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.17 - Acids and Bases

Tro - Chemistry: A Molecular Approach 6th Edition

Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217당신이 사용하는 게 아니라요?교과서 변경

모든 교과서

Tro 6th Edition

Ch.17 - Acids and Bases

문제 61c

17장, 문제 61c

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

검증된 단계별 안내

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.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

도움이 되었나요?

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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+].