. The ionization constant Kô for its conjugate base A- is: (a)…

A: Given that : Ka for HA = 4.3 x 10-6 We have to calculate Kb for its conjugate base A-.

Q: 14. Which of the following compounds can act as an Arrhenius, Bronsted, and Lewis base? (a) H₂O (b)…

Q: 1b) Consider the reaction B: + H3O¹ → BH + H₂O. For the following named bases: a) draw the structure…

A: Given is a box of bases. To find the conjugate acid of the bases and their pKa values. Concept:Base:…

Q: 14. Circle the most acidic compound in each of the following pairs. Explain your choice by…

A: The acidity of carboxylic acids depends on the stability of carboxylate ions.More stable the…

Q: Order these species in terms of increasing base strength: ClF, F¯, NH2- (A) Cl¯<F¯< NH2¯ (B) Cl-<NH2…

A: The species given are Cl-, F- and NH2-.

Q: Note: be sure each number you put in the table has the correct number of significant digits. Ka pK.…

A: pKa=10.9 Ka=? pKa = -logKa = 10.9 logKa = -10.9 Ka = 10^(-10.9) =1.25 ×10^-11

Q: Try to do this problem without consulting a table of acidity constants. Select the single best…

A: CH3-OH+ - CH3 is strong acid than protonated amine. Answer- Option 2

Q: What is the conjugate base of H,PO, 1) H,O+ (aq) 2) H,PO, (aq) 3) HPO,2 (aq) 4) PO, (aq) 4. -3

A: What is conjugate base of H2PO4- ?

Q: Predict the products of the following acid-base reactions, and predict whether the equilibrium lies…

A: Acids are proton donors and bases are proton acceptors. In an acid-base reaction, essentially a…

Q: estigate In the following acid-base reaction, H3O+ is the A HCI(g) + H₂O(1)→ H3O+(aq) + Cl-(aq)…

A: We know, base takes H+ to form conjugate acid and acid releases H+ to form conjugate base .

Q: Consider two acids: Cl,CHCO,H (dichloroacetic acid, pK,=1.3) and HCO,H (formic acid, pK, = 3.8).…

A: In this question, we will select the strongest acid. You can see details explanation and answer…

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

1. Based on the given ionization constants, arrange the following solutions from least
basic to most basic: (a) aniline Kb = 3.8 x 10-10
(b) methylamine Kb = 4.4 x 104
(c) caffeine Kb = 5.3 x 10-14
2. Which of the ff. oxoacids is weaker? HNO3 or HNO2
3. Consider the following acids and their ionization constant, determine which conjugate
base is stronger.
(а) НСООН Ка %3D 1.7 х 104
(b) HCN Ka %3D 4.9х 10-10

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

Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: HCI, HBr, HI. (b)basicity: H2O, OH-, H-, CI-. (c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (Hint: Formula could also be written as HCIO4). (d) acidity: HF, H2O, NH3, CH4
Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. In addition, write Lewis structures for all starting materials and products. Label the original acid and its conjugate base; label the original base and its conjugate acid. If you are uncertain about which substance in each equation is the proton donor, refer to Table 4.1 for the relative strengths of proton acids. (a) NH3+HCl (b) CH3CH2O+HCl (c) HCO3+OH (d) CH3COO+NH4+
Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: HO, 467 kJ/mol; HS, 363 kJ/mol; HSe, 276 kJ/mol) b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H c. NH4+, HONH3+ d. NH4+, PH4+ (bond energies: NH, 391 kJ/mol; PH, 322 kJ/mol) Give reasons for the orders you chose.
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?
How is acid strength related to the value of Ka? What is the difference between strong acids and weak acids (see Table 13-1)? As the strength of an acid increases, what happens to the strength of the conjugate base? How is base strength related to the value of Kb? As the strength of a base increases, what happens to the strength of the conjugate acid?
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a base, can we say there is no H+. since having H+ would imply that the solution is acidic?
Will 0.10 M solutions of the following salts be acidic, basic, or neutral? See Appendix 5 for Ka values. a. ammonium bicarbonate b. sodium dihydrogen phosphate c. sodium hydrogen phosphate d. ammonium dihydrogen phosphate e. ammonium formate
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
Hydrazine, N2H4 (having the structure H2NNH2), and its derivatives have been used as rocket fuels. Draw the Lewis electron-dot formula for the hydrazine molecule. Describe the geometries expected about the nitrogen atoms in this molecule. Why would you expect hydrazine to be basic? Which substance, NH3 or N2H4, would you expect to be more basic? Why? Write the chemical equation in which hydrazine reacts with hydrochloric acids to form the salt N2H5Cl. Consider the positive ion of this salt. How does its basic character compare with that of NH3 and N2H4? Explain.
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.
Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 13-2 and 13-3. a. NaNO3 b. NaNO2 c. C5H5NHClO4 d. NH4NO2 e. KOCl f. NH4OCl