a. Balance the above chemical equation. b. Calculate the concentration (in molarity) of H3O+ in the prepared dilute solution of sulfuric acid. c. The strength of an acid can be measured by of the molar concentration of hydronium H3O+ (usually denoted as [H3O+]) produced when acid dissociates in water. The greater the [H3O+] the stronger is the acid. The value of [H3O+] is usually low especially for the so-called weak acids, thus, we usually express [H3O+] in terms of pH, which is pH = – log ([H3O+]/co) where co is the standard molar concentration equal to 1.00 M. We will learn more about these aspects of acid-base chemistry in this “Acid-base equilibria” unit of this course. Sulfuric acid is a strong acid (acids with pH < 7.00). Using the result in item 3.b, calculate the pH of the dilute sulfuric acid described above.
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.
In the chemistry lab, aqueous solutions of sulfuric acid are usually prepared from a concentrated reagent of this acid which has a concentration of 18.4 M. To prepare a dilute solution of this acid, 1.00 mL of the concentrated reagent is dissolved in enough water and the volume of the mixture is adjusted to 1.00 L. In this process, sulfuric acid reacts with water to produce hydronium and sulfate ions,
H2SO4(aq) + H2O(l) → H3O+(aq) + SO42-(aq)
This reaction is known as acid-dissociation reaction. It is an example of an acid-base reaction where the acid (sulfuric acid) transfer its protons (H+) to a base (water).
a. Balance the above chemical equation.
b. Calculate the concentration (in molarity) of H3O+ in the prepared dilute solution of sulfuric acid.
c. The strength of an acid can be measured by of the molar concentration of hydronium H3O+ (usually denoted as [H3O+]) produced when acid dissociates in water. The greater the [H3O+] the stronger is the acid. The value of [H3O+] is usually low especially for the so-called weak acids, thus, we usually express [H3O+] in terms of pH, which is
pH = – log ([H3O+]/co)
where co is the standard molar concentration equal to 1.00 M. We will learn more about these aspects of acid-base chemistry in this “Acid-base equilibria” unit of this course.
Sulfuric acid is a strong acid (acids with pH < 7.00). Using the result in item 3.b, calculate the pH of the dilute sulfuric acid described above.
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