Calculate the pH and pOH of a solution at 25°C, if [OH-] = 1.3 x 10-⁹ M. Answer to the hundredths place. pH = pOH =

Q: Identify the acid, base, conjugate acid and conjugate base in the following reactions: HF (aq) + H2O…

A: Note: As per our guidelines, we are supposed to answer only the first question (question number 1).…

Q: Ascorbic acid (H2C6H6O6; H2Asc), known as vitamin C, is a diprotic acid (Ka1 = 1.0x10-5 and Ka2 =…

A: Given: The concentration of ascorbic acid (H2Asc) is 0.050 mol/L. The dissociation constants of…

Q: In a solution, [H+] = 1.54 x 10-2 M. What is its pH and is it considered an acid or a base?

A: Given is,  [H+] = 1.54 x 10-2 M

Q: What is the pH of a solution that has [OH-] = 5.0 x 10-7 M?

A:

Q: Calculate the [OH-| and the pH of a solution with an [H*] = 2.6 x 10-1" M at 25 °C. [OH-] = pH :…

A: pH measures acidity of the solution. pH of a solution depends on the hydrogen ion concentration.

Q: Given that Kw for water is 2.4 × 10-14 at 37 °C, calculate the pH of a neutral aqueous solution at…

A: pH of solution is defined as negative logarithm of hydrogen ions present in solution.

Q: Determine the [H+], [OH-], and pOH of a solution with a pH of 3.20 at 25 °C. [H+] = [OH-] = pOH =

A: PH is commonly known as power of hydrogen lower the pH higher the acidic nature of solution .

Q: Trimethylamine,(CH3)3N , is produced when plants and animals decompose and has a very unpleasant…

A:

Q: Calculate the pH of a solution that has a concentration of OH- equal to 5.92 x 10^ (- 9) M.  (Write…

A: The objective of this question is to calculate the pH of a solution given the concentration of…

Q: 1) Write a chemical reaction to show the neutralization of hydriodic acid (HI) by sodium hydroxide…

A:

Q: Part A pH = 8.77 Express your answer using two significant figures. Enter your answers numerically…

A: Part A  pH = 8.77  pH = -log[H3O+]  Log[H3O+] = -pH  [H3O+] = antilog(-pH) = antilog(-8.77)  [H3O+]…

Q: Which of the following is a basic solution? [H3O+] = 1.23 × 10-9 pH = 7 [H3O+] = [OH-]

A: The pH of the solution helps in the determination of the acidity or basicity of the solution. It…

Q: Determine the [H*]. [OH ]. and pH of a solution with a pOH of 13.48 at 25 °C. [H*] = (OH] = %3D pH =

A: Hi, as you have posted 2 questions and have not mentioned which one you want us to solve, hence we…

Q: [OH"] [OH¯] = pH = pOH =

A:

Q: 5. Make the following conversions. Report answers to 2 decimal places.In each case, tell whether the…

A: pH = -log[H3O+]  [H3O+].[OH-] = kw  Kw at 25°C = 1.00 × 10-14

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

A:

Q: Calculate [OH-] for each solution. pOH = 13.28     pH = 1.82     pOH =

A: The question is based on the concept of hydronium ion and hydroxide Ion concentration. We have to…

Q: In a solution, [H+ ] = 3.25 x 10-10 M. What is its pH and is it considered an acid or a base?

A: A solution can be classified as acidic or basic or neutral depending on the pH value. For a solution…

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.