Answered: -7 The acid dissociation constant K of…

-7 The acid dissociation constant K of alloxanic acid (HC4H₂N₂O²) is 2.24 × 10¯7. Calculate the pH of a 3.6M solution of alloxanic acid. Round your answer to 1 decimal place.

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.45EP

See similar textbooks

Related questions

Q: Write the formula of the conjugate base of CH3CO2H

A: Conjugate base of an acid contains one less proton.

Q: The acid dissociation constant K of acetic acid (HCH3CO2) is 1.8 × 10¯5. a Calculate the pH of a…

Q: -8 The base protonation constant K, of lidocaine (CH, NONH) is 1.15 × 10 °. 14 Calculate the pH of a…

Q: The pH of a solution is 2.45. What is the molar concentration of hydronium ions in the solution?…

A: We have given that pH = 2.45 [H3O+] = ?

Q: Calculate the pH of the resulting solution if 26.0 mL of 0.260 M HCl(aq) is added to 36.0 mL of…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a solution…

Q: Determine the pH of a 0.18 M solution of pyridinium nitrate (C5H5NHNO3) at 25 ° C. [Pyridinium…

A: Given,Molarity of pyridinium nitrate (C5H5NHNO3) = 0.18 MKb = 1.7 × 10−9The value of Ka can be…

Q: ✓9 10 A chemist titrates 160.0 mL of a 0.4381 M benzoic acid (HC, H,CO₂) solution with 0.2772M NaOH…

A: “Since you have posted multiple questions, we will provide the solution only to the first question…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

Q: What is the pH and the pOH of a 0.0125 M KOH solution at 100.0 °C? The value for Kw for water is…

A: Concentration of KOH solution as 0.0125 M at 100 °C

Q: 7. Identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate…

Q: Calculate the pH of a 0.0076 M solution of acetic acid, CH3COOH. The Ka of acetiç acid = 1.8 x 10-5.…

A: Kaa of acetic acid = 1.8× 10- 5 initial concentration of acetic acid = 0.0076 M

Q: Calculate the pH and pOH of the following solutions (see Appendix 11 of your textbook for pKa…

A: "Since you have asked multiple questions and not mentioned the question number to be solved, we will…

Q: Calculate the pH of the resulting solution if 22.0 mL of 0.220 M HCl(aq) is added to 32.0 mL of…

A: Given : To calculate the pH of the resulting solutions for both problems. The titration is between…

Q: Determine the pH of a 1.2 M solution of ammonia, NH3, with K 1.8 x 105

Q: A chemist dissolves 866. mg of pure perchloric acid in enough water to make up 50. mL of solution.…

A: Given: Mass of perchloric acid (HClO4) = 866 mg =866×10-3 g Volume of the solution = 50 ml = 50×10-3…

Q: For the weak base piperidine, C5H₁0NH, K = 1.30 × 10³. What is the equilibrium concentration of all…

Q: The acid dissociation constant K, of alloxanic acid (HC H₂N₂O) is 2.24 x 10 Calculate the pH of a…

A: Ka of alloxanic acid HC4H3N2O5 = 2.23×10-7Concentration of alloxanic acid = 3.9 MpH of the solution…

Q: The base protonation constant K, of morpholine (C¸H¿ONH) is 2.14 × 10 °. 9- Calculate the pH of a…

A: Since morphine is a weak base. Hence the base dissociation reaction of morphine is C4H8ONH (aq) +…

Q: 10. 0.94 The base protonation constant K of ammonia (NH3) is 1.8 × Calculate the pH of a 0.94 M…

A: Given- Concentration of Ammonia= 0.94 M Kbof Ammonia= 1.8×10-5 pH of solution = ? To find

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 × 10'. Calculate the pH of a 2.9 M…

A: Given, Ka of carbonic acid (H2CO3) = 4.5 × 10-7 Molarity of H2CO3 solution = 2.9 M The…

Q: The base protonation constant K, of allantoin (C,H,N;03NH,) is 9.12 × 10 °. Calculate the pH of a…

A: Given:

Q: The base protonation constant K of allantoin (CH4NO3NH2) is 9.12 × 10 Calculate the pH of a 1.1 M…

Q: The acid dissociation constant K of hydrocyanic acid (HCN) is 6.2 × 10 10 a Calculate the pH of a…

Q: -6 The base protonation constant K of morpholine (C₂HONH) is 2.14 × 10 Calculate the pH of a 1.0 M…

A: Answer:Ostwald's dilution law is applicable for the weak electrolytes and as morpholine is a weak…

Q: The acid dissociation constant Kof boric acid (H₂BO3) is 5.8 × 10 Calculate the pH of a 3.8M…

A: The concentration of boric acid = 3.8 MThe dissociation constant of boric acid = pH of the solution…

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

A: The given compounds are salts of given weak acids and base. Weak base have conjugate acid salt and…

Q: The acidity of a solution is measured by its pH. If H+ represents the concentration of hydrogen ions…

A: Given that : pH of solution B = 3.4 using pH = -log[H+] [H+] = 10-pH = 10-3.4 = 3.98 × 10-4 M So,…

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

-7
The acid dissociation constant K of alloxanic acid (HC4H₂N₂O) is 2.24 × 10¯7.
Calculate the pH of a 3.6M solution of alloxanic acid. Round your answer to 1 decimal place.
78°F
pH =
0
Explanation
Check
X
Ś
O
Search

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: Given alloxanic acid

VIEW

Step 2: Working formula and pH

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

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?
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?
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
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.
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
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. HC3H3O3 b. HCN c. H2SO4 d. H2SO3
Consider the following four solutions: (1) apple juice, pH 3.8, (2) pickle juice, pH 3.5, (3) carbonated beverage, pH 3.0, and (4) drinking water, pH 7.2. a. Which solution has the highest [H3O+]? b. Which solution has the highest [OH]? c. List the solutions in order of increasing acidity. d. List the solutions in order of decreasing basicity.
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. H3PO4 b. H3PO3 c. HBr d. HC2H3O2
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+()
Indicate whether each of the following samples is acidic, basic, or neutral. a. butter, pH 6.1 b. lemon juice, pH 2.2 c. peach, pH 3.5 d. milk of magnesia, pH 10.5
Classify each of the acids in Problem 10-20 as a strong acid or a weak acid. a. H2SO4 (sulfuric acid) b. HC2H3O2 (acetic acid) c. H2C5H6O4 (glutaric acid) d. HCN (cyanic acid)