For each strong base solution, determine [OH – ], [H 3 O + ], pH, and pOH. a. 0.15 M NaOH b. 1.5×10 –3 M Ca(OH) 2 c. 4.8×10 –4 M Sr(OH) 2 d. 8.7×10 –5 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.16 - Acids and Bases

Tro - Chemistry: A Molecular Approach 4th Edition

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Tro 4th Edition

Ch.16 - Acids and Bases

Problem 81

Chapter 16, Problem 81

For each strong base solution, determine [OH^–], [H₃O⁺], pH, and pOH. a. 0.15 M NaOH b. 1.5×10^–3 M Ca(OH)₂ c. 4.8×10^–4 M Sr(OH)₂ d. 8.7×10^–5 M KOH

Verified step by step guidance

Identify the strong base: Calcium hydroxide, Ca(OH)_2, is a strong base that dissociates completely in water.

Write the dissociation equation: Ca(OH)_2 \rightarrow Ca^{2+} + 2OH^{-}.

Calculate [OH^-]: Since each formula unit of Ca(OH)_2 produces two OH^- ions, multiply the concentration of Ca(OH)_2 by 2 to find [OH^-].

Calculate [H_3O^+]: Use the water dissociation constant, K_w = 1.0 \times 10^{-14}, and the relationship [H_3O^+][OH^-] = K_w to find [H_3O^+].

Determine pH and pOH: Use the formulas pOH = -\log[OH^-] and pH = 14 - pOH to find the pH and pOH of the solution.

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Key Concepts

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

Strong Bases

Strong bases are substances that completely dissociate in water to produce hydroxide ions (OH-). Common examples include alkali metal hydroxides and alkaline earth metal hydroxides, such as calcium hydroxide (Ca(OH)2). The concentration of the base directly influences the concentration of OH- ions in solution.

pH and pOH Calculations

pH and pOH are measures of the acidity and basicity of a solution, respectively. pH is calculated as the negative logarithm of the hydronium ion concentration ([H3O+]), while pOH is the negative logarithm of the hydroxide ion concentration ([OH-]). The relationship between pH and pOH is given by the equation pH + pOH = 14 at 25°C.

Ion Product of Water

The ion product of water (Kw) is the equilibrium constant for the self-ionization of water, defined as Kw = [H3O+][OH-] = 1.0 x 10^-14 at 25°C. This relationship allows for the calculation of [H3O+] from [OH-] and vice versa, which is essential for determining the pH and pOH of a solution when the concentration of a strong base is known.