Answered: For each value of Ka, calculate the…

For each value of Ka, calculate the corresponding value of pKa. Which compound is the stronger acid? Q.) chloroacetic acid, Ka = 1.38 X 10-3

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 7ALQ: You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide...

See similar textbooks

Related questions

Q: Identify the weakest acid from the following data: a. Hydrofluoric acid K₂ = 6.7 x 10-14 b. Acetic…

A: In this question, we will see which acid is weakest acid. Acid strength is depends on Ka value of…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: The dissociation constant, Ka of acid, and pKa are related as follows: pKa = -log Ka The strength of…

Q: pKa

A: According to the question, we need to determine the conjugate acid of the molecule and then…

Q: Which compound in the following pair is the stronger acid? Select the single best answer. HO COH

Q: Using your knowledge of the Brønsted-Lowry theory of acids and bases, write equations for the…

A: Bronsted-Lowry theory- Acid: Compound which removes proton. Base: Compound which accepts proton.

Q: Which of the following acids has the strongest conjugate base? O A. succinic acid, Ka = 6.2 x 10-5…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: The three pKa’s for phosphoric acid (H3PO4) are 2.1, 6.9, and 12.4. At what pH does [H3PO4]…

Q: An acid has a Ka = 7.77 x 10-4. Is it stronger or weaker than an acid with Ka = 7.77 x 10-3 ? A.…

A: We have to compare the acid strength.

Q: Which of the following would represent the strongest acid? OK₁ = 2.5 x 10-5 O pk = 14.5 O pk = 4.60…

Q: 2.4 8 (a) Define in words the following: (i) Ka (ii) pKa (b) Calculate the pH of 0.0005 mol dm³…

A: Ka and pka both are represent the dissociation constant of acid. When acid are equilibrium we need…

Q: 2. In both instances below, order the acids by increasing pKa a) Al(OH)3 H3ASO, HCIO3 H3PO4 B(OH)3…

Q: If the Ka1 value of chronic acid (H2CrO4) is 0.16 and its Ka2 value is 3.2x10^-8, what is the value…

A: Given ; values of Ka1 and Ka2

Q: A weak base has Kp 6.5x10-6. Calculate the pKa of the conjugate acid. Express your answer to two…

A: The dissociation constant of an aqueous solution of weak acid is known as the acid ionization…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: Since pKa = -logKa Hence substituting the values we get A) pKa = -log(1.26 X 10-3) = 2.90 B) pKa =…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: Ka is known as acid dissociation constant. Larger the value of pka, lesser is the acidic strength.

Q: To what category of basicity does CrO42- belong? Select one: a. strongly or very strongly basic b.…

Q: 10. The Kb of pyridine (C5H5N) is 1.8 x 10-9. What is the Ka of pyridine's conjugate acid?

A: The reaction as follows,

Q: CI HO HO FF Но но Br 1 2 3 4 2. Arrange the following (using the numbers) in order of increasing…

A: The given molecules are :

Q: One way to determine the predominant species at equilibrium for an acid-base reaction is to say that…

A: The given data is:

Q: HA has a pka of 15, while HB has a pka of 5. The stronger acid is The stronger conjugate base is…

Q: List the bases from strongest to weakest Ammonia, Kb=1.8x10^-5 Dimethylamine, kb= 5.4x10^-4…

A: Kb…

Q: In the following reaction, identify the Lewis acid. (d) NH3 + CH3CO2H NH4 + CH3CO2 (a) CH;CO2 (b)…

A: The reaction taking place is given as, => NH3 + CH3CO2H -----> NH4+ + CH3CO2-

Q: (3 pts) For the following sets of compounds, place the compounds in order of increasing acidity, and…

A: Acidity is measured as strength to loose a H atom or H+ ion. (a) The increasing order of acid…

Q: Weak acids do not dissociate completely in water and have pKa values of - 3 or higher. Which of the…

A: Given acids, A. HNO3 B. HCl C. H2SO4 D. H2CO3

Q: Assuming that base (B:) and acid (AH) are mixed in equal concentrations and using pka values of acid…

A: pKa for AH = 4.7 pKa = -log Ka Ka = 10-pKa Ka1 = 10-4.7 = 2×10-5 pKa for BH+ = 5.1 Ka2 = 10-5.1 =…

Q: 2. Out of the following, which is incorrect? a) The Ka of an acid-base pair conjugate characterizes…

Q: Which of the following acids has the weakest conjugate base? Chlorous acid, Ka = 1.1 x 10-2…

A: The strongest an acid , the weakest is its conjugate base. The acid which has highest Ka value is…

Q: The pKa of ascorbic acid (vitamin C, page 55) is 4.17, showing that it is slightly more acidic than…

A: Introduction: The acid or base form after the losing or gaining a proton is called conjugate acid…

Q: (a) Given that Kb for ammonia is 1.8 x10-5 and that forhydroxylamine is 1.1 x 10-8, which is the…

A: (a) The Ka and Kb are the dissociation constants of acids and bases respectively. Hence, higher the…

Q: What is the approximate pKa value of acetic acid? Is it protonated or not at pH -10? At pH 7? Please…

A: The pKa is calculated as : pKa = - log10(Ka) where Ka is the acid dissociation constant

Q: (b) Calculate the pH of 0.0005 mol dm-3 ethanois acid when its pKa = 4.75 CH3COO (a H(a + CH;COOH()…

Q: Pyridine is a weak base with K, = 1.7x10-10. %3D C3H5N(aq) + H20) C5H5NH" (aq) + OH Write the K…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

Q: assign the acid its appropriate pKa

A: 2-oxopropanoic acid is a strong acid than 3-oxobutanoic acid because of the electron withdrawing…

Q: 2-Methylvaleric acid, CH3(CH2)2CH(CH»)COOH, has a pKa =4.9. Draw the skeletal structure of the…

A: According to the Bronsted-Lowry acid-base theory, the dissociation of acids in water will lose a…

Q: Chloroacetic acid, HC₂H₂O₂Cl, is a stronger monoprotic acid than acetic acid. In a 0.10 M solution,…

A: We have to calculate the Ka of chloroacetic acid and aso it PKa value .

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: pH defined the acidic or basic strength of the given solution. Mathematically, it is the value of…

Q: The base protonation constant K, of trimethylamine ((CH,) N) is 6.31 × 10 3 Calculate the pH of a…

A: In this question, we want to determine the pH of the Solution in one decimal place. You can see…

Q: Acid Conjugate base Acid H2CO3 HCO3 Base Strength Strength Increases Increases H2PO4 HPO,- (1) The…

A: Ka is the tool to measure the acidic strength of a given acid

Q: If you mix equal molar quantities of NH3 (Kb = 1.8 x 10-5) and CH3CO2H (Ka= 1.8 x 10-5), the…

A: Given that the solution contains equal molar concentrations of NH3 and CH3COOH. Also given Kb of NH3…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: pKa value: pKa value negative logarithm of the acid dissociation constant (Ka). pKa = -logKa Low pKa…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

Q: Identify which of the acids below will yield the stronger conjugate base and why. a) HOCl (K a =…

Q: Please rank the following acids in order of increasing pK. O HCI, HF, CH;COOH, H,O O H2O, CH;COOH,…

A: Acidity can be best explained using pKa values which is inversely proportionate to the acidity.…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

Q: 2-Methylvaleric acid, CH»(CH2)½CH(CH))COOH, has a pka =4.9. Draw the skeletal structure of the…

A: The skeletal structure of an organic compound is the series of atom that are bonded together forms…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: Ka is the acid dissociation constant. It is basically the equilibrium constant for weak acids. This…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: ->pKa = -log Ka ->Ka tells about acid strength ->Ka proportional to acid strength ->pKa…

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

For each value of K_a, calculate the corresponding value of pK_a. Which compound is the stronger acid?

Q.) chloroacetic acid, K_a = 1.38 X 10^-3

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

Consider these acids (a) Arrange the acids in order of increasing acid strength from weakest to strongest. (b) Which acid has the smallest pKa value?
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
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?
Calculate Ka for the weak acids that have the following PKa values. (a) 3.9(b) 10.12 (c) 13.07
Which is the stronger of the following two acids? (a) acetic acid, CH3CO2H, Ka = 1.8 105 (b) chloroacetic acid, ClCH2CO2H, pKa = 2.85
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) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.
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)
Several acids and their respective equilibrium constants are: Which is the strongest acid? Which is the weakest acid? Which acid has the weakest conjugate base? Which acid has the strongest conjugate base?
Calculate the pKa value for each of the following acids. a. Phosphoric acid (H3PO4), Ka = 7.5 103 b. Hydrofluoric acid (HF), Ka = 6.8 104 c. Hydrogen phosphate ion (HPO42), Ka = 4.2 1013 d. Propanoic acid (HC3H5O2), Ka = 1.3 105
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?