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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Trial 1 |
Calculations |
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Weight of Antacid
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1.541 g |
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Concentration of HCl used |
0.500 M |
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Vol HCl added (mL) |
49.67 mL |
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Concentration of NaOH |
0.453 M |
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Total moles of HCl added |
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Moles HCl = Molarity x volume in liters |
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Initial buret reading (NaOH) |
25.65 mL |
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Final buret reading (NaOH) |
49.72 mL |
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Vol NaOH added (mL) |
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Final -Initial buret readings (NaOH) |
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Moles of NaOH used |
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Moles NaOH used = Molarity x volume in L |
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Moles of HCl neutralized by NaOH |
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Moles of HCl neutralized by NaOH = moles NaOH (1mole acid/1 mole base) |
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Moles of HCl neutralized by antacid |
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Moles of HCl neutralized by the antacid = total moles HCl added – moles HCl neutralized by NaOH |
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Moles of HCl consumed per gram of antacid |
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Moles of HCl consumed per gram of antacid= moles HCl neutralized by antacid/ grams of antacid |
Calculate the total moles of HCl added
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