A friend of yours has to find the pH of a 1.0 x 10-8 M hydrochloric acid at 25˚C. Your friend notes that HCl is a strong acid and plugs [H+] = 1.0 x 10-8 M into pH = -log[H+]. She finds the pH to be 8.0. However, this value is basic, and HCl is a strong acid! a.) What went wrong? Why? (What other reactions can contribute to the [H+] in an aqueous solution?) b.) When do you need to worry about this problem affecting the pH you calculate? c.) Calculate the correct pH using an ICE table.
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.
3. A friend of yours has to find the pH of a 1.0 x 10-8 M hydrochloric acid at 25˚C. Your friend notes that HCl is a strong acid and plugs [H+] = 1.0 x 10-8 M into pH = -log[H+]. She finds the pH to be 8.0. However, this value is basic, and HCl is a strong acid!
a.) What went wrong? Why? (What other reactions can contribute to the [H+] in an aqueous solution?)
b.) When do you need to worry about this problem affecting the pH you calculate?
c.) Calculate the correct pH using an ICE table.
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