1.8 g of acetic acid (CH3COOH) is dissolved in 250 mL of water tò create an acidic solution. What volume of a 0.46 M calcium hydroxide solution is required to completely neutralize the acidic solution? State your answer in mL (without units). Hint: acetic acid is a weak monoprotic acid.
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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.
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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.
First of all, we calculate the Molarity of Acetic acid solution using Following formula -
Molarity of Acetic acid = mass×1000/Molar mass×volume of solution
Here,
Molarity of Acetic acid = ?
Mass of Acetic acid = 1.8 g
Molar mass of Acetic acid = 60.052 g/mol
Volume of solution = 250 mL
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