The mass of $CaCO_3$ produced when carbon dioxide is bubbled through 500 mL of 0.5 M $Ca(OH)_2$ will be
- 10 g
- 20 g
- 50 g
- 25 g
The Correct Option is D
Solution and Explanation
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Notes on Mole concept and Molar Masses
Concepts Used:
Mole Concept
In the field of chemistry, a mole is defined as the amount of a substance that contains exactly 6.02214076 * 1023 βelementary entitiesβ of the given substance.
The number 6.02214076*1023 is popularly known as the Avogadro constant and is often denoted by the symbol βNAβ. The elementary entities that can be represented in moles can be atoms, molecules, monoatomic/polyatomic ions, and other particles (such as electrons).
For example, one mole of a pure carbon-12 (12C) sample will have a mass of exactly 12 grams and will contain 6.02214076*1023 (NA) number of 12C atoms. The number of moles of a substance in a given pure sample can be represented by the following formula:
n = N/NA
Where n is the number of moles of the substance (or elementary entity), N is the total number of elementary entities in the sample, and NA is the Avogadro constant.
The word βmoleβ was introduced around the year 1896 by the German chemist Wilhelm Ostwald, who derived the term from the Latin word moles meaning a βheapβ or βpile.
The mole concept refers to the atomic mass of a mole that is measured in grams. The gram atomic mass of an element is known as a mole. The mole concept combines the mass of a single atom or molecule in a.m.u. to the mass of a large group of comparable molecules in grams. Atomic mass is the mass of a single atom, whereas molecular mass is the mass of a group of atoms.
The Formula of Mole Concept
The number of units that make up a mole has been calculated to be 6.022 Γ10Β²Β³. The fundamental constant is also known as Avogadro's number (NA) or Avogadro constant. This constant is appropriately represented in chemistry using an explicit unit termed per mole.
Number of Moles = (Mass of the Sample)/(Molar Mass)
Read More: Mole Fraction