d. A 15.00 mL sample of a solution of H2SO4 of unknown concentration was titrated with 0.3200 N NaOH. The titration required 21.30 mL of the base. Assuming complete neutralization of the acid, i) What was the normality of the acid solution? ii) What was the molarity of the acid solution?
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.
![Show all setups. Be careful with significant figures.
a. Calculate the volume of 0.450 M Ba(OH)2 which will be needed to neutralize 46.00 mL of
0.252 M HC1.
b. Find the molar concentration of a sulfuric acid solution, 35.00 mL of which neutralizes
25.00 mL of 0.320 M NaOH. (Careful! Sulfuric acid is diprotic!)
c. Calculate the “molarity of water" [H2O] in pure water at 30C. [Hint: The density of water
at 30°C is 0.9957 g/mL.]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48488273-ed4c-408c-b0f1-f07ef553f0b6%2F13a604fc-721c-4e62-bc7d-a5ad6f7b9208%2Fkvnvgtn_processed.png&w=3840&q=75)
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