The pOH of an acidic solution is 11.37. What is [OH¯]?

Q: is the pH of a solution with a pOH of 1.36? s the pOH of a solution with a [OH-] of 2.97 X

A: pH +pOH= 14 pOH = -log[OH-]

Q: A solution has a pOH of 5. Which of the following is also true?

A: Solution of 1  Given pOH = 5 Therefore pH = 9 Hence    [H3O+] = 10^-9 Answer = option (b)

Q: Calculate the pH of a 0.165 M  solution of KOH.   Calculate the pOH of a 0.165 M  solution of KOH.

A: Concentration of solution of KOH = 0.165 M

Q: What is the pOH of an aqueous solution of 0.315 M perchloric acid? pOH =

A:

Q: The pOH of a 0.0140 M solution of HCl is

A: Given that the concentration of HCl solution = c =0.0140 M So, pH of the solution = -log c = -log…

Q: Determine the pOH of a 0.0036 M HNO3 solution. HNO3 is an acid

A: 0.0036 M HNO3 SOLUTION PH= ?

Q: The pOH of an acidic solution is 8.87. What is [H*]?

A: We know that, the sum of pH and pOH is equal to 14.i.e.                            pH + pOH = 14…

Q: Calculate the H3O+ concentration for a solution with a pOH of 5.68

A: We have pOH as 5.68, we have to calculate the hydrogen ion concentration.

Q: What is the concentration of a hydrochloric acid solution with a pOH of 11.759?

A:

Q: The pOH of a 0.270 M solution of NaOH is

A: The pOH of the solution is calculated using the following equation: pOH=-logOH-······(1) Here, OH-…

Q: The pOH of an acidic solution is 12.87. What is [H⁺]?

A: We have to calculate the concentration of hydrogen ion.

Q: Calculate [OH-] for a solution with a pOH of 8.03. What is the[H3O+] of this solution? What is the…

A:

Q: Calculate the pOH for the solution with a concentration of [H+] = 2.4x10

A:

Q: The pOH of a solution is 9.10. What is the Ht concentration in the solution?

A: pH and pOH Solutions that have more value of pH in the solution, are basic solutions and solutions…

Q: A solution with a pOH of 5.55 has an [OH–] of __________

A: We know,                            pOH = - log[OH-]                    Or, log[OH-] = - pOH…

Q: The pOH of a solution is 3.43. What is the OH" concentration in the solution?

A:

Q: 2) What is the pOH of a 0.0235 M HCI solution? 21 Wh at ie

A: We know that  pH + pOH = 14 So,  pOH = 14-pH

Q: The pOH of a 0.0390 M solution of HCl is

A:

Q: The pOH of a 0.0120 M solution of HCl is

A:

Q: The pOH of a basic solution is 3.91. What is [OH⁻]?

A:

Q: The pOH of an acidic solution is 11.37. What is [OH 1?

A: In this question, we have to find out the correct answer of given problem by the help of the pOH…

Q: The pOH of an acidic solution is 10.01. What is [H*]?

A: Find the solution below

Q: The pOH of a basic solution is 3.83. What is [OH]?

A: For basic solutions calculation of POH formula  POH= - log[ -OH]  Calculation of [ -OH]  formula  […

Q: The pOH of an acidic solution is 10.79. What is [OH]?

A: pOH = 10.79  pOH = - log [OH-]  10.79 = - log [OH-]  [OH-] = 10-10.79 [OH-] = 1.6218 × 10-11 M…

Q: The pOH of a solution is 3.21. What is the OH⁻ concentration in the solution?

A:

Q: The pOH of an acidic solution is 11.55. What is [OH 1?

A: The pOH of the solution is = 11.55 The hydroxide ion concentration of the solution is =?

Q: The pOH of an aqueous solution of 0.453 M acetic acid is

A: Dissociation of weak polyprotic acid and pH  calculation:

Q: The pOH of a basic solution is 3.47. What is [H*]?

A: Given data, pOH = 3.47 To calculate the [H+].

Q: The pOH of a solution is 3.21. What is the OH concentration in the solution?

A:

Q: The pOH of a basic solution is 5.85. What is [OH⁻]?

A:

Q: The pOH of a 0.200 M solution of NaOH is

A: The pOH of a 0.200 M Solution can be calculated as -

Q: What is the pOH of of a solution with a OH concentration of 0.00000000001

A:

Q: The pOH of an acidic solution is 12.53. What is [H⁺]?

A:

Q: If the pOH for a solution is 3.00, what is the pH

A: POH = 3.00 PH = ?

Q: The pH of an acidic solution is 4.17. What is pOH?

A: pH and POH is defined for acid and base. We have relation between them so we will use the same

Q: oh−

A:

Q: The pOH of a solution is 5.23. What is the PH of the solution?

A: When the pH of the solution is high than the solution is considered as basic solution and when the…

Q: The pOH of a basic solution is 5.63. What is [OH⁻]?

A: POH is defined as, POH = – log [OH–]

Q: The pOH of a basic solution is 2.35. What is pH?

A: Given, the pOH of a basic solution is 2.35we are asked to calculate the pH of the solution.

Q: A solution formed by dissolving an antacid tablet has a pOH of 4.82. Calculate 3H+4.

A: We know that pH + pOH = 14 Given: pOH = 4.82 So, pH = 14 - 4.82 = 9.18

Q: The pOH of an aqueous solution of 0.528 M acetic acid is

A: The solution is as follows:

Q: The pOH of a 0.180 M solution of NaOH is

A:

Q: The pOH of an acidic solution is 10.37. What is [H⁺]?

A: The pOH of the solution is = 10.37 The [H⁺] (hydrogen ion concentration) of the given solution is =?

Q: The pOH of a 0.170 M solution of NaOH is

A:

Q: The pOH of an acidic solution is 8.53. What is [H⁺]?

A: Answer: [H+] = 3.4 ×10-6 M

Q: The pOH of an acidic solution is 11.13. What is pH? The pH of a 0.0077 M solution of Ca(OH)₂ is?

A: PH is defined as negative logarithm of concentration [H+] ion.  PH + POH = 14

Q: Calculate the [H*] when the pOH of the solution is equal to 1.24.

A: Given :- pOH of solution = 1.24  To calculate :- hydrogen ion concentration i.e. [H+]

Q: A solution has a pOH of 2.00. What is the [H+] and [OH-]?

A:

Q: The pOH of an aqueous solution of 0.377 M acetic acid is

A:

Q: The pOH of a solution is 9.05. What is the H* concentration in the solution?

A: [OH-] = 10-pOH  [H+].[OH-] = 10-14  [H+] = 10-14/ [OH-]

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.