What is the pH of a solution with a hydroxide concentration of 4.20 × 10^-5 M ? What is the pH of a solution with a hydrogen ion concentration of 6.25 × 10^ -6 M? What is the pOH of 1.95 M solution of hydroiodic acid? What is the pH of 1.20 M HCl solution? What is the pOH of a solution that has a pH of 11.1? The pH of a 1.80 M ammonia NH3 solution (Kb = 1.8 x 10^-5) is? What is the pH of a 3.95 M solution of HNO2 (Ka = 4.5 x 10^-4)? A 2.45 M solution of an unknown acid has a pH of 1.22. What is the Ka? What is the pH of a 2.95 M solution of NH4Cl (Kb of NH3= 1.8 x 10^-5)?
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.
Answer:-
This question is answered by using the simple concept of calculation of pH and pOH using the simple formulas. Using the experience of Ka and Kb , pH of each solution is calculated.
pH = - log[H3O+]
[OH-] x[H3O+] = Kw = 1.0 x 10-14
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