Calculate the hydronium ion concentration and the pH when 70.0 mL of 0.75 M NH3 is mixed with 70.0 mL of 0.75 M HC1 ( K₁ = 5.6 × 10-¹0). Concentration = pH = Submit Answer Try Another Version M 2 item attempts remaining

Calculate the hydronium ion concentration and the pH when 70.0 mL of 0.75 M NH3 is mixed with 70.0 mL of 0.75 M HC1 ( K₁ = 5.6 × 10-¹0). Concentration = pH = Submit Answer Try Another Version M 2 item attempts remaining

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter8: Acids And Bases

Section: Chapter Questions

Problem 8.49P: 8-49 A solution of NaOH base was titrated with 0.150 M HCI, and 22.0 mL of acid was needed to reach...

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

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 hydronium ion concentration and the pH when 70.0 mL of 0.75 M
NH3 is mixed with 70.0 mL of 0.75 M
HC1 (
K₁ = 5.6 × 10-¹0).
Concentration =
pH =
Submit Answer
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M
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