Calculate [H 3 O + ] and [OH – ] for each solution at 25 °C. a. pH = 8.55

Hello. In this problem at 25 degrees Celsius, we are asked, what are the values of the hydro ni um and hydroxide ion concentration for a solution with a Ph of 3.55 col at 25 degrees Celsius. The Ph plus the P O H is equal to 14. And so our P O H then will be equal to 14 minus the ph This be 14 -3.55. So our POH works out to 10.45. You can find the hydrogen ion concentration by taking 10 to the negative Ph that's 10 to the negative 3.55. So our high joining my concentration works out to 2.8 times 10 - Mueller. And we can find our hydroxide ion concentration. It's equal to 10 to the minus P O H. So that's equal to 10 to the -10.45. And so our hydroxide ion concentration works out to 3.5 Times 10 to the -11 Moller. So we could do a check on our work. The iron product constant water at 25 degrees Celsius tells us that the hydrogen ion concentration type. The hydroxide iron concentration is equal to one times 10 to minus 14. So we can plug in the values that we found for our hydro mind concentration and our hydroxide in concentration to verify that we got the correct concentrations. Thanks for watching. Hope this out.

Ch.17 - Acids and Bases

Tro - Chemistry: A Molecular Approach 6th Edition

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Tro 6th Edition

Ch.17 - Acids and Bases

Problem 53a

Chapter 17, Problem 53a

Calculate [H₃O⁺] and [OH^–] for each solution at 25 °C. a. pH = 8.55

Verified step by step guidance

Identify the relationship between pH and [H3O+]. Use the formula: \([H_3O^+] = 10^{-pH}\).

Substitute the given pH value into the formula to find \([H_3O^+]\).

Use the relationship between [H3O+] and [OH-] at 25 °C, which is given by the ion product of water: \(K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14}\).

Rearrange the equation to solve for \([OH^-]\): \([OH^-] = \frac{K_w}{[H_3O^+]}\).

Substitute the calculated \([H_3O^+]\) into the equation to find \([OH^-]\).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is considered neutral, while values below 7 indicate acidity and values above 7 indicate basicity. The pH is logarithmically related to the concentration of hydrogen ions, [H+], in the solution, where lower pH values correspond to higher [H+] concentrations.

Hydronium Ion Concentration

The concentration of hydronium ions, [H3O+], in a solution can be calculated from the pH using the formula [H3O+] = 10^(-pH). This relationship shows that as pH increases, the concentration of hydronium ions decreases, indicating a more basic solution. For a pH of 8.55, this calculation is essential to determine the exact concentration of hydronium ions present.

Water Ion Product

At 25 °C, the product of the concentrations of hydronium ions and hydroxide ions, [H3O+][OH-], is constant and equal to 1.0 x 10^-14, known as the water ion product (Kw). This relationship allows for the calculation of hydroxide ion concentration, [OH-], using the formula [OH-] = Kw / [H3O+]. Understanding this concept is crucial for determining the balance between hydronium and hydroxide ions in a solution.