t. Turn in Post-Lab Report (Use the In-lab observations to complete the laboratory report. to your Instructor when you have completed the report.) 25 0.05 20 Temperature of the Lab Concentration of HCI used Volume saturated Ca(OH), used Volume HCI used Average Volume HCI. Average conc. of [OH-] Average conc. of [Ca²+] K of Ca(OH)₂ Molar solubility Ca(OH)₂ Solubility of Ca(OH)₂ Show calculation of K Trial 1 7.8 mL mL Trial 2 7.7 M M mL °C M mL Trial 3 7.7 mL Show calculation of [OH-] mol/L Show calculation of [Ca²+] g/L Show calculation of molar solubility and solubility in g/L of Ca(OH)₂ POST-LAB
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.
![Laboratory 10
Determination of the K of a
Slightly Soluble Compound
NAME:
TA:
Temperature of the Lab
Concentration of HCI used
Volume saturated Ca(OH), used
Post-Lab Report (Use the In-lab observations to complete the laboratory report. Turn in
to your Instructor when you have completed the report.)
25
0.05
20
Volume HCI used
Average Volume HCI
Average conc. of [OH-]
Average conc. of [Ca²+]
K of Ca(OH)₂
Molar solubility Ca(OH)₂
Solubility of Ca(OH)₂
Show calculation of K
Trial 1
7.8
mL
mL
Trial 2
7.7
M
M
LABORATORY 10 | DETERMINATION OF THE K
DATE:
mL
SECTION:
°C
M
mL
Trial 3
7.7
mL
Show calculation of [OH-]
mol/L Show calculation of [Ca²+]
g/L
Show calculation of molar solubility and solubility in g/L of Ca(OH)₂
143
POST-LAB](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff9c7da2c-77cf-406e-8958-b4c26bba595a%2F4e122359-0c2a-4a8d-be71-8ab6b4083220%2F9df5h7t_processed.jpeg&w=3840&q=75)
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