Normality and Molarity in Solutions

The video tutorial by Irfan Sheikh on Pharma Game Insights explains how to prepare molar and normal solutions for both solids and liquids. It covers the definitions of molarity and normality, provides formulas for solution preparation, and includes examples for clarity. The video also discusses the preparation of liquid solutions, emphasizing the importance of using correct measurements and calculations. The tutorial concludes with a call to action for viewers to like, share, and subscribe.

What is the definition of molarity?

• The number of moles of solute in one liter of solution

• The number of grams of solute in one liter of solution

• The number of moles of solute in one kilogram of solvent

• The number of grams of solute in one kilogram of solvent

Which formula is used to calculate the weight of solute for a molar solution?

• Weight = Molarity x Molecular Weight x Volume / 1000

• Weight = Normality x Equivalent Weight x Volume / 1000

• Weight = Molarity x Volume / Molecular Weight

• Weight = Normality x Volume / Equivalent Weight

How much NaOH is needed to prepare 100 ml of a 0.5 molar solution?

• 4 grams

• 2 grams

• 1 gram

• 3 grams

What is normality in terms of solution concentration?

• The number of gram equivalent weight of solute in one liter of solution

• The number of moles of solute in one liter of solution

• The number of moles of solute in one kilogram of solvent

• The number of grams of solute in one liter of solution

How is the equivalent weight of a compound calculated?

• Molecular weight divided by the number of moles

• Molecular weight multiplied by the number of replaceable H+ or OH- ions

• Molecular weight divided by the number of replaceable H+ or OH- ions

• Molecular weight multiplied by the number of moles

What is the equivalent weight of NaOH?

• 40

• 30

• 20

• 50

What is the formula for preparing a molar solution of a liquid?

• V1 = Molarity x Molecular Weight x V2 / (Percentage x Density x 1000)

• V1 = Normality x V2 / (Equivalent Weight x Density x 1000)

• V1 = Normality x Equivalent Weight x V2 / (Percentage x Density x 1000)

• V1 = Molarity x V2 / (Molecular Weight x Density x 1000)

How much concentrated HCl is needed to prepare 500 ml of a 0.5 molar solution?

• 19.5 ml

• 18.5 ml

• 20.5 ml

• 21.5 ml

What is the percentage of sulfuric acid used in the example for preparing a normal solution?

• 99%

• 96%

• 97%

• 98%

How much concentrated H2SO4 is required to prepare 500 ml of a 0.5 normal solution?

• 7.8 ml

• 5.8 ml

• 6.8 ml

• 8.8 ml