Some acids are polyprotic, meaning that they have two or more acidic protons in their formula. Phosphoric acid is an example of a triprotic acid, meaning that it has three acidic protons. The third equivalence point would be the volume of base required to neutralize all three-- the first, second, and third protons of the acid's formula. The calculation for the following problem will require the correct stoichiometry for this acid-base neutralization reaction to be used. Hint: Be careful about your molar ratio. How many mL of 0.101 M NaOH solution do we need to titrate 0.0250 L of 0.103 M H3PO4(aq) and reach the second equivalence point?
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.
Some acids are polyprotic, meaning that they have two or more acidic protons in their formula. Phosphoric acid is an example of a triprotic acid, meaning that it has three acidic protons. The third equivalence point would be the volume of base required to neutralize all three-- the first, second, and third protons of the acid's formula. The calculation for the following problem will require the correct stoichiometry for this acid-base neutralization reaction to be used. Hint: Be careful about your molar ratio.
How many mL of 0.101 M NaOH solution do we need to titrate 0.0250 L of 0.103 M H3PO4(aq) and reach the second equivalence point?
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
