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Conclusion


NaOH(aq)+1KHP(s)<===>H2O(l)+KP¯¹(aq)

This simple experiment consisted of only one titration repeated twice for greater accuracy and precision to the actual values. The reaction that took place is written as

NaOH(aq)+1KHP(s)<===>H2O(l)+KP¯¹(aq)

====== Equilibrium ======

This equation represents the reaction that takes place when the ratio of the concentration of NaOH to KHP = 1/1. At this point, the chemical compound reaches equilibrium, and reacts untill it stops in a favored state. This chemical reacted fully with the addition of the final drop, proving that the concentrations must reach an exact ratio to react. When this ratio occoured, the base (NaOH), and the acid (KPH) acted to neutralize each other, forming water and salt. As this is a reversible reaction, adding more KHP would of caused the pink solution to revert to the origional state with an inbalance of KHP and NaOH.