Answered: If the Ka of the conjugate acid is 4.39…

Science

Chemistry

If the Ka of the conjugate acid is 4.39 × 10-8 , what is the pKb for the base?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 8RQ: For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in...

See similar textbooks

Related questions

Q: Explain what happens to the concentration of hydrogen ions in anaqueous solution when you add a base…

A: The pH of a solution depends upon the concentration of hydrogen ion present in the solution. The…

Q: The pH of a half-neutralized solution of a weak acid is 4.3. What is the dissociation constant (Ka)…

Q: On acidity and basicity of aqueous solutions, the following relationships are valid, except…

A: Given : We have to tell the incorrect statement.

Q: What is the ratio of concentrations of acetate ion and undissociated acetic acid in a solution that…

A: Ethanoic acid is a weak acid and the dissociation of acetic acid is given by: CH3COOH ⇌ CH3COO-…

Q: What is the pH of a solution consisting of 0.85M HC2H3O2 and 0.60M NaC2H3O2? Given: Ka of HC2H3O2 =…

Q: A weak acid has Ka of 4.82 x 10-5. What is pKa for this weak acid? Enter a numerical value in the…

A: Given: Ka = 4.82 × 10-5

Q: Amphetamine (C,H13N) is a weak base with a pKp of 4.2. Part A Calculate the pH of a solution…

A: 1-Phenylpropan-2-amine is amphetamine. Its molecular mass (M) is 135.23 g/mol Concentration of…

Q: Calculate the Ka of weak acid. The initial concentration of the weak acid is 4.93 x 10-4 M. The…

Q: The Ka of a weak acid is 3 x 10^-12 What is the pKa of this acid?

A: Ka which is dissociation constant of acid is given 3*10^-12 Pka = ?

Q: A weak acid has a Ka of 2.5×10^-5. What is the Kb of its conjugate base? Which is stronger, the…

Q: What is the Kb for the conjugate base of an unknown acid with a Ka of (7.1x10^-3)

Q: A 0.3 M solution of a weak acid, HA, has an [H30*] of 0.002 M. What is the Ka of the acid, HA?…

A: Dissociation of acid is HA + H2O --------> H3O+ + A- the relation between concentration of H+ or…

Q: Calculate the percent ionization of ascorbic acid (HC6H7O6) in solutions of each of the following…

Q: A solution is prepared from two weak acids, 0.2 M HA and 0.1 M HB. If the Ka of HA is 1x10-5 and the…

A: pH - It is the negative logarithm of the hydronium ion concentration of a solution. Equilibrium -…

Q: Determine the pH

A: The scale which is used to analyze the acidity and basicity of an aqueous solution is called as pH…

Q: Calculate the pH of a solution that is 0.214 M acetic acid and 0.152 M sodium acetate. The Ka of…

Q: Hydrogen cyanide, HCN, also called hydrocyanic acid is a weak acid with a pKa near 10. What would be…

Q: at 95 ℃ water has an autoionization constant (Kw) of 4.518 X 10-13. Determine the ph of pure water…

A: Given :- Kw at 95°C = 4.518 × 10-13 To determine :- pH of pure water at 95°C

Q: Suppose 0.0013 mol HA and 0.0013 mol A− are present in 170. mL solution and the pH is 4.00. What is…

A: We have to calculate the acid dissociation constant value.

Q: The Ka of acetic acid is 1.80 x 10-5. A. What is the pH of a 0.0010 M solution of acetic acid? B.…

Q: What is the ratio of conjugate base to undissociated acid for a weak acid with a pk, of 4.4 at a pH…

A: Given : pKa = 4.4 pH = 9 To determine : Ratio of conjugate base to weak acid

Q: If acetic acid has a Ka of 1.8 x 10-5, what would be pH corresponding to the half-equivalence point…

Q: 7. The ka for acetic acid is 1.0 x 10.5. Is acetic acid a weak or a strong acid?

A: Strong acids completely dissociate in aqueous solution (Ka > 1, pKa < 1).

Q: calcualate the pH of a 0.15 M solution of pyruvic acid ka of pyruvic acid is 4.1x10^-3

A: Given: Molarity or concentration of pyruvic acid = 0.15M Ka of pyruvic acid = 4.1 × 10-3

Q: If the Ka of the conjugate acid is 7.68 × 10-4 , what is the pKb for the base?

A: Applying relationship between ka and kb Ka× kb= Kw

Q: A weak acid solution with concentration 0.020 M has a pH of 3.7, what is the pKa of this acid?

A: Given pH = 3.7 Initial Concentration = 0.020 M

Q: What is the value of pKb for the cyanide anion, CN- at 25⁰C? Ka(HCN) = 6.2 ´ 10^-10?

Q: Determine whether the statements are true or false. ( a. The stronger the base, the smaller the pKp.…

A: The pH scale range and the acid character of an acid or base can be known using Pka and PKb or just…

Q: If the Ka of the conjugate acid is 2.78 × 10-7 , what is the pKb for the base

A: Based on Bronsted theory, whenever a base accepts a proton that is H+, the formation of conjugate…

Q: Acetic acid has a Ka = 1.8 x 10- 2 points 5 Determine the pH of a O.2 M acetic acid solution *…

Q: A weak acid, HA, has a pK, of 4.047. If a solution of this acid has a pH of 4.313, what percentage…

Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is…

A: Sodium acetate is a salt of weak acid (CH3COOH) and strong base(NaOH).CH3COONa → CH3COO- +…

Q: The Henderson-Hasselbalch equation for the reaction can be written as : pH = pKa + log ([A–]/[HA])…

A: The Henderson-Hasselbalch equation for the reaction can be written as : pH = pKa +log[salt][acid]…

Q: If the Ka of a weak acid is 1.6 x 10-8, the Kb of its conjugate base partner must be which of the…

Q: A weak acid has KA = 1.59 x 10-8. What is the pKB of its conjugate base?

Q: A 0.500M solution of a weak acid has a pH of 2.251. a. What is the pKa of the weak acid?

A: Given data Concentration of weak acid : C = 0.500 M pH of solution = 2.251 We know that for a weak…

Q: If a weak acid has a Ka of 2.04 x 10-7 what is the value of pKb?

A: Given Ka value of weak acid = 2.04 × 10-7 PKb = ?

Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. What is the…

Q: What is the pH of a 0.639 M solution of lactic acid? The pKa of lactic acid is 3.854.

Q: The concentration of an unknown acid is 1.2M with a pH of 1.60. What is the pk the acid?

Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is…

A: Kb for the acetate ion is determined as follows,

Q: Codeine 1C18H21NO32 is a weak organic base. A 5.0 * 10-3M solution of codeine has a pH of 9.95.…

A: Given: Concentration of the solution=5.0×10-3M pH=9.95 To find: The pKb for the base.

Q: Calculate the expected pH of a 0.100 M acetic acid solution. Ka for acetic acid is 1.76 x 10-5…

A: Given data, Concentration of acetic acid = 0.100 M Ka for acetic acid = 1.76 × 10-5

Q: The Keq for the reaction: A + B ↔ AB is 2.03 What is the Keq for AB ↔ A + B Keq = ?

A: The equilibrium constant, Keq for the reaction: A + B ⇌ AB is 2.03 The equilibrium constant, Keq…

Q: What is the pH of an acetic acid solution with a K a of 1.76 x 10 -5 of 0.05 M?

A: Given K a of acidic acid 1.76 x 10 -5 of 0.05 M

Q: The pK, of a particular weak acid is 5.17. What is the pH of the weak acid solution when exactly…

Q: How many milligrams of CH3COOH (fw 60) should be added to 250 mL of water to get pH 3. K. = 1 x 10-5

A: CH3COOH is weak acid in aqueous solution. It will dissociate in solution as below-

Q: The Ka of acetic acid is 1.8 X 10-5. The Kb of the acetate ion is

A: Acetic acid is a weak acid and its conjugate base is acetate ion. The reaction of conjugate acid-…

Q: Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5.

A: Given,Concentration = 0.461M.Ka = 6.5×10-5Then,

Q: Calculate the pH of a 0.05 mol dm3 CH;COOH solution: the dissociation constant Ka for CH;COOH is…

A: An acid which will not dissociate completely to furnish hydrogen ion is called weak acid

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

If the K_a of the conjugate acid is 4.39 × 10^-8 , what is the pK_b for the base?

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 with 1 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

The Ka of a weak acid is 3.33 x 10-5, what is the pKb of it's conjugate base?
COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
If the concentration of an acid in solution is 2.3 times larger than the concentration of its conjugate base, and the pH of the solution is 4.9, what is the pKa of the acid?
A weak acid has KA = 1.59 x 10-8. What is the pKB of its conjugate base?
The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial concentration of the acid if the pKa of the acid 5.74?
An aqueous 0.6 M solution of a weak base has pOH of 4.5, what is the pKb of the weak base?
CH3CH2CO2H , Ką = 1.3 x 105 CH3CH2CO2 , Kp = 7.7 x 10-10 F, Kp = 1.4 x 10-11 HF , Ką = 7.2 x 10-4 For the reaction between propanoic acid (CH3CH2CO2H) and a solution containing fluoride ions (F"): (a) The name of the conjugate base produced is (b) The name of the conjugate acid produced is (c) The reaction is favoured (write 'reactant' or 'product'), because the reactants are the (write 'weaker' or 'stronger') set of acid and base.
(a) Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .
Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.
(c) Calculate the pH of 0.5 mol/L sodium hydrogen carbonate, NaHCO3. The Ka,1 of carbonic acid, H₂CO3, is 4.3 x 10-7. Нансез END
8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)
If a weak acid has a Ka of 2.04 x 10-7 what is the value of pKb?