The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCH3CO₂ is a weak acid. 0.9 mol of NaOH is added to 1.0 L of a 0.9M HCH₂CO₂ 0 solution. 0.3 mol of NaOH is added to 1.0 L of a solution that is 0.8M in both HCH₂CO₂ and NaCH3CO2. U 0 O acids: bases: other: acids: bases: other: 0 X S
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.
Given -
1.Moles of NaOH = 0.9 mol
Volume of HCH3CO2 =1.0 L
Molarity of HCH3CO2 = 0.9M
2. Moles of NaOH = 0.3 mol
Volume of solution = 1.0L
Molarity of solution = 0.8M
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