Sample 1 43.07 g 42.05 g 1.02 g 8.95 mL .98 mL Sample 2 42.77 g 41.09 g 1.68 g 22.66 mL 8.95 mL 13.71 mL Mass of flask and KHP Mass of empty flask Mass of KHP Final buret reading Initial buret reading Volume of base used 7.97 mL Calculations: In the spaces below, show calculation set-ups for Sample 1 only. Show the answers for both samples in the boxes. Remember to use the correct number of significant figures in all calculations. (Ex. The number 0.005 has only 1 significant figure.) Calculations Table Sample 1 = 0.00499 moles KHP 1.68 g x 1 mole = 0.00822 moles KHP Sample 2 1. Moles of acid (KHP, molar mass = 204.2 1.02 g x 1 mole 204.2 g/mole 204.2 g/mole g/mole). Show calculations for Sample 1 here. 2. Moles of base used to neutralize the acid above. Show calculations for Sample 1 here. 3. Molarity of base (N2OH). Show calculations for Sample 1 here.
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.
Titration lab - need help with the following questions and how to set up the formulas, thank you!
Moles of base used to neutralize a base of 7.97 ml (sample 1) and 13.71 ml (sample 2)
Molartity of base (NaOH)
Average molarity of base
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