5. Use the following reaction to answer each part of this question: NaCN + OH HCN (a) Label the acid, base, conjugate acid, and conjugate base. (b) What is the pKa of the acid and of the conjugate acid? + iONA ONa (c) What is the strongest acid in this reaction? (d) Does the equilibrium lie to the left (toward reactants) or to the right (toward products)?
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.
Acids and bases are two fundamental categories of substances in chemistry:
Acids: Acids are substances that can donate protons (H+ ions) when dissolved in water. They are characterized by a pH level less than 7 and have a sour taste. Common examples include hydrochloric acid (HCl) and citric acid (found in citrus fruits).
Bases: Bases are substances that can accept protons (H+ ions) or donate hydroxide ions (OH-) when dissolved in water. They typically have a pH level greater than 7 and have a bitter taste. Common examples include sodium hydroxide (NaOH) and ammonia (NH3).
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