Consider a buffer comprised of a weak acid (HA), pKa = 5.0) and its conjugate base (A). Which of the following statements about this buffer is/are true? The buffer is better able to absorb excess base at pH 4 than at pH 6. At pH values lower than the pKa, the concentration of the weak acid (HA) is higher than the concentration of the conjugate base (A¯). The pH of a buffered solution will remain constant no matter how much acid or base is added to the solution. The capacity of the buffer would be increased if equal concentrations of HCI and NaOH were added. When the pH 5.0, the concentration of the weak acid (HA) is equal to the concentration of the salt (A¯). =
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.
Select all that apply!
Buffer solution : It is an acid or a base aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa.. Its pH changes very little when a small amount of strong acid or base is added to it.
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