H2Z is a diprotic acid with Ka1 = 3.0 × 10^-3 and Ka2 = 8.0 x 10^-8. Suppose you start with 1.00 L of 1.00 M H2Z(aq) and add 1.00 M KOH (aq) gradually. Calculate the pH at the following volumes of added strong base: a) 0.00 L; b) 0.50 L; c) 1.00 L; d) 1.50 L; e) 2.00 L. Report the pH values with 2 decimal places after dot. Write relevant chemical equations and show work on every part of this problem.
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.
H2Z is a diprotic acid with Ka1 = 3.0 × 10^-3 and Ka2 = 8.0 x 10^-8. Suppose you start with 1.00 L of
1.00 M H2Z(aq) and add 1.00 M KOH (aq) gradually. Calculate the pH at the following volumes of added strong base: a) 0.00 L; b) 0.50 L; c) 1.00 L; d) 1.50 L; e) 2.00 L. Report the pH values with 2 decimal places after dot. Write relevant chemical equations and show work on every part of this problem.
f. Sketch the titration curve
g. How many liters of 1.00 M KOH(ag) should be added to 1.00 L of 1.00 M H2Z to obtain a buffered solution with pH = 7.50? Hint to part g: you may calculate the moles of two salts in the buffer, then
moles of K* ions in the salt, and finally consider that all K* ions come from KOH(ag).
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