For each strong base solution, determine [OH – ], [H 3 O + ], pH, and pOH. c. 1.9×10 –4 M KOH

hey everyone we're asked to solve for our P. O. H. Ph concentration of hydro ni um ions and concentration of hydroxide ions In a 1.2 times 10 to the negative 3rd moller strontium hydroxide strong based solution First. We can go ahead and solve our concentration of hydroxide ions by taking our 1.2 Times 10 to the negative 3rd molar of strontium hydroxide. And we can see through our multiple ratios that one mole of strontium hydroxide contains two mole of hydroxide ions, solving for our hydroxide ion concentration. We end up with a value of 2.4 times 10 to the negative third molar of hydroxide ions, solving for our P. O. H. We can then go ahead And take the negative log of 2. Times 10 to the -3 Molar. This will get us to a p. h. of 2.62, Solving for our ph we can then take 14 and subtract 2.62 which is our P. O. H. This will get us to a ph of 11.38. Now, lastly to solve for our concentration of hydro ni um ions We can take 10 to the negative 11. And this will get us to a concentration of 4.2 Times 10 to the -12 Molar and this is going to be our final answers for this question. So I hope this made sense. And let us know if you have any questions

Ch.17 - Acids and Bases

All textbooks

Tro 5th Edition

Ch.17 - Acids and Bases

Problem 82c

Previous problem

Next problem

Chapter 17, Problem 82c

For each strong base solution, determine [OH^–], [H₃O⁺], pH, and pOH. c. 1.9×10^–4 M KOH

Verified step by step guidance

Step 1: Identify the strong base. Potassium hydroxide (KOH) is a strong base, which means it dissociates completely in water. Therefore, the concentration of OH⁻ ions is equal to the concentration of the KOH solution, which is 1.9 \times 10^{-4} \text{ M}.

Step 2: Calculate the concentration of H₃O⁺ ions. Use the water dissociation constant (K_w = 1.0 \times 10^{-14} \text{ at 25°C}) to find [H₃O⁺]. The relationship is given by: [H₃O⁺] = \frac{K_w}{[OH⁻]}.

Step 3: Calculate the pOH of the solution. The pOH is calculated using the formula: \text{pOH} = -\log[OH⁻].

Step 4: Calculate the pH of the solution. Use the relationship between pH and pOH: \text{pH} + \text{pOH} = 14. Therefore, \text{pH} = 14 - \text{pOH}.

Step 5: Summarize the results. You now have the values for [OH⁻], [H₃O⁺], pH, and pOH for the given KOH solution.

Verified Solution

Video duration:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

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

Strong Bases

Strong bases, such as potassium hydroxide (KOH), completely dissociate in water to produce hydroxide ions (OH-). This means that the concentration of the base in solution is equal to the concentration of OH- ions produced. Understanding this dissociation is crucial for calculating the concentrations of hydroxide and hydronium ions in the solution.

pH and pOH Calculations

pH and pOH are logarithmic scales used to measure the acidity and basicity of a solution, respectively. The pH is calculated using the formula pH = -log[H3O+], while pOH is calculated as pOH = -log[OH-]. The relationship between pH and pOH is given by the equation pH + pOH = 14 at 25°C, which is essential for converting between these two measures.

Ion Product of Water

The ion product of water (Kw) is a fundamental concept in acid-base chemistry, defined as Kw = [H3O+][OH-] = 1.0 x 10^-14 at 25°C. This relationship allows us to find the concentration of hydronium ions when the concentration of hydroxide ions is known, and vice versa. It is critical for determining the pH and pOH of a solution when dealing with strong bases.