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. c. 1.25 g HBr

five or interact with the addition of 2.56 g of Hydrofluoric acid exceeds the capacity. The 250 million births solution That is 0.125 moller of hydrogen fluoride, 0.175 moller studying fluoride. You know that Hydrofluoric acid is an acid. It's gonna consume the conjugate base and it will exceed hit. The malls of hydrochloric acid is greater than the malls of sodium fluoride. We need to calculate the malls of each Have 2. grams clark acid. And in one bowl have the molar mass. This is 1.008g. R 35 .453g. We're gonna get 36.46 g. We get 0.0702 walls of hydrochloric acid. And we know that polarity was more than that wanted by leaders of the solution. I need to convert our volume into leaders 250 million years And in one liter of 1000 ml You get 0.25 leaders Number was 0.175 miles studying fluoride and one leader We have 0.25 leaders. Just give us 0.04 37 5 malls. So this number is less than the moles of hydrochloric acid. Yes, it will exceed the buffer capacity. Thanks for watching my video and I hope it was helpful

Ch.18 - Aqueous Ionic Equilibrium

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Tro 5th Edition

Ch.18 - Aqueous Ionic Equilibrium

Problem 59c

Chapter 18, Problem 59c

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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Step 1: Identify the acid and base in the buffer solution. In this case, HNO2 is the weak acid and KNO2 (which dissociates to give NO2-) is the weak base.

Step 2: Calculate the moles of HNO2 and NO2- in the buffer solution. This can be done by multiplying the molarity by the volume of the solution (in liters).

Step 3: Calculate the moles of HBr that are being added to the buffer solution. This can be done by dividing the mass of HBr (in grams) by its molar mass.

Step 4: Determine if the buffer can neutralize the added HBr. The buffer can neutralize the HBr if the moles of NO2- (the base) are greater than or equal to the moles of HBr (the acid). If the moles of HBr are greater than the moles of NO2-, then the buffer's capacity to neutralize the acid has been exceeded.

Step 5: If the buffer's capacity is exceeded, calculate by how much. This can be done by subtracting the moles of NO2- from the moles of HBr.

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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, the buffer is composed of HNO2 (a weak acid) and KNO2 (its conjugate base), which helps maintain the pH when HBr, a strong acid, is introduced.

Buffer Capacity

Buffer capacity refers to the amount of acid or base that a buffer solution can neutralize before a significant change in pH occurs. It depends on the concentrations of the weak acid and its conjugate base. In this scenario, the buffer's capacity will be tested by the addition of HBr, and determining whether the buffer can handle this addition is crucial for understanding its effectiveness.

Stoichiometry of Acid-Base Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions. For the buffer solution, the addition of HBr will react with the weak base (KNO2) present in the buffer. Calculating the moles of HBr added and comparing it to the moles of KNO2 will help determine if the buffer can neutralize the added strong acid without exceeding its capacity.

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Textbook Question

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

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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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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. b. 350 mg KOH

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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. d. 1.35 g HI

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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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Textbook Question

The graphs labeled (a) and (b) show the titration curves for two equal-volume samples of monoprotic acids, one weak and one strong. Both titrations were carried out with the same concentration of strong base.

(i) What is the approximate pH at the equivalence point of each curve?

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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

Verified Solution

Key Concepts

Buffer Solutions

Buffer Capacity

Stoichiometry of Acid-Base 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. c. 1.25 g HBr