A 0.6845 g sample of an unknown monoprotic acid requires 28.4 mL of 0.553 M NaOH for neutralization to a phenolphthalein end point. There are 7.35 mL of 0.914 M HCl used for back-titration. a. How many moles of OH¯ are used? Moles of OH moles OH" How many moles of H+ from HCl? Moles of H+ moles H* b. How many moles of H* are there in the solid acid? Moles H+ in solid acid = Moles OH in NAOH soln. – Moles Ht in HCl soln. Moles of H+ in the solid acid = moles H* in solid c. What is the molar mass of the unknown acid? с. Grams of acid Molar Mass = Moles of Ht ion furnished Molar Mass of the unknown acid |g/mol
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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