Which of the following acids will most likely be the strongest?O Acid A: Ka = 6.43 × 10-/O Acid B: Ka = 4.27 × 10-6O Acid C: Ka = 3.85 × 10-5Acid D: Ka = 2.37 x 10-4

* Ka represent dissociation constant * Greater the dissociation constant, greater is ka value…

Answered: Acid A: Ka = 6.43 x 10- Acid B: Ka = 4…

Science

Chemistry

Acid A: Ka = 6.43 x 10- Acid B: Ka = 4 27 × 10-6 Acid C. Ka = 3.85 × 10-5 Acid D: Ka = 2.37 × 10-4

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 93AP

See similar textbooks

Related questions

Q: = ACIDS AND BASES Determining the strength of acids from a sketch = H₂O 2 3 Solution 1 Solution 3…

A: Here we are provided with the molecular structure of acid dissolved in water. We need to predict the…

Q: Knowing the approximate pKavalues above will help in answering this question. A) Which form…

A: Hi, this question can be solved without using pKa values.

Q: Chemistry 204 Homework Alcohols, Phenols, Ethers . Write “most" under the compound which is most…

Q: Calculate the Kb for the weak acid of Ka = 3.1 x 10-8. Calculate Ka for the weak base of Kb = 6.5 x…

Q: RE SSURESCH Evaluate the problem. Show your complete solution and box your final answer. 1. If the…

A: Write the first reaction. 2 C2H6+7 O2→4 CO2+6 H2O ∆H=-2.650 kJ Write the second…

Q: A weak acid has a Ka = 5.78x10. What is its pK3? %3D 9.244 8.238 O 1.660 0.999

A: Given, the Ka for a weak acid = 5.78 × 10-9 We have to calculate the pKa of the acid.

Q: a solution that is 0.160 M in propanoic acid and 0.110 M in potassium propanoate (where pK, = 4.87…

A: pH of a buffer is given by the following equation. pH=pKa + log[base][acid]

Q: If [H* ] = 4.3 x 10-4 M, what is [OH]?

A: The given problem can be solved by using the formula given below as; H+ OH- = Kw= 1.0×10-14…

Q: Complete the following table. Acid Ka pKa A HNO2 4.5×10-4 B HClO 3.5×10-8 The weaker acid…

Q: Consider the following acid/base reaction. Will 1 or 2 act as the acid? Will the equilibrium favor…

A: A substance which can easily provide H+ ion will act as acid while the one which accept the H+…

Q: Which of the following acids has the weakest conjugate base? O Benzoic acid, Ka = 6.5 x 10-5 %3D O…

A: Conjugate base of any acid is formed by removing the acidic proton from the acid.

Q: The weak base pyridine has a base-ionization constant of 1.4 x 10-9. CSH5N(aq) + H20(1) = OH"(aq) +…

A: Pyridine is a weak base and dissociation slightly Given dissociation constant of base(Kb)=1.4…

Q: Calculate the [OH-] and the pH of a solution with an [H+] = 0.0056 M at 25 °C. [OH-] = pH =…

A: pH is defined as the negative logarithm (base 10) of activity of hydrogen ions.Similarly,pOH is…

Q: [H;O*] in a Sauvignon Blanc with a pH of 3.22. Find the

A: The negative logarithm to the base 10 of hydronium ion concentration, [H3O+] expressed in mol/L of a…

Q: Q1// A buffer solution prepared by adding adequate amount of Acetic acid and Sodium acetate to…

A: A buffer solution is a solution that resists a change in its pH on the addition of a small amount of…

Q: Consider citric acid shown below. How many acidic protons are in this compound? _OH HO 2 5 OH OH

A: Given is the structure of citric acid.To find the number of acidic protons present in citric acid.

Q: Which one of the following is the weakest acid? O HF (Ka = 6.8 × 10-4) HCIO (Ka = 3.0 x 10-8) O HNO2…

A: Lower the value of acid dissociation constant (Ka), lower the concentration of H+ ions. Hence, we…

Q: highlighted reactant reaction Bronsted-Lowry Bronsted-Lowry neither acid base NH3(aq) + H,O(1) - NH…

Q: True or False Potassium hydroxide will produce less OH-1 ions when dissolved in water than…

A: Strong base produces more OH-1 ions in water than weak base.

Q: What are the concentrations of H,o* and OH¯ in oranges that have a pH of 3.77? [H,O*] = 1.999 x10° M…

A: pH of a solution is given by the negative logarithm of proton.

Q: Predict the products of the following neutralization reaction: KOH (aq) + HCI (aq) → O H20 and KCI O…

A: In neutralization reaction acid and base reacts to form salt and water.

Q: 3. Rank the acidity of the following molecules. OH X NH₂ OH SH

Q: Identify the strongest acid based upon its Ka. O Acid X, Ka = 1.8 × 10-6 O Acid Y, Ka = 2.2 × 10-5 O…

A: The acid dissociation constant, Ka, is a measure of the strength of an acid in solution. It is the…

Q: What is the % ionization of a 1.72e-4 M HBrO? See reaction below HBrO + H2O ↔ BrO- + H3O+ Ka =…

A: Interpretation - To determine the % ionization of a 1.72e-4 M HBrO, For given reaction -…

Q: 2H3O2 HO2 Ka = 1.8E-4 %3D

A: acidic strength increase as the releasing power of H+ increase. HBr is more acidic because size of…

Q: Show your complete and detailed solution. Make sure to include the given and the formula. How many…

A: The molarity of the solution is defined as the no of moles of solute present per liter of the…

Q: In the following acid/base reaction, which reactant is a base? HCI + H₂O HCI H₂O H3O+ + CI

Q: Calculate the pH of a 0.429 M aqueous solution of formic acid (HCOOH, Ka = 1.8 x 10-4). pH…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: In the acid-base reaction: F-(aq) + HNO3 (aq) HF (aq) + NO3- (aq), which species is the base?

A: The correct answer is given below

Q: ng the table below, arrange the following compounds according to increasing acidity: Compound…

A: pKa value pKa is the negative base 10 logarithm of the acid dissociation constant Ka pKa = -log10Ka…

Q: Pepsi has a pH of 2.5 and black tea has a pH of 5.5. How much more acidic is Pepsi than tea.

A: pH of pepsi = 2.5 pH of tea = 5.5 How much more acidic is pepsi than black tea = ?

Q: What is N3− classified as? Group of answer choices strong acid weak acid strong base weak base salt…

A: Given, N3−

Q: which of the following would have the strongest conjugate base?

A: The equilibrium constants, Ka and Kb of weak acid and conjugate base are related through the below…

Q: Be sure to answer all parts. Hydrofluoric acid, HF, has a K₂ of 6.8 × 10-4. What are [H3O+], [F],…

A: Concentration of HF = 0.790 MKa of HF = 6.810-4Kw = 1.010-14

Q: A student makes a diagram Base to show neutralization. Acid i. Find any error(s) in his PH = 4 PH =…

A: We have given the a diagram which represents a neutralization reaction between acid and base and we…

Q: If 5 M of HN3 (a weak acid with pKa = 4.72) is added to water, then how much of this acid will…

A: To determine how much of the weak acid HN3 remains in solution at equilibrium when 5 M of HN3 is…

Q: Answer the following questions about acid-base equilibrium reactions (d)Based on the following…

A: A strong acid shows complete dissociation to respective anion and H3O+whereas a weak acid can only…

Q: 1. MeLi 2. "workup" with dilute HCI (aq)

A: Reactions are processes by which the reactant is transformed into a product. A reaction mechanism is…

Q: [H+] [OH-] pH Acid, Base, Neutral [OH] = (1 x 10 -14):1 x 10- %3D pH = (-)log(10^-5) 1 x 10-5…

A: pH < 7: acid pH = 7: neutral pH > 7: base

Q: Which of the following acids is the strongest acid? HNO2 Ka = 4.5x10-4…

A: The strongest acid can be identified as Based on Ka values which acid has more Ka value means that…

Q: Lactic acid, HC3H5O3, is found in sour milk. What is the pH of 0.30 M lactic acid? This acid is a…

A: Acid is a substance that donates a H+ion. If an acid on dissolving in water cannot dissociate…

Q: What is the [H3O+¹] of a solution with pH = 5.900 ? OA. 9.00 x 10-5 M OB. 1.26 x 10-6 M OC. 5.00 x…

Q: Calculate the pH for the following concentration: [H,0*] = 2.19 x 10-5 M A. pH=4.7 B. PH=4.9 C.…

Q: for five acids are given be = 4.6 x 10-9 a= 1.2 x 107 a = 3.42 x 10 11 Fa = 7.0 x 10 2 %3 Ka = 6.6.…

A: Acidic strength is depend on Acid dissociation constant. As higher is the Ka ,lower is Acidic…

Q: Question 5 Which one of the following statements is true? H pka - 10 O NH₂ H Question 6 NH₂ pka ~35…

A: We know K = [ product] / [reactant]

Q: Which of the following compounds is most acidic?

A: Carboxylic acids are acidic in nature and the acidity of carboxylic acid depends on the nature of…

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

100%

Which of the following acids will most likely be the strongest?
O Acid A: Ka = 6.43 × 10-/
O Acid B: Ka = 4.27 × 10-6
O Acid C: Ka = 3.85 × 10-5
Acid D: Ka = 2.37 x 10-4

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

8-17 For each of the following, tell whether the base is strong or weak. (a) NaOH (b) Sodium acetate (c) KOH (d) Ammonia (e) Water
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)
8-21 Write the formula for the conjugate base of each acid. (a) H2PO4- (b) H2S (c) HCO3- (d) CH3CH2OH (e) H2O
Gastric juice, the digestive ?uid produced in the stomach, contains hydrochloric acid, HCl, Milk of Magnesia, a suspension of solid Mg(OH)2 in an aqueous medium, is sometimes used to neutralize-excess stomach acid. Write a complete balanced equation for the neutralization reaction, and identify the conjugate acid—base pairs.
Calculate the ionization constant for each of the following acids or bases form the ionization constant of its conjugate base or conjugate acid: (a) F- (b) NH4+ (c) AsO43- (d) (CH3)2 NH2+ (e) NO2- (f) HC2O4- (as a base)
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.
What is the conjugate acid of each of the following? What is the conjugate base of each?. (a) OH-. (b) H2O. (c) HCO3-. (d) NH3. (e) HSO4-. (f) H2O2. (g) HS-. (h) H5N2+
Use Table 13-3 to help answer the following questions. a. Which is the stronger base, ClO4 or C6H5NH2? b. Which is the stronger base, H2O or C6H5NH2? c. Which is the stronger base, OH or C6H5NH2? d. Which is the stronger base, C6H5NH2 or CH3NH2?
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 ionization constant for each of the following acids or bases from the ionization constant of its conjugate base or conjugate acid: (a) HTe- (as a base]. (b) (CH3)3 NH+. (c) HAsO43- (as a base). (d) H02 _ (as a base). (e) C6H5NH3+. (f) HSO3- (as a base)
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+
Each box represents an acid solution at equilibrium. Squares represent H+ ions, and circles represent the anion. Water molecules are not shown. Which figure represents a strong acid? Which figure is a weak acid?