Determine the pH of the following: a single solution prepared to final concentrations of 0.01469 M HCl and 0.01469 M NaOH. a single solution prepared to final concentrations of 0.01469 M H2SO4 (assume complete dissociation) and 0.01469 M HCl.
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.
Determine the pH of the following:
a single solution prepared to final concentrations of 0.01469 M HCl and 0.01469 M NaOH.
a single solution prepared to final concentrations of 0.01469 M H2SO4 (assume complete dissociation) and 0.01469 M HCl.
pH is the negative logarithm of hydrogen ion concentration. When an acid is mixed with a base, both of these reacts together and form salt and water.
According to normality equation,
NV= N1V1-N2V2
Here N represents the concentration of hydrogen ion after mixing the acid and base. N1, N2 represents the concentration of acid and base respectively. V1 and V2 show the volume of acid and base respectrively.
Here the concentrations of HCl and NaOH are 0.01469M.Both have equal concentrations, so its hydrogen ion after mixing cannot be predicted.
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