What is the [OH-] in a solution that has a [H3O+] = 1.0 × 10-5 M?

Q: How would you categorize a solution that has a concentration of hydroxide ions equal to 3 x 102 M? O…

A: A solution is acidic if pH<7 Basic if pH>7 Neutral if pH=7 pH is the -log[H+] pOH = -log[OH-]…

Q: 5) Consider the reaction given below. H H #[#] H-C-N: + HH HH H-C-N-H HH In the above reaction,…

A: The objective of the question is to identify the substance acts as a Lewis acid and which acts as a…

Q: Calculate the [H+] and pH of a 1.39×10-4 M butanoic acid solution. The Ka of butanoic acid is…

A: The objective of this question is to calculate the concentration of hydrogen ions [H+] and the pH of…

Q: Is the [H+] of a pH 7.6 solution higher or lower than the [H+] of a pH 9.4 solution?

A:

Q: Find the [OH-] in an acidic solution where [H+] = (6.0x10^-5)

A: An acid is a molecules which can donates protons or they are capable of donating hydrogens. Bases…

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: What is the [OH-] in a solution that has a [H3O+] = 1.0 × 10-5 M?

A: Given information is as follows: The concentration of H3O+ = 1.0×10-5 M The concentration of OH- = ?…

Q: What is [OH-] in a solution of 1.25 M NH3 and 0.78 M NH4NO3? NH3 (aq) + H2O (l) = NH4 (aq) + OH-…

A: The question is based on the concept of the pOH of the solution.It is defined as a negative…

Q: 4) What is the [OH] for a solution with a [H,O'] of 9.97 X 104 M? Is the solution acidic, basic or…

A:

Q: A solution has a [OH−] = 3.4 × 10−5 M at 25 °C. What is the [H3O+] of the solution?

A:

Q: What is the [ H3O+] in a solution that has a [OH-] = 9.0×10−2 M?

A: Given, Concentration of OH- = 9.0 * 10-2 Concentration of H3O+ =? By using the autoionization…

Q: What is the concentration of OH- in an aqueous solution with [H3O+] = 1.0 x 10-11 M?

A: Given  :  [H3O+] = 1.0 x 10-11 M Calculate : [OH-] = ?

Q: What is the [OH-] concentration (M) for a solution, if the [H3O+]=3.2x10-5M?

A: Answer: [OH-] =3.16 × 10-10 M Given    Concentration  of  H3O+,-H3O+=3.2×10-5M    Concentration  of…

Q: What is the [OH-] in a solution that has a [H3O+] = 1.0 × 10-8 M?

A:

Q: If the hydronium ion (H3O+) concentration of a solution is 1 x 10-11 M (at 25°C), then what is the…

A:

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

A: Given, Concentration of NaOH = 0.62M

Q: A solution has [OH-] = 1×10-10. What is the concentration of H3O+ ion?

A:

Q: What are [H+] and [OH-] in a 0.00338 M solution of KOH

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: 2. What is the pOH of a solution in which the hydroxide ion concentration is 3.2x10-3M? 3. What is…

A: POH = -log[OH-] [H]+[OH-] = 10-14 M2

Q: What is the [OH-] of a 1.40 M solution of pyridine (CsHsN, Kb = 1.70 × 10-⁹)?

A:

Q: What is the OH- concentration of a solution  with a H3O+ concentration of 8.47x 10-8

A: Given concentration of H3O+ is 8.47 × 10-8  [H3O+] = 8.47 × 10-8

Q: Find the [OH-] of the solution, if the [H3O+] is: 2 ´ 10-11 M

A: Given that,  Concentration of [H3O+]   = 2×10-11 M

Q: What is the [OH-] in a solution that has a [H3O+] = 1 × 10-6 M?

A:

Q: A solution has [H+] or [H3O+] = 4.7 ×10–3 M. The [OH–] in this solution is

A: We know that [ H+ ] [ OH- ] = 10-14  As [ H+ ] = 4.7 * 10-3

Q: A solution has [OH-] = 1×10-10. What is the concentration of H3O+ ion?

A: The auto ionization constant of water is shown below: OH- H3O+ = KwOH- H3O+=1×10-14

Q: A solution has [OH-] = 1×10-10. What is the concentration of H3O+ ion?

A: The pH of solution indicates the acidity or basicity of the given solution, which is the negative…

Q: A solution has a [H 3O +] of 1.024x 10 -10 M. What is the [OH -]?

A: PH= - log [H 3O +]  POH=log [OH -]

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.7 × 10⁻⁴ M, then [OH⁻] is

A: In an aqueous solution [H₃O⁺] ×   [OH⁻]  = Kw

Q: A solution has [H+] = 3.5x10-4 M. The [OH-] in the solution is what?

A: • The values provided in the question are:-    i) Hydrogen ion concentration of a solution, [H+] =…

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: Arrange the following in order of increasing strength of the base: HAt HNO3 H2SO3 HF

A:

Q: Calculate (H,O*] for a 5.19 x 10-3 M HBr solution. [H,O*) = Calculate (H,O*] for a 1.60 x 10-2 M KOH…

A: Hydrogen bromide is a strong acid and the strong acid dissociates completely in an aqueous solution.

Q: What is the [OH- ] of 1.634x10-4 M HNO3?

A:

Q: a) NaOEt SA ETOH OEt HCI + OEt

A:

Q: What is the pOH of a .0767 M HydroIodic Acid Solution?

A: We know that, pH is the negative logarithm of hydrogen ion concentration and pOH is the negative…

Q: 15

A: Correct answer is HF. Weaker the acid , stronger the conjugate base. HF is the weakest acid. Acid…

Q: Which of the following solutions is most basic? Group of answer choices [OH-] = 1 X 10-4 [H+] = 1…

A:

Q: What is the [H3O+] of an ammonia cleaning solution with [OH-] = 4.0 x 10−4M? Is the solution…

A: The product of the concentration of the hydronium ions and hydroxyl ions is equal to ionic product…

Q: Calculate the [H3O+] of a stomach acid solution that contains [OH-] = 1.80 x 10-12 M.

A:

Q: A solution with the [OH-] = 1.00 x 10-11 has a [H+] of?

A: Given, [OH-] = 1.00 x 10-11 What is the [H+]?

Q: Calculate the [H+] and pH of a 2.35×10−4 M hydrazoic acid solution. The Ka of hydrazoic acid is…

A: We wil use concept of weak acid for H+ and pH.

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.