-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.

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…

A:

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

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

A:

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…

A:

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 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

A:

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…

A:

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: 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…

A:

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

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,…

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.