How to Calculate [OH-] from pOH.

Q: The [H3O+] in a solution with pOH of 0.253 is ____.

A:

Q: Calculate 3OH-4 and pH for each of the following strong base solutions: (a) 0.182 M KOH

A:

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: (a) What are [H3O+], [OH-], and pOH in a solution with a pH of 4.77? (b) What are [H3O+], [OH-], and…

A: a) The [H3O+], [OH-], and pOH of the solution has to be calculated, pOH of the solution is…

Q: What is the [H3O+] for a solution with a [OH-] of 7.79 X 10-6 M? Is the solution acidic, basic or…

A: The solution which have: pH > 7 basic pH = 7 neutral pH < 7 acidic

Q: The pOH of a basic solution is 5.09. What is [H⁺]?

A: pH is equal to negative logarithmic value of hydrogen ions concentration

Q: concentration of OH

A:

Q: Calculate the [H3O+] and pH of a 0.62M NaOH solution.

A: Given, Concentration of NaOH = 0.62M

Q: gaibrocat thoug wyr 2. Calculate the value of [OH-] from the given [H3O+] in each solution and label…

A: (H3O+) (OH-) = Kw =  1×10^-14

Q: If the [OH-] of a solution is 7.7 x 10-11 M, the pOH of the solution is

A: Given data set: Concentration of OH- = 7.7*10-11 M   We need to calculate the pOH of this solution.

Q: What are the Four factors affect the acidity of HA ?

A:

Q: Calculate the concentration of H3O+ and OH- in a sample of pH 3.30 solution?

A: As we know  pH = -log [H+] and pOH = -log[OH-]  and also pH+ pOH = 14

Q: 0.52 M KOH [H+] [OH-] PH POH

A:

Q: the

A: Given data set: pH = 6.84 We need to determine the [OH-] Now, we know that: pH = -log[H+] [H+][OH-]…

Q: Calculate the [H3O+] in an HCl solution with a pH of 2.3.

A: The pH of the solution can be calculated by using the following expression:  To determine the…

Q: What is the [OH -] in a solution with a pH of 8.97?

A: Since pH = -log[H+] = 14 + log [OH -]

Q: Calculate [OH-] given pH=13.58

A: The sum of the pH and pOH is 14. here, pH and pOH are the log concentrations of the protons and…

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 3.47? (b) What are [H₃O⁺],…

A: pH is equal to the negative logarithm of hydronium while pOH is equal to the negative logarithm of…

Q: Calculate the pOH and pH of a 0.0045 M solution of NaOH.

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: If HNO3 is added to water, how does [OH-] change? How does pH change? (b) Use the pH…

A: a. HNO3 releases  H+ in the water Therefore, acidity of water increases pH of water decreases HNO3 +…

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

A: pOH of a solution = 5.63 [OH-] = ?  -----------------------------------

Q: Calculate [OH-] given pH=1.92

A: Acidity of the aqueous solution is given in the term of pH. pH is given as,…

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 8.97? (b) What are [H₃O⁺], [OH⁻],…

A: The concentration of the hydrogen ions in the solution is determined in the pH scale.…

Q: 2a) Write the hydrolysis reaction of a 0.050M solution of hydrochloric acid. Clearly identify the…

A: The objective of the question is to determine the following. Write the hydrolysis reaction. Identify…

Q: (a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 9.85? (b) What are [H₃O⁺], [OH⁻],…

A: a) pH of a solution is equal to negative logarithm of hydronium ion concentration present in it. So;…

Q: 6. A substance has a [H,O'] of 5.21 x 10³, determine [OH], pH and pOH and determine if the substance…

A: [H3O+][OH-] = 1 x 10-14 pH = -log[H3O+] pOH = -log[OH-] pH < 7 , acidic pH > 7 , basic pH = 7,…

Q: Calculate the value of [OH] from the given [H₂O*] and label the solution as acidic or basic. a. 10-¹…

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: The pOH of a basic solution is 6.07. What is [H⁺]?

A:

Q: Is NH4ClO basic, acid, or neutral?

A: When a salt of strong base and weak acid is hydrolysed it gives basic solution i e salt is basic in…

Q: 4a) Write the hydrolysis reaction of hydroiodic acid. Clearly identify the acid, base, conjugate…

A: The objective is to determine the hydrolysis reaction of hydroiodic acid.Identify acid, base,…

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.