Podcast
Questions and Answers
A 70% (w/w) solution of nitric acid means that it contains 70 g of nitric acid per 100 g of solution.
A 70% (w/w) solution of nitric acid means that it contains 70 g of nitric acid per 100 g of solution.
True (A)
Volume percent is typically used to specify the concentration of a solution by diluting a solid compound with a liquid.
Volume percent is typically used to specify the concentration of a solution by diluting a solid compound with a liquid.
False (B)
A 5% (v/v) aqueous solution of methanol is prepared by diluting 5.0 mL of methanol with enough water to give 100 mL.
A 5% (v/v) aqueous solution of methanol is prepared by diluting 5.0 mL of methanol with enough water to give 100 mL.
True (A)
Weight to volume percent is often used to describe the concentration of concentrated aqueous solutions.
Weight to volume percent is often used to describe the concentration of concentrated aqueous solutions.
Parts per Million (ppm) is a convenient way to express concentration for concentrated solutions.
Parts per Million (ppm) is a convenient way to express concentration for concentrated solutions.
When 20 ml of 10 N HCl are diluted with distilled water to form one liter of the solution, the normality of the diluted solution remains 10 N.
When 20 ml of 10 N HCl are diluted with distilled water to form one liter of the solution, the normality of the diluted solution remains 10 N.
Molarity is the number of moles of a solvent that is contained in 1 liter of the solution.
Molarity is the number of moles of a solvent that is contained in 1 liter of the solution.
Normality is the number of equivalents of solute that is contained in 1 liter of solution.
Normality is the number of equivalents of solute that is contained in 1 liter of solution.
Weight percent is a common method used to express the concentration of commercial aqueous reagents.
Weight percent is a common method used to express the concentration of commercial aqueous reagents.
For salt, the calculation of (n) is the total number of replaceable H+1 ions.
For salt, the calculation of (n) is the total number of replaceable H+1 ions.
In a 2M H2SO4 solution, the molar mass of H2SO4 is 49g/mol.
In a 2M H2SO4 solution, the molar mass of H2SO4 is 49g/mol.
In a 500ml solution, if 0.4g of NaOH (40g/mol) is dissolved, the molarity of the solution is 0.08M.
In a 500ml solution, if 0.4g of NaOH (40g/mol) is dissolved, the molarity of the solution is 0.08M.
Flashcards
70% w/w Solution
70% w/w Solution
Contains 70 g of solute in 100 g of solution.
Volume Percent
Volume Percent
Specifies concentration by volume of liquid in the solution.
5% v/v Aqueous Solution
5% v/v Aqueous Solution
5.0 mL of solute diluted to a final volume of 100 mL.
Weight to Volume Percent
Weight to Volume Percent
Signup and view all the flashcards
Parts per Million (ppm)
Parts per Million (ppm)
Signup and view all the flashcards
Normality
Normality
Signup and view all the flashcards
Molarity Misconception
Molarity Misconception
Signup and view all the flashcards
Weight Percent
Weight Percent
Signup and view all the flashcards
Acid H+ Ions Calculation
Acid H+ Ions Calculation
Signup and view all the flashcards
Molar Mass of H2SO4
Molar Mass of H2SO4
Signup and view all the flashcards
Molarity Calculation
Molarity Calculation
Signup and view all the flashcards
Dilution Law
Dilution Law
Signup and view all the flashcards
Study Notes
Molar Concentration (Molarity)
- Molarity is the number of moles of a solute in 1 liter of the solution.
- Example: 2.30g of C2H5OH in 3.50 L of solution has a certain molar concentration.
- Molarity can be calculated using the formula: Molarity = number of moles of solute / volume of solution (in liters).
Examples of Molarity Calculations
- Example 1: Calculate the molar concentration of ethanol in an aqueous solution.
- Example 2: Determine the mass of H2SO4 in a 2M solution.
- Example 3: Calculate the molarity of a solution of NaOH.
- Example 4: Calculate the molarity of a solution of sodium metal.
Normal Concentration (Normality)
- Normality is the number of equivalents of solute in 1 liter of solution.
- Calculation of normality (n) for acid: n = number of replaceable H+1.
- Calculation of normality (n) for base: n = number of replaceable OH-1.
- Calculation of normality (n) for salt: n = total number of positive or negative charge.
- Example: Find the normality of H2SO4 in a 500ml solution.
Percent Concentration
- Percent concentration is a way to express the concentration of a solution.
- Three common methods are: weight percent, volume percent, and weight to volume percent.
- Example: A 5% (w/v) aqueous solution of silver nitrate.
Parts per Million (ppm)
- ppm is a convenient way to express concentration for very dilute solutions.
- A handy rule: for dilute aqueous solutions, 1 ppm = 1.00 mg/L.
Dilution
- Example: A 20 ml of 10 N HCl is diluted with distilled water to form one liter of the solution.
- What is the normality of the diluted solution?
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
