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 pH of each of the following mixtures.
500 ml 0.35 M KOH + 500 ml 0.25 M HNO3
500 ml 0.35 M CH3CH2NH2 + 500 ml 0.25 M HNO3
500 ml 0.35 M HCl + 500 ml 0.25 M CH3CH2NH2
500 ml 0.35 M HF + 500 ml 0.25 M KOH
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The mixture will go through a neutralization reaction
Molarity of KOH=0.35 M
Given Volume of KOH= 500ml = 0.5 L
So, Number of moles of KOH = Molarity x Volume = 0.35 x 0.5 = 0.175 mol
Molarity of = 0.25 M
Given Volume = 500ml = 0.5 L
So, Number of moles of = Molarity x Volume = 0.25 x 0.5= 0.125 mol
We can see that, Number of moles of KOH > Number of moles of
Therefore, is the limiting reagent and there will be KOH remaining.
The reaction will continue until all is consumed
Number of moles of KOH remaining = 0.175-0.125 = 0.050 moles
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