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Chemical concentrations: Molar concentration, Analytical molarity, Equilibrium molarity of a particular species, Percent concentration, Parts per million/billion (ppm/ppb), Volume ratios for dilution procedures. notes for this bsc students in the form of ppt
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Chemical Concentrations
1. Molar Concentration (Molarity)
Definition: Moles of solute per liter of solution.
Formula: M = moles of solute / liters of solution
Example: A 1 M solution of NaCl contains 1 mole of NaCl dissolved in 1 liter of solution.
2. Analytical Molarity
Definition: The total concentration of a species in solution, regardless of its chemical form.
Example: A solution containing 0.1 M FeCl3 has an analytical molarity of 0.1 M for Fe(III) even though some of it may exist as FeCl4-.
3. Equilibrium Molarity
Definition: The concentration of a species at equilibrium, taking into account any reactions that may have occurred.
Example: In a solution of acetic acid (CH3COOH), the equilibrium molarity of H+ is less than the analytical molarity of acetic acid due to the dissociation equilibrium.
4. Percent Concentration
Definition: Expresses the amount of solute as a percentage of the total solution or solvent.
Types:
Weight/Weight (% w/w): grams of solute per 100 grams of solution.
Weight/Volume (% w/v): grams of solute per 100 mL of solution.
Volume/Volume (% v/v): mL of solute per 100 mL of solution.
5. Parts per Million (ppm) and Parts per Billion (ppb)
Definition: Units of concentration used for very dilute solutions.
Formula: ppm = (mass of solute / mass of solution) x 10^6
Example: 1 ppm of a substance means that there is 1 mg of the substance in 1 kg of solution.
6. Volume Ratios for Dilution Procedures
Formula: M1V1 = M2V2
M1: Initial molarity
V1: Initial volume
M2: Final molarity
V2: Final volume
Example: To prepare 500 mL of a 0.5 M solution from a 1 M stock solution, use the formula to calculate the required volume of the stock solution.
Important Notes
Concentration units are important and must be carefully considered when making calculations.
Temperature affects the solubility of solutes and therefore the concentration of solutions.
Dilution is a process of decreasing the concentration of a solution by adding more solvent.
For a more detailed explanation and examples, refer to your chemistry textbook or online resources.
1. Molar Concentration (Molarity)
Definition: Moles of solute per liter of solution.
Formula: M = moles of solute / liters of solution
Example: A 1 M solution of NaCl contains 1 mole of NaCl dissolved in 1 liter of solution.
2. Analytical Molarity
Definition: The total concentration of a species in solution, regardless of its chemical form.
Example: A solution containing 0.1 M FeCl3 has an analytical molarity of 0.1 M for Fe(III) even though some of it may exist as FeCl4-.
3. Equilibrium Molarity
Definition: The concentration of a species at equilibrium, taking into account any reactions that may have occurred.
Example: In a solution of acetic acid (CH3COOH), the equilibrium molarity of H+ is less than the analytical molarity of acetic acid due to the dissociation equilibrium.
4. Percent Concentration
Definition: Expresses the amount of solute as a percentage of the total solution or solvent.
Types:
Weight/Weight (% w/w): grams of solute per 100 grams of solution.
Weight/Volume (% w/v): grams of solute per 100 mL of solution.
Volume/Volume (% v/v): mL of solute per 100 mL of solution.
5. Parts per Million (ppm) and Parts per Billion (ppb)
Definition: Units of concentration used for very dilute solutions.
Formula: ppm = (mass of solute / mass of solution) x 10^6
Example: 1 ppm of a substance means that there is 1 mg of the substance in 1 kg of solution.
6. Volume Ratios for Dilution Procedures
Formula: M1V1 = M2V2
M1: Initial molarity
V1: Initial volume
M2: Final molarity
V2: Final volume
Example: To prepare 500 mL of a 0.5 M solution from a 1 M stock solution, use the formula to calculate the required volume of the stock solution.
Important Notes
Concentration units are important and must be carefully considered when making calculations.
Temperature affects the solubility of solutes and therefore the concentration of solutions.
Dilution is a process of decreasing the concentration of a solution by adding more solvent.
For a more detailed explanation and examples, refer to your chemistry textbook or online resources.
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