Smaller, Larger, or the Same as the true molarity? Explain. Hint: This question is similar to the one about having an air bubble in your pitette tip, in an earlier lab..... -We added 20 mL of distilled water to the vinegar, but we did not use this volume in the calculation of molarity. Why do you think we are able to ignore this volume in the calculation?
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.
-Assume that your vinegar contained a small amount of citric acid (a triprotic acid). Using the same experimental data, would you expect the molarity of this sample to be the same or different than a sample which contained only pure acetic acid?
Hint:
A way to think of this question is you have a sample fo vinegar, and someone adds lemon juice to it (which contains acid). What will happen to the molarity of acid in the sample?
-Assume that the tip of your buret was not properly filled with NaOH solution. It contained an air bubble which was eliminated during the titration.
Would the calculated molarity of the vinegar be:
Smaller, Larger, or the Same
as the true molarity? Explain.
Hint:
This question is similar to the one about having an air bubble in your pitette tip, in an earlier lab.....
-We added 20 mL of distilled water to the vinegar, but we did not use this volume in the calculation of molarity.
Why do you think we are able to ignore this volume in the calculation?
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