Answered: Calculate [OH−] for the following solution; [H3O+] = 8.87×10−9 M Is the solution basic at 25°C?

Chemistry

10th Edition

ISBN: 9781305957404

Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher: Cengage Learning

See similar textbooks

Related questions

Q: Calculate [OH-] when given the [H3O+] in each of the following aqueous solutions and classify the…

A: The OH- has to be calculated for the given aqueous solutions and whether they were acidic, basic or…

Q: Determine [H3O+] in a solution where [NaOH] = 0.0118 M.

Q: determine the [H+], [OH-], and pH of a solution with a pOH of 3.49 at 25 degrees Celsius.

Q: Calculate either [H,O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 1.15 x 10-7…

Q: A solution has a [H3O+] of 0.0015 M. Calculate the [OH-], the pH, and the pOH of the solution. Is…

A: In the question is given that concentration of [H3O]+ is 0.0015. i.e. [H]+ = 0.0015 [OH]- = ? pH =…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.4 × 10⁻⁴ M, then [OH⁻] is:

A: The concentration of OH- can be calculated as:

Q: Calculate either [H3O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.79 x 10-7…

A: The hydronium ion and hydroxide ion concentration are related to ionic product of water since they…

Q: [OH-] = 5.0 × 10–2 Express the concentration to two significant figures and include the appropriate…

A: Consider the given information is as follows; OH-=5.0×10-2H3O+ = ?Acidic, basic or neutral = ?…

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: Determine [H30*] in a solution where [OH"]= 9.72 × 109 M. Identify the solution as acidic, basic, or…

A: At 25ºC, the ionic product of water, Kw is given by: Kw = 10-14 = [H3O+][OH-] The pH of the solution…

Q: What is the pH of an aqueous solution if the [H+] = 0.1M?

A: Given Data : [H+] = 0.1M To calculate : pH. Formula : - log [H+]

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…

Q: Determine the [H+], pH, and pOH of a solution with an [OH−] of 0.086 M at 25 °C.

Q: What is the pH of an aqueous solution in which [H+] is 0.0025 M?

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.2 × 10⁻⁴ M, then [OH⁻] is:

Q: Calculate the concentration of H3 O + in a solution that contains 5.5×10-5 M OH– at 25°C. Identify…

Q: Calculate the [ H3O+ ] of an aqueous solution that is 3.0 × 10−9 M in OH−.

Q: An aqueous solution at 25°C has a hydroxide ion concentration of 7.0×10-8 M. Calculate [H3O+] for…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.3 × 10⁻⁴ M, then [OH⁻] is:

A: Using ionic product of water, concentration of hydroxyl ion can be determined from the hydronium ion…

Q: calculate ph of 7*10^-3 M aqueous solution of Ca(OH)2 at 25 degrees

Q: Determine the [OH]- concentration of a solution that has a pH = 4.33 at 25°C?

Q: Determine [OH-] in a solution where [Ba(OH)2] = 0.0249 M.

A: Strong Base - A base which completely dissociates into it's ions in aqueous solution called strong…

Q: Ammonia solutions are used for household cleaning and typically have a hydroxide ion concentration,…

Q: Determine the [OH¯], pH, and pOH of a solution with a [H*] of 2.1 × 10-¹² M at 25 °C. [OH-] = pH =…

A: given H+ = 2.1 x 10-12

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]= 7.1 * 10^-9 M

A: Given information: Concentration of H3O+ = 7.1×10-9 M

Q: Betermine the [HT] = [OH-] = pH = 2 and pH of a solution with a pOH of 4.98 at 25

A: We can determine the [H+] , [OH-] and pH from pOH using the following formulas : pH +pOH = 14 pH =…

Q: An aqueous solution of a strong base has pOH 1.76 at 25°C. Calculate the concentration of base in…

Q: 54 For each of the following solutions, calculate [OH ] from [H;O*], or [H30*] from [OH]. Classify…

A: Since, you have given multiple subparts, we will solve the first 3 subparts for you. For other parts…

Q: Calculate the [OH-] of [H+] = 5.4 x 10^-5 M at 25 degrees Celsius. Identify the solution as neutral,…

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]= 8.2 * 10^-4 M

A: pH of the solution is given by, By using given concentration to get the pH of…

Q: Calculate either [H,O*] or [OH-] for each of the solutions at 25 °C. Solution A: [OH) = 2.97 x 107…

A: Autoionization of water takes place as follows:In pure water, the concentration of hydronium ion and…

Q: Determine [H3O+] in a solution where [NaOH] = 0.0298 M.

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: [OH-] = 1.0 x 10-7 Express the concentration to two significant figures and include the appropriate…

A: Given-> [OH^-] = 1.0 × 10^-7 M If [H3O^+] is 1.0 × 10^-7 M => then it is neutral .

Q: Part A Calculate (OH] in the following aqueous solution at 25 °C: [H3O*] = 1.6x10-8 mol - L Express…

A: Answer :- A) [OH-] = 6.7 × 10-7 (mol.L-1) B) The solution is Basic…

Q: Determine [OH-] in a solution where [HNO3] = 0.472 M.

A: Given: [HNO3] = 0.472 M We have to determine the [OH-] in the solution.

Q: Indicate, by letter, the strongest acid and the weakest acid of those below. COOH The strongest acid…

A: The acidity of an acid is determined by its ability to donate a proton (H+) in a chemical…

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: Calculate [OH-] for a 1.00E-1 M HClO4 solution. Do not enter units as part of your answer.

A: [HClO4] = 1.00E-1 M then, at 25 °C, [OH-] =?

Q: Calculate [H], [CIO], and [OH-] in an aqueous solution that is 0.110 M in HC1O4 (aq) at 25 °C. [H+]…

A: PH of the solution decides the solution is either basic or acidic ,if pH is less than 7 then…

Q: the pH of a solution with [H3O+] = 2.0×10^-4 M is

A: The pH of a solution is a measure of its acidity or alkalinity. It is defined as the negative…

Q: Determine [H30*] in a solution where [OH] = 4.97 x 10-4 M. Identify the solution as acidic, basic,…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.2 × 10⁻⁴ M, then [OH⁻] is:

A: pH +pOH = 14

Q: Determine [OH-] in a solution where [Ba(OH)2] = 0.0359 M.

A: Strong electrolytes are the electrolyte which completely dissociates into ions.

Concept explainers

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 equilibri…

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.

Question

Calculate [OH⁻] for the following solution;

[H₃O⁺] = 8.87×10⁻⁹ M

Is the solution basic at 25°C?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution

See solution Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW