Answered: Calculate the pH of each of the…

Calculate the pH of each of the following strong acid solutions. (a) 0.00483 M HNO3 pH (b) 0.501 g of HBr in 46.0 L of solution pH (c) 45.0 mL of 6.10 M HNO3 diluted to 3.60 L pH

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.37QAP

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Concept explainers

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 pH of each of the following strong acid solutions.

(a) 0.00483 M HNO₃

pH

(b) 0.501 g of HBr in 46.0 L of solution

pH

(c) 45.0 mL of 6.10 M HNO₃ diluted to 3.60 L

pH

(d) a mixture formed by adding 78.0 mL of 0.00338 M HNO₃ to 80.0 mL of 0.000570 M HBr

pH

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