1 Ca(OH)2 +2 HBr - 1 CaBr2 + 2 H2O Concentration of base 2.5 M Final buret reading 16.8 mL Initial buret reading 10.6 mL Volume of base used (in mL) mL Volume of base used (in L) L Volume of acid used (in mL) 30 mL Volume of acid used (in L) Concentration of acid unknown Step1: determine the number of moles of base reacted. Put this in BCA table Step2: Use BCA table to calculate the number of moles of acid reacted Step3: calculate the concentration of the acid M of acid (round to 2 decimal places)
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.
![Use the data from the table and the balanced reaction to determine the concentration of the acid:
1 Ca(OH)2 + 2 HBr
- 1 CaBr2 + 2 H20
Concentration of base
2.5 M
Final buret reading
16.8 mL
Initial buret reading
10.6 mL
Volume of base used (in mL)
mL
Volume of base used (in L)
Volume of acid used (in mL)
30 mL
Volume of acid used (in L)
Concentration of acid
unknown
Step1: determine the number of moles of base reacted. Put this in BCA table
Step2: Use BCA table to calculate the number of moles of acid reacted
Step3: calculate the concentration of the acid
M of acid (round to 2 decimal places)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fca37b449-3abe-41b0-9001-82ec9a5dc31d%2F0b8c07e6-1471-4cd9-a0c8-ffcc45287a9d%2F5yzfy4q_processed.png&w=3840&q=75)
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