For each strong acid solution, determine [H 3 O + ], [OH – ], and pH. c. a solution that is 0.052 M in HBr and 0.020 M in HNO 3

Step 1: Recognize that both HBr and HNO 3 are strong acids, which means they completely dissociate in water. Therefore, the concentration of H 3 O + ions from each acid is equal to the initial concentration of the acid itself.. Step 2: Calculate the total [H 3 O + ] by adding the contributions from both acids: [H 3 O + ] = [HBr] + [HNO 3 ].. Step 3: Use the ion product of water, K w = 1.0 x 10 -14 , to find [OH - ]. The relationship is given by [H 3 O + ][OH - ] = K w . Solve for [OH - ].. Step 4: Calculate the pH of the solution using the formula pH = -log[H 3 O + ].. Step 5: Review your calculations to ensure that the assumptions of complete dissociation and the use of K w are valid for the given concentrations.

For each strong acid solution, determine [H 3 O + ], [OH – ], and pH. c. a solution that is 0.052 M in HBr and 0.020 M in HNO 3

Hey everyone, we're asked to calculate the ph the concentration of our hydro knee um ion and the concentration of our hydroxide ion for a solution that is 0.26 molar hydrochloric acid and 0.18 molar hydrochloric acid. Now, when we look at these two acids we can see that these are both strong acids and we know that strong acids disassociate completely. And because they dissociate completely, we can easily find the concentration of our hydro ni um ion which is going to be the concentration of our hydrochloric acid initially plus the concentration of a hydrochloric acid initially. So plugging in these values, we have 0.26 Mohler plus 0.18 moller. And this will get us to a total of 0.44 moller. And this will be the concentration of our hydro ni um ion. Now let's go ahead and calculate the concentration of our hydroxide ion to do so we can take our K. W. Which is one point oh times 10 to the negative 14 and divided by the concentration of our hydro ni um ion. So plugging in these values, we get one point oh times 10 to the negative 14, divided by 0.44 moller. And this gets us to a concentration of 2.27 times 10 to the negative 13 moller. Which is going to be our final answer. And finally they want us to calculate the P. H. To calculate the ph we're going to take the negative log of the concentration of our hydro ni um ion. So, plugging in that value, we get the negative log of 0.044, Which gets us to a p. h. 1.36. And this is going to be our final answer as well. 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 57c

Chapter 16, Problem 57c

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. c. a solution that is 0.052 M in HBr and 0.020 M in HNO₃

Verified step by step guidance

Step 1: Recognize that both HBr and HNO3 are strong acids, which means they completely dissociate in water. Therefore, the concentration of H3O+ ions from each acid is equal to the initial concentration of the acid itself.

Step 2: Calculate the total [H3O+] by adding the contributions from both acids: [H3O+] = [HBr] + [HNO3].

Step 3: Use the ion product of water, Kw = 1.0 x 10-14, to find [OH-]. The relationship is given by [H3O+][OH-] = Kw. Solve for [OH-].

Step 4: Calculate the pH of the solution using the formula pH = -log[H3O+].

Step 5: Review your calculations to ensure that the assumptions of complete dissociation and the use of Kw are valid for the given concentrations.

Verified Solution

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Key Concepts

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

Strong Acids and Ionization

Strong acids, such as HBr and HNO3, completely dissociate in water, meaning that they release all of their hydrogen ions (H+) into the solution. This complete ionization leads to a direct relationship between the concentration of the acid and the concentration of hydronium ions ([H3O+]), which can be calculated from the molarity of the acid.

pH Calculation

The pH of a solution is a measure of its acidity, defined as the negative logarithm of the hydronium ion concentration: pH = -log[H3O+]. For strong acids, the pH can be easily calculated using the concentration of the acid, as it directly corresponds to the concentration of H3O+ in the solution.

Relationship Between [H3O+] and [OH-]

In aqueous solutions, the product of the concentrations of hydronium ions and hydroxide ions ([H3O+][OH-]) is constant at 25°C, known as the ion product of water (Kw = 1.0 x 10^-14). Therefore, once [H3O+] is determined from the strong acid concentration, [OH-] can be calculated using the equation [OH-] = Kw / [H3O+].