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

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Ch.16 - Acids and Bases

Problema 57c

Capitolo 16, Problema 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

Guida verificata passo dopo passo

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.

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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.

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Percorso guidato

01:09

Strong Acid-Strong Base Titration

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.

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02:15

pH Calculation Example

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+].

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02:43

Relationship between ∆E°, ∆G°, and K

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