Calculate the pH of an aqueous 0.629 M CH3CH₂NH3Cl solution. The K₂ of CH3CH₂NH₂ (ethylamine) is 5.6 × 10-4.Report your answer to two decimal places. Example: 7.00Type your answer... Calculate the pH of a 0.44 M HF solution at 25 °C.HF (aq) = H+ (aq) + F¯ (aq), K₂ = 6.9 × 10-4 at 25 °CReport your answer to three significant figures.Type your answer...

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Calculate the pH of an aqueous 0.629 M CH3CH₂NH3Cl solution. The K of CH3CH₂NH₂ (ethylamine) is 5.6 × 10-4. Report your answer to two decimal places. Example: 7.00 Type your answer...

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.15QAP

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Concept explainers

Ionic Equilibrium

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Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Calculate the pH of an aqueous 0.629 M CH3CH₂NH3Cl solution. The K₂ of CH3CH₂NH₂ (ethylamine) is 5.6 × 10-4.
Report your answer to two decimal places. Example: 7.00
Type your answer...

Calculate the pH of a 0.44 M HF solution at 25 °C.
HF (aq) = H+ (aq) + F¯ (aq), K₂ = 6.9 × 10-4 at 25 °C
Report your answer to three significant figures.
Type your answer...

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