Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at...

Question

Question

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at...

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at 25°C. Identify the solution as acidic, basic, or neutral.

Answer choice are

a- 1.8 × 10^-10 M, acidic

b- 1.8 × 10^-10 M, basic

c- 9.2 × 10^-1 M, basic

d- 9.2 × 10^-1 M, acidic

e- 5.5 × 10^-10 M, neutral

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #2

Concepts and reason

The concepts used here are based on the water autoionization constant and pH of the solution.

Firstly, the concentration of hydronium ion is calculated. After that, the nature of the solution is identified using the pH scale.

Fundamentals

Water autoionization constant :

It is an equilibrium constant which is used to represent the relation between the concentration of hydroxide and hydrogen ions.

It is represented as follows.

…… (1)

Here, is the concentration of hydroxide ion and is the concentration of hydrogen ion.

The value of at is .

The pH tells the acidity or basicity of a solution. It is a negative logarithm of hydrogen or hydronium ion concentration of the solution.

…… (2)

The pH scale has a range from .

Substitute the value of as and as in the equation (1).

The concentration of hydronium ion is .

Substitute the value as in the equation (2).

Since, the pH is greater than , the solution is basic.

Ans:

The concentration of hydronium ion is .

Add a comment

Answer 2

Answer #1

The concentration of OH-is 5.5×10-5 M Calculate the concentration of HO+ as follows -14 H.o*1 1.0x10-* 5.5x10-5 1.82x10-0 M C pH > 7, so the solution is basic.

Add a comment

Answer 3

Similar Homework Help Questions

Calculate the concentration of OH- in a solution that contains 3.9 × 10-4 mol L-1 H3O+...

Calculate the concentration of OH- in a solution that contains 3.9 × 10-4 mol L-1 H3O+ at 25 °C. Also identify the solution as acidic, basic, or neutral. Group of answer choices 2.7 × 10-2 mol L-1, acidic 2.7 × 10-2 mol L-1, basic 2.6 × 10-11 mol L-1, basic 2.6 × 10-11 mol L-1, acidic 3.9 × 10-4 mol L-1, neutral
Can anyone solve question 32? A basic solution does not contain H30+ A neutral solution does...

Can anyone solve question 32? A basic solution does not contain H30+ A neutral solution does not contain any H3O+ or OH- A neutral solution contains [H20] - [H30-1 In a neutral solution the pH must equal 7 Question 31 1 pts ho What is the concentration of hydroxide ions in pure water at 35.0°C. if Kw at this temperature is 1.87 x 10-14? (show work on given page) Question 32 1 pts Calculate the concentration of H30" in a...
Plz answer 1. Calculate the concentration of H30" in a solution that contains 5.0 Identify the...

Plz answer 1. Calculate the concentration of H30" in a solution that contains 5.0 Identify the solution as acidic, basic, or neutral. A) 2.0x 10-5 M, basic D) 9.0x 10-1 M, acidic 10-10 M OH at 25°C B) 2.0 10-5 M, acidic E) 9.0 10-1 M. basic 2. Calculate the [H3O~] concentration in an aqueous solution with a pH of 9.85 at 25 C c)5.0x 10-10 M, neutral A) 7.1x 10-5 M B) 4.2x 10-10 M C)8.7 10-10 M E)...

A solution has [OH-] = 4.33 x 10-5 M. Calculate [H3O+] and pH of the solution....

A solution has [OH-] = 4.33 x 10-5 M. Calculate [H3O+] and pH of the solution. Then, tell whether the solution is acidic, basic, or neutral. Also, calculate pOH.
Please answer 18 and 19! and show work What are the Bronsted-Lowry acids in the following...

Please answer 18 and 19! and show work What are the Bronsted-Lowry acids in the following chemical reaction? HBr(aq) + CH_3COOH (aq) CH_3C (OH)^+_2 (aq) + Br^-(aq) a) CH_3COOH, CH_3C (OH)^+_2 b) CH_3COOH, Br^- c) HBr, CH_3COOH d) HBr, CH_3C(OH)^+_2 What is the strongest acid among the following? a) H_2SO_3 b) H_2SeO_3 c) H_2SO_4 d) H_2SeO_4 What is the K_w of pure water at 50.0 degree C, if the pH is 6.630? a) There is not enough information to calculate...
5. What is the pH of a solution with a OH concentration of 2.52 x 10'M?...

5. What is the pH of a solution with a OH concentration of 2.52 x 10'M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer 6. What is the pH of a solution with a H2O* concentration of 2.7 x 10 M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer 7. What is the pH of a solution with a OH concentration of 5.53 x 10-M? Is this solution...

Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 1.0×10−9 M . Calculate [H3O+]...

Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 1.0×10−9 M . Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 2.3×10−2 M . Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 6.1×10−12 M . Classify the solutions as acidic or basic. [OH−]=1.0×10−9 M[OH−]=1.0×10−9 M [OH−]=2.3×10−2 M[OH−]=2.3×10−2 M [OH−]=6.1×10−12 M[OH−]=6.1×10−12 M
Calculate [H3O+] given [OH−] in each aqueous solution. Part A [OH−] = 6.6×10−11 M Part B...

Calculate [H3O+] given [OH−] in each aqueous solution. Part A [OH−] = 6.6×10−11 M Part B Classify this solution as acidic or basic. Part C [OH−] = 4.5×10−9 M Part D Classify this solution as acidic or basic. Part E [OH−] = 6.6×10−4 M Part F Classify this solution as acidic or basic. Part G [OH−] = 2.5×10−2 M Part H Classify this solution as acidic or basic.
Calculate either [H3O+] or [OH−] for each of the solutions. Solution A:[OH−]=2.59×10−7 M Solution A: [H3O+]=...

Calculate either [H3O+] or [OH−] for each of the solutions. Solution A:[OH−]=2.59×10−7 M Solution A: [H3O+]= M Solution B:[H3O+]=8.91×10−9 M Solution B: [OH−]= M Solution C:[H3O+]=7.61×10−4 M Solution C: [OH−]= M Which of these solutions are basic at 25 °C? A:[OH−]=2.59×10−7 M B:[H3O+]=8.91×10−9 M

Instructions: Determine if each solution is acidic, basic, or neutral. [H3O+] = 1 x 10-10 M;...

Instructions: Determine if each solution is acidic, basic, or neutral. [H3O+] = 1 x 10-10 M; [OH-] = 1 x 10-4 M [H3O+] = 1 x 10-7 M; [OH-] = 1 x 10-7 M [H3O+] = 1 x 10-1 M; [OH-] = 1 x 10-13 M [H3O+] = 1 x 10-13 M; [OH-] = 1 x 10-1 M Instructions: Calculate [OH-] given [H3O+] in each aqueous solution and classify the solution as acidic or basic. [H3O+] = 2.6 x 10-3...

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at...

Homework Answers

Add Answer to:
Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at...

Post as a guest

Earn Coins

Calculate the concentration of OH- in a solution that contains 3.9 × 10-4 mol L-1 H3O+...

Can anyone solve question 32? A basic solution does not contain H30+ A neutral solution does...

Plz answer 1. Calculate the concentration of H30" in a solution that contains 5.0 Identify the...

A solution has [OH-] = 4.33 x 10-5 M. Calculate [H3O+] and pH of the solution....

Please answer 18 and 19! and show work What are the Bronsted-Lowry acids in the following...

5. What is the pH of a solution with a OH concentration of 2.52 x 10'M?...

Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 1.0×10−9 M . Calculate [H3O+]...

Calculate [H3O+] given [OH−] in each aqueous solution. Part A [OH−] = 6.6×10−11 M Part B...

Calculate either [H3O+] or [OH−] for each of the solutions. Solution A:[OH−]=2.59×10−7 M Solution A: [H3O+]=...

Instructions: Determine if each solution is acidic, basic, or neutral. [H3O+] = 1 x 10-10 M;...

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at...

Homework Answers

Add Answer to: Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at...

Post as a guest

Earn Coins

Add Answer to:
Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at...