One method for chemical analysis involves finding a reactant that will precipitate the species of interest, but not the other species. The mass of the precipitate is then used to determine the mass of the species of interest present in the original sample. For example, calcium ions can be precipitated from an aqueous solution by adding of sodium oxalate Na2C2O4. The balanced equation is: Ca2+(aq) + Na2C2O4 (aq) --> CaC2O4 (s) + 2 Na+ (aq) Suppose you had a solution with approximately 15.0 g of calcium ions. Show by calculation whether the addition of 15.0 g of sodium oxalate will precipitate all of the calcium ions present in the sample.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
One method for chemical analysis involves finding a reactant that will precipitate the species of interest, but not the other species. The mass of the precipitate is then used to determine the mass of the species of interest present in the original sample. For example, calcium ions can be precipitated from an aqueous solution by adding of sodium oxalate Na2C2O4. The balanced equation is:
Ca2+(aq) + Na2C2O4 (aq) --> CaC2O4 (s) + 2 Na+ (aq) Suppose you had a solution with approximately 15.0 g of calcium ions.
Show by calculation whether the addition of 15.0 g of sodium oxalate will precipitate all of the calcium ions present in the sample.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
