Calculate the pH of the following strong acid solution: 1.52 g of HNO, dissolved in 575 mLof solution. Molar mass of HNO;: 63 g molO a. 1.52 Which of the following substances are more soluble in acidicsolution than in basic solution?I. CaCO3II. NANO3III. Mg(OH)2IV. BaF2

Given: Mass of HNO3 = 1.52 gm Volume of solution = 575 ml Molar mass of HNO3 = 63 g/mol

Answered: Calculate the pH of the following…

Calculate the pH of the following strong acid solution: 1.52 g of HNO, dissolved in 575 mL of solution. Molar mass of HNO;: 63 g mol O a. 1.52

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.27E

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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.

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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 the following strong acid solution: 1.52 g of HNO, dissolved in 575 mL
of solution. Molar mass of HNO;: 63 g mol
O a. 1.52

Which of the following substances are more soluble in acidic
solution than in basic solution?
I. CaCO3
II. NANO3
III. Mg(OH)2
IV. BaF2

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