The toughest part about titration is adding just enough of the titrant (NaOH, in this case). If you add the NaOH too quickly, you will likely end up adding too much ("overshooting the endpoint"). Alternatively, you could add it very slowly, drop-by-drop, but with this approach, you'll probably run out of time in the lab! The best option is to know in advance a rough idea of how much you'll need to add. Get close to this amount, then slow down and start adding NaOH in drop-fashion. Considering that the NaOH should be within a few percent of 0.30 M, what volume (in mL) would you expect to use for your third trial with 0.7943 g of KHP? Round your answer to 2 sig figs. Record this volume on your Cover Page and refer to it when performing your titration in Part 1.
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.
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