Calculate the pH of each of the following strong acid solutions. (a) 0.00251 M HIO4 pH = (b) 0.432 g of HNO3 in 38.0 L of solution pH = (c) 66.0 mL of 4.80 M HIO4 diluted to 1.60 L pH =
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.
Calculate the pH of each of the following strong acid solutions.
(a) 0.00251 M HIO4
pH =
(b) 0.432 g of HNO3 in 38.0 L of solution
pH =
(c) 66.0 mL of 4.80 M HIO4 diluted to 1.60 L
pH =
(d) a mixture formed by adding 30.0 mL of 0.00363 M HIO4 to 33.0 mL of 0.00853 M HNO3
pH =
Step by step
Solved in 2 steps with 2 images
