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.
![Questions
• 1
• i. Sulfuric acid, H2SO4, is a strong acid and when in aqueous solution it dissociates almost completely into
hydrogen ions and sulfate ions.
• ii. Potassium hydroxide, KOH, is a strong base that is also soluble in water and so is called an alkali. It is
almost completely dissociated in aqueous solution into its component ions.
• iii. Sulfuric acid reacts with potassium hydroxide, in aqueous solution, to form a salt, which is itself fully
ionized, potassium sulfate.
. iv. Hydrochloric acid, HCI, reacts with solid calcium carbonate, CaCO3, limestone, to form a salt and water.
Carbon dioxide gas is given off.
• v. Carbonic acid and ethanoic (CH3COOH) acid are both weak acids and are predominantly in the molecular
form, although carbonic acid is easily decomposed at room temperatures into carbon dioxide and water.
• vi. Glycine is an amino acid, NH2CH2COOH. This molecule in acid solution forms a positive ion whereas in
alkaline solution a negative ion is produced.
• vii. Amino acids incorporated into proteins can act as pH controllers or 'buffers' to modify changes in acidity
or alkalinity.
. 2. What is meant by pH and how is it measured? What do all acids have in common?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d555b61-3806-4b51-bac5-95950c28cf38%2F5684606f-a278-4674-a3db-b79b8902491f%2Fjr3z7x_processed.jpeg&w=3840&q=75)
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