Use the References An aqueous solution of trichloroacetic acid, that is 3.00 percent by weight trichloroacetic acid, has a density of 1.0133 g/mL. A student determines that the freezing point of this solution is -0.611 °C. Based on the observed freezing point, what is the percent ionization of the acid and the value of Ka? K for H₂O is 1.86 °C/m. % ionized- K₂ W
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 the weight percent of trichloroacetic acid(CCl3COOH) = 3.00 % w/w
So 100 g of the solution has 3.00 g trichloroacetic acid(CCl3COOH) and 100-3.00 = 97.0 g of solvent water.
First, we have to find the molality(m) of the solution from this data.
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