A 500.0-mL buffer solution is 0.100 M in HNO 2 and 0.150 M in KNO 2 . Determine if each addition would exceed the capacity of the buffer to neutralize it. b. 350 mg KOH

Hi everyone. So I asked if the addition of 1.5 g of potassium hydroxide will exceed the capacity of the 250 millimeter buffer solution. That is 0.125 moles of hydrogen fluoride. 0.175 moles of sodium fluoride. We know that potassium hydroxide is it base I was gonna consume the acid and it will exceed it. The mall's potassium hydroxide is greater than the malls of hydrogen fluoride. So we need to first calculate the moles of E at 1.5 g of potassium hydroxide. And in one moment we have the smaller mouse. This is 39.098 g. That's 15 .999 g. That's 1.008 g. Let's give us 56 11 g. So you're going to get 0.0267 moles of potassium hydroxide. We know that the polarity equal some balls of the salute lot by leaders. And the solution we need to convert our volume into leaders. 250 male leaders. And in one leader we have 1000 ml. We're gonna get 0.25 leaders. 0.125 malls. Oh how's your floor ride in one leader? And then we have 0.25 L of solution. We're gonna get 0.03 balls of hydrogen fluoride. And this is more than a number of multiple tasks and hydroxide and now it will not exceed the capacity. Thanks for watching my video And I hope it was helpful

Ch.17 - Aqueous Ionic Equilibrium

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Tro 4th Edition

Ch.17 - Aqueous Ionic Equilibrium

Problem 59b

Chapter 17, Problem 59b

A 500.0-mL buffer solution is 0.100 M in HNO₂ and 0.150 M in KNO₂. Determine if each addition would exceed the capacity of the buffer to neutralize it. b. 350 mg KOH

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Convert the mass of KOH to moles by using its molar mass. The molar mass of KOH is approximately 56.11 g/mol.

Calculate the moles of HNO_2 in the buffer solution using its concentration and volume. Use the formula: moles = concentration (M) × volume (L).

Calculate the moles of KNO_2 in the buffer solution using its concentration and volume. Use the formula: moles = concentration (M) × volume (L).

Determine the buffer capacity by comparing the moles of KOH to the moles of HNO_2 and KNO_2. A buffer can neutralize added acid or base as long as the moles of added substance do not exceed the moles of the buffer components.

Assess if the moles of KOH exceed the buffer capacity. If the moles of KOH are less than or equal to the moles of HNO_2 and KNO_2, the buffer can neutralize the addition. Otherwise, it exceeds the buffer capacity.

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Key Concepts

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

Buffer Solutions

Buffer solutions are mixtures that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. In this case, HNO2 is the weak acid, and KNO2 provides the conjugate base, allowing the solution to maintain a stable pH despite the addition of KOH.

Buffer Capacity

Buffer capacity refers to the amount of acid or base that a buffer can neutralize before a significant change in pH occurs. It is influenced by the concentrations of the acid and base components in the buffer. The greater the concentrations, the higher the buffer capacity, meaning it can neutralize more added acid or base without exceeding its limits.

Stoichiometry of Neutralization Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions. In the context of buffer solutions, it is essential to determine how much of the buffer components will react with the added KOH. The neutralization reaction between KOH (a strong base) and HNO2 (a weak acid) will dictate whether the buffer can effectively neutralize the added base without exceeding its capacity.

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Which buffer system is the best choice to create a buffer with pH = 9.00? For the best system, calculate the ratio of the masses of the buffer components required to make the buffer. HF/KF HNO₂/KNO₂ NH₃/NH₄Cl HClO/KClO

Textbook Question

A 500.0-mL buffer solution is 0.100 M in HNO₂ and 0.150 M in KNO₂. Determine if each addition would exceed the capacity of the buffer to neutralize it. a. 250 mg NaOH

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A 500.0-mL buffer solution is 0.100 M in HNO₂ and 0.150 M in KNO₂. Determine if each addition would exceed the capacity of the buffer to neutralize it. c. 1.25 g HBr

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A 500.0-mL buffer solution is 0.100 M in HNO₂ and 0.150 M in KNO₂. Determine if each addition would exceed the capacity of the buffer to neutralize it. d. 1.35 g HI

Textbook Question

A 1.0-L buffer solution is 0.125 M in HNO₂ and 0.145 M in NaNO₂. Determine the concentrations of HNO₂ and NaNO₂ after the addition of each substance: a. 1.5 g HCl b. 1.5 g NaOH c. 1.5 g HI

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A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. b. 350 mg KOH

Verified video answer for a similar problem:

Key Concepts

Buffer Solutions

Buffer Capacity

Stoichiometry of Neutralization Reactions

A 500.0-mL buffer solution is 0.100 M in HNO₂ and 0.150 M in KNO₂. Determine if each addition would exceed the capacity of the buffer to neutralize it. b. 350 mg KOH