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.
Calculate the molar solubility and solubility product of Ca(OH)2 for each trial. Thank you!
![Concentration of standardized HCl solution (M)
0.0646
Part A
Trial 1
Trial 2
Volume of sample analyzed (mL)
25.00
25.00
Initial buret reading (mL)
0.75
26.03
Final buret reading (mL)
25.80
50.40](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc0000f46-99cd-4ff7-a4f7-2945716c158c%2F7f3dd2f2-8414-477f-9176-13843bd07876%2Fhk859re_processed.jpeg&w=3840&q=75)
![Prenare a clean 50 mL buret for titration. Rinse the buret and tip with three 5 mL portions of the
1.
standardized 0.05 M HCI solution and discard. Fill the buret with standardized 0.05 M HCI, remove the air
bubbles in the buret tip, and, after 10-15 seconds, read and record the initial volume using all certain digits
(from the labeled calibration marks on the buret) plus one uncertain digit (the last digit which is the best
timate between the calibration marks). Place a sheet of white paper beneath the receiving flask to make
the end point of the titration easier to see.
Part A- Molar Solubility and Solubility Product of Calcium Hydroxide
Obtain a sample of saturated Ca(OH)2 solution (without added CaCl2) from your instructor.
2.
, Pinet 25 mL of the saturated Ca(OH)2 solution into a 125 mL flask and add 2 drops of methyl orange
indicator.
4 Titrate the Ca(OH)2 solution to the methyl orange endpoint, where the color changes from yellow to red.
Remember, the addition of HCl should stop within one-half drop of the end point. Read and record the final
volume of standard HCl in the buret.
5. Titrate an additional 25 mL aliquot of the saturated Ca(OH)2 solution.
Data Analysis
Calculate the molar solubility and solubility product of Ca(OH)2 for each trial and report their average values.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc0000f46-99cd-4ff7-a4f7-2945716c158c%2F7f3dd2f2-8414-477f-9176-13843bd07876%2F6ik56j_processed.jpeg&w=3840&q=75)
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