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Questions and Answers
What is the primary purpose of volumetric analysis?
What is the primary purpose of volumetric analysis?
- To determine the concentration of solutions (correct)
- To measure the mass of a solid compound
- To analyze the temperature of a reaction
- To isolate chemical compounds from mixtures
Which step is NOT part of preparing a 0.1 N Sodium Hydroxide solution?
Which step is NOT part of preparing a 0.1 N Sodium Hydroxide solution?
- Heating the solution to 80°C (correct)
- Diluting to volume in a volumetric flask
- Dissolving in carbon dioxide free water
- Weighing 4.5 grams of sodium hydroxide
What is the purpose of using potassium biphthalate in the standardization of the sodium hydroxide solution?
What is the purpose of using potassium biphthalate in the standardization of the sodium hydroxide solution?
- To lower the pH of the solution
- To increase the volume of the solution
- To act as a color indicator
- To serve as a primary standard (correct)
What indicates the endpoint of the titration between sodium hydroxide and potassium biphthalate?
What indicates the endpoint of the titration between sodium hydroxide and potassium biphthalate?
What initial treatment is necessary for potassium biphthalate before it is used in the standardization process?
What initial treatment is necessary for potassium biphthalate before it is used in the standardization process?
When preparing a volumetric solution, what is the reason for using carbon dioxide free water?
When preparing a volumetric solution, what is the reason for using carbon dioxide free water?
During a neutralization reaction, what are the products formed?
During a neutralization reaction, what are the products formed?
Which is a critical step to take after diluting the sodium hydroxide solution in a volumetric flask?
Which is a critical step to take after diluting the sodium hydroxide solution in a volumetric flask?
What is the purpose of weighing anhydrous sodium carbonate before beginning the standardization of hydrochloric acid solution?
What is the purpose of weighing anhydrous sodium carbonate before beginning the standardization of hydrochloric acid solution?
At what temperature should anhydrous sodium carbonate be heated prior to weighing?
At what temperature should anhydrous sodium carbonate be heated prior to weighing?
What indicator is used during the titration of hydrochloric acid solution in this experiment?
What indicator is used during the titration of hydrochloric acid solution in this experiment?
How much anhydrous sodium carbonate is equivalent to 1 mL of 1N hydrochloric acid?
How much anhydrous sodium carbonate is equivalent to 1 mL of 1N hydrochloric acid?
What is the final color change expected when the titration with hydrochloric acid reaches the endpoint?
What is the final color change expected when the titration with hydrochloric acid reaches the endpoint?
Why is it necessary to repeat the titration procedure and conduct three trials?
Why is it necessary to repeat the titration procedure and conduct three trials?
Which of the following concentrations exceeds the handling precautions for hydrochloric acid?
Which of the following concentrations exceeds the handling precautions for hydrochloric acid?
What is the primary aim of standardizing a hydrochloric acid solution?
What is the primary aim of standardizing a hydrochloric acid solution?
Why is laboratory grade hydrochloric acid unsuitable as a primary standard?
Why is laboratory grade hydrochloric acid unsuitable as a primary standard?
What is the purpose of standardization in this experiment?
What is the purpose of standardization in this experiment?
Which of the following steps is NOT part of preparing a 1N hydrochloric acid solution?
Which of the following steps is NOT part of preparing a 1N hydrochloric acid solution?
What is the formula used to compute the normality of a solution?
What is the formula used to compute the normality of a solution?
What type of solution is used to standardize hydrochloric acid in this experiment?
What type of solution is used to standardize hydrochloric acid in this experiment?
Which procedure step should be done first when preparing the hydrochloric acid solution?
Which procedure step should be done first when preparing the hydrochloric acid solution?
What does the term 'primary standard' refer to in this context?
What does the term 'primary standard' refer to in this context?
Which property of sodium carbonate makes it suitable for standardizing hydrochloric acid?
Which property of sodium carbonate makes it suitable for standardizing hydrochloric acid?
What is the purpose of an indicator in a titration?
What is the purpose of an indicator in a titration?
What represents the endpoint in a titration process?
What represents the endpoint in a titration process?
How is normality calculated based on the weight of potassium biphthalate?
How is normality calculated based on the weight of potassium biphthalate?
What is the significance of the equivalence point in titration?
What is the significance of the equivalence point in titration?
What is the acceptable percentage range for sodium bicarbonate in tablets according to specifications?
What is the acceptable percentage range for sodium bicarbonate in tablets according to specifications?
What quantity does 1 mL of 0.1 N NaOH equate to in milligrams of potassium biphthalate?
What quantity does 1 mL of 0.1 N NaOH equate to in milligrams of potassium biphthalate?
In the purity determination formula, what does the denominator represent?
In the purity determination formula, what does the denominator represent?
What is the primary objective of performing a titration on sodium bicarbonate tablets?
What is the primary objective of performing a titration on sodium bicarbonate tablets?
What visual change indicates the endpoint of the titration of sodium hydroxide with sulfuric acid?
What visual change indicates the endpoint of the titration of sodium hydroxide with sulfuric acid?
What is the normality of the sulfuric acid solution prepared from 49.04 g of H2SO4 in 1000 mL?
What is the normality of the sulfuric acid solution prepared from 49.04 g of H2SO4 in 1000 mL?
Which indicator is mentioned for use in standardizing sulfuric acid solution against sodium hydroxide?
Which indicator is mentioned for use in standardizing sulfuric acid solution against sodium hydroxide?
What type of acid-base reaction occurs when sulfuric acid is titrated with sodium hydroxide?
What type of acid-base reaction occurs when sulfuric acid is titrated with sodium hydroxide?
How much concentrated sulfuric acid is needed to prepare 1000 mL of a 1 N solution?
How much concentrated sulfuric acid is needed to prepare 1000 mL of a 1 N solution?
What is the pH of the resulting solution at the endpoint when titrating a strong acid with a strong base?
What is the pH of the resulting solution at the endpoint when titrating a strong acid with a strong base?
What is the outcome of titrating sulfuric acid with sodium hydroxide?
What is the outcome of titrating sulfuric acid with sodium hydroxide?
How many trials of titration should be performed during the standardization?
How many trials of titration should be performed during the standardization?
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Study Notes
Preparation and Standardization of 1N Hydrochloric Acid Solution
- Use 150 mg of anhydrous sodium carbonate, preheated at 270°C for 1 hour, for accurate results.
- Dissolve sodium carbonate in 100 mL of distilled water and add 2 drops of methyl orange as an indicator.
- Titrate until color changes from yellow to orange, indicating the endpoint.
- Each 52.99 mg of sodium carbonate equals 1 mL of 1N hydrochloric acid.
- Calculate normality using formula: Normality = gm/mEq x mL consumed in HCl solution.
- Hydrochloric acid can be concentrated up to 40%, necessitating special handling due to evaporation.
Preparation and Standardization of 0.1N Sodium Hydroxide Solution
- Weigh 4.5 grams of sodium hydroxide pellets and dissolve in carbon dioxide-free water.
- Transfer to a 1 liter volumetric flask and dilute to volume with carbon dioxide-free water.
- Store the prepared NaOH in a labeled 1L stock bottle.
Standardization of 0.1N Sodium Hydroxide Solution
- Use 100 mg of potassium biphthalate, dried at 120°C for 2 hours, for standardization.
- Dissolve in 75 mL carbon dioxide-free water and add 2 drops of phenolphthalein.
- Titrate with NaOH until a permanent pink color is produced, indicating endpoint.
- Each mL of 0.1N NaOH equates to 204.23 mg of potassium biphthalate.
- Calculate normality using: Normality = gm/mEq x mL consumed in NaOH solution.
Assay of Sodium Bicarbonate Tablets
- Aim to determine the purity or % label claim of sodium bicarbonate in tablets via direct titration.
- Specification requires sodium bicarbonate tablets to contain 95.0% to 105.0% NaHCO3.
- Use formula for computation:
- % Assay = (mL x N HCl x 84.01/1000) / Weight of Sample (grams) × 100.
Standardization of 0.1N Sulfuric Acid Solution
- Run out 20 mL of 0.1N sodium hydroxide solution into a clean Erlenmeyer flask.
- Add 2 drops of methyl orange and titrate with sulfuric acid until a color change occurs from yellow to orange.
- Calculate normality of sulfuric acid after completing three trials.
Overview of Sulfuric Acid
- Sulfuric acid is diprotic with a 1N solution containing 49.04 g H2SO4.
- Approximately 49.0 mL of concentrated sulfuric acid is required to prepare 1000 mL of solution.
- Alkalimetry occurs when a strong acid is titrated with a strong base, resulting in a neutral pH of 7.0 at the endpoint.
- The standardization of sulfuric acid can use phenolphthalein as an indicator to observe endpoint.
Important Terms
- Titrant: The substance in the burette used for titration.
- Analyte: The titrand, typically a pure substance being analyzed.
- Indicator: A chemical that changes color to signify the endpoint of a reaction.
- Endpoint: The stage indicating reaction completion via color change.
- Equivalence Point: Point in titration where the amount of titrant is stoichiometrically equivalent to the analyte.
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