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 [H3O+], [OH–], and pH. c. a solution that is 0.052 M in HBr and 0.020 M in HNO3

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.

Ch.16 - Acids and Bases

Tro - Chemistry: A Molecular Approach 4th Edition

Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook

All textbooks

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, K_w = 1.0 x 10^-14, to find [OH^-]. The relationship is given by [H₃O⁺][OH^-] = K_w. 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 K_w are valid for the given concentrations.

Verified video answer for a similar problem:

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

Video duration:

Was this helpful?

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+].

Recommended video:

Guided course

02:43

Relationship between ∆E°, ∆G°, and K

Related Practice

Textbook Question

What mass of HI must be present in 0.250 L of solution to obtain a solution with each pH value?

a. pH = 1.25 b. pH = 1.75 c. pH = 2.85

108

views

Textbook Question

Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HClO₄ c. a solution that is 0.045 M in HClO₄ and 0.048 M in HCl d. a solution that is 1.09% HCl by mass (assume a density of 1.01 g/mL for the solution)

Textbook Question

Determine the concentration of H₃O⁺ to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.52

2011

views

Textbook Question

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. d. a solution that is 0.655% HNO₃ by mass (assume a density of 1.01 g/mL for the solution)

1747

views

Textbook Question

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. b. 0.015 M HNO₃

441

views

Textbook Question

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

716

views

rank