For each strong acid solution, determine [H 3 O + ], [OH – ], and pH. a. 0.25 M HCl

Step 1: Recognize that HCl is a strong acid, which means it completely dissociates in water. Therefore, the concentration of hydronium ions, [H 3 O + ], is equal to the initial concentration of HCl, which is 0.25 M.. Step 2: Use the relationship between [H 3 O + ] and [OH - ] given by the water dissociation constant, K w = 1.0 x 10 -14 at 25°C. The formula is [H 3 O + ] x [OH - ] = K w . Substitute [H 3 O + ] = 0.25 M into the equation to solve for [OH - ].. Step 3: Calculate the pH of the solution using the formula pH = -log[H 3 O + ]. Substitute [H 3 O + ] = 0.25 M into the equation to find the pH.. Step 4: Verify your calculations by checking that the product of [H 3 O + ] and [OH - ] equals 1.0 x 10 -14 , ensuring that the calculations are consistent with the properties of water at 25°C.. Step 5: Summarize the results: [H 3 O + ] = 0.25 M, [OH - ] calculated from K w , and pH calculated from the pH formula.

For each strong acid solution, determine [H 3 O + ], [OH – ], and pH. a. 0.25 M HCl

Hey everyone we're asked for a 0.36 molar hydrochloric solution, calculate our PHP. O. H. And the concentration of our hydro knee um ion and the concentration of our hydroxide ion. So looking at this acid, we can see that we have a strong acid. And as we've learned we know that strong acids disassociate completely. And because they dissociate completely, we can easily determine the concentration of our hydro knee um ion, which essentially is the same as the concentration of our hydro biotic acid initially. So this is going to be equal to 0.36 molar. Now to calculate our ph we can take the negative log of the concentration of our hydro ni um ion. So plugging in that value we get the negative log of 0. which gets us to a ph of 0.44. Now let's go ahead and calculate for our P. O. H. To calculate for our P. O. H, we can take 14 and subtract our ph which is 0.44. Now, when we calculate this out, we end up with a p. h. of 13.56. Lastly we can go ahead and calculate the concentration of our hydroxide ion by taking 10 to the negative P. O. H. So plugging in that value we get 10 to the negative 13.56. So this gets us to a concentration of 2.75 times 10 to the -14 moller which is going to be our final answer. Now I hope this made sense. And let us know if you have any questions.

Ch.16 - Acids and Bases

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Tro 4th Edition

Ch.16 - Acids and Bases

Problem 57a

Chapter 16, Problem 57a

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. a. 0.25 M HCl

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Step 1: Recognize that HCl is a strong acid, which means it completely dissociates in water. Therefore, the concentration of hydronium ions, [H3O+], is equal to the initial concentration of HCl, which is 0.25 M.

Step 2: Use the relationship between [H3O+] and [OH-] given by the water dissociation constant, Kw = 1.0 x 10-14 at 25°C. The formula is [H3O+] x [OH-] = Kw. Substitute [H3O+] = 0.25 M into the equation to solve for [OH-].

Step 3: Calculate the pH of the solution using the formula pH = -log[H3O+]. Substitute [H3O+] = 0.25 M into the equation to find the pH.

Step 4: Verify your calculations by checking that the product of [H3O+] and [OH-] equals 1.0 x 10-14, ensuring that the calculations are consistent with the properties of water at 25°C.

Step 5: Summarize the results: [H3O+] = 0.25 M, [OH-] calculated from Kw, and pH calculated from the pH formula.

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Key Concepts

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

Strong Acids

Strong acids, such as hydrochloric acid (HCl), completely dissociate in water, meaning that all the acid molecules break apart into their constituent ions. For a 0.25 M HCl solution, this results in a hydronium ion concentration, [H3O+], of 0.25 M, as each HCl molecule produces one H3O+ ion.

pH Calculation

The pH of a solution is a measure of its acidity, calculated using the formula pH = -log[H3O+]. For the 0.25 M HCl solution, the pH can be determined by substituting the [H3O+] value into the formula, yielding a pH of approximately 0.60, indicating a highly acidic solution.

Water Ion Product

In pure water at 25°C, the product of the concentrations of hydronium ions and hydroxide ions is constant, known as the water ion product (Kw = [H3O+][OH-] = 1.0 x 10^-14). To find the hydroxide ion concentration, [OH-], in a strong acid solution, use the relationship [OH-] = Kw / [H3O+]. For the 0.25 M HCl solution, this results in [OH-] being approximately 4.0 x 10^-14 M.

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For each strong acid solution, determine [H3O+], [OH–], and pH. a. 0.25 M HCl

Verified Solution

Key Concepts

Strong Acids

pH Calculation

Water Ion Product

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. a. 0.25 M HCl