1. If you had to make a 0.750M solution of Na₂CO3 from 100mL of solution, determine the mass of Sodium Carbonate necessary. 2. If you had to make a 0.250M solution of CaCl2 from 100mL of solution, determine the mass of Calcium Chloride necessary. 100 ml of the Sodium Carbonate solution from #1 and an excess of Calcium
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.
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Chem 105 Online
Safety:
While these are household items that you could easily purchase at the store, please understand
that this is still for chemistry purposes. Do not INGEST anything or leave readily available for pets
and young children to get into (especially your chalk, um-I mean your final precipitate). All
items can be thrown away at the end. Ice melt solutions can be thrown away outside away
from pet areas. Even though Calcium Carbonate is relatively harmless-please note that this
should not be ingested.
Prelab:
1. If you had to make a 0.750M solution of Na2CO3 from 100mL of solution, determine the
mass of Sodium Carbonate necessary.
2. If you had to make a 0.250M solution of CaCl2 from 100mL of solution, determine the
mass of Calcium Chloride necessary.
3. If you use 10.0 mL of the Sodium Carbonate solution from #1 and an excess of Calcium
Chloride, how many grams of Calcium Carbonate should be theoretically be produced?
4. If you use 25.0 mL of the Calcium Chloride solution from #2 and an excess of Sodium
Carbonate, how many grams of Calcium Carbonate should be theoretically be
produced?
5. Using your answers from problems 3 and 4, what is the theoretical yield of 25.0mL of a
0.250M solution of CaCl2 when mixed with 10.0 mL of a 0.750M Sodium Carbonate
solution?
6.
Suppose the student performs the experiment in the previous problem, what is the
percent yield if they generate 0.565g of CaCO3?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa7e1480f-493b-4334-b48e-1a7032a37693%2Ffb2aeec1-118b-4660-9a0b-bb0e3217a307%2F1hsj50c_processed.jpeg&w=3840&q=75)
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