Sodium hydroxide easily absorb water and carbon dioxide.
It is necessary to standardize a solution of NaOH using a primary standard like KHP because primary standards are highly pure and have a known exact mass. This allows for accurate and precise determination of the concentration of the NaOH solution, ensuring reliable and consistent results in experiments.
Yes, it is possible to prepare a standard NaOH solution by dissolving an accurate amount of NaOH pellets in a known volume of water. This process allows for the calculation of the concentration of the NaOH solution based on the amount of NaOH used and the volume of water.
Because NaOH is hygroscopic, meaning it absorbs water from the air, NaOH cannot be accurately weighed. To standardize 0.1 M NaOH, a solution is made to an approximate concentration of 0.1 M and then standardized by titrating an accurately weighed quantity of a primary standard.
The reasons KHP is used as a primary standard are as follows: (1) It is not hydroscopic, (2) it has a high molecular weight, so a reasonable amount to titrate can be easily weighed, and (3) it is stable at temperatures over 100°C so that any water may be driven off by heating.
To standardize 0.02 N NaOH, you would titrate it against a known concentration of an acid, such as a primary standard like potassium hydrogen phthalate. By carefully adding the NaOH to the acid until the endpoint is reached, you can determine the exact concentration of the NaOH solution.
NaOH
It is necessary to standardize a solution of NaOH using a primary standard like KHP because primary standards are highly pure and have a known exact mass. This allows for accurate and precise determination of the concentration of the NaOH solution, ensuring reliable and consistent results in experiments.
Yes, it is possible to prepare a standard NaOH solution by dissolving an accurate amount of NaOH pellets in a known volume of water. This process allows for the calculation of the concentration of the NaOH solution based on the amount of NaOH used and the volume of water.
Because NaOH is hygroscopic, meaning it absorbs water from the air, NaOH cannot be accurately weighed. To standardize 0.1 M NaOH, a solution is made to an approximate concentration of 0.1 M and then standardized by titrating an accurately weighed quantity of a primary standard.
The reasons KHP is used as a primary standard are as follows: (1) It is not hydroscopic, (2) it has a high molecular weight, so a reasonable amount to titrate can be easily weighed, and (3) it is stable at temperatures over 100°C so that any water may be driven off by heating.
The standard concentration of NaOH is typically 1.0 M for laboratory use.
To standardize 0.02 N NaOH, you would titrate it against a known concentration of an acid, such as a primary standard like potassium hydrogen phthalate. By carefully adding the NaOH to the acid until the endpoint is reached, you can determine the exact concentration of the NaOH solution.
In titration, the standardization of NaOH solution involves determining its exact concentration by titrating it against a primary standard substance (e.g., potassium hydrogen phthalate). Citric acid cannot be used for standardizing NaOH directly due to its multiple acidic protons and lack of stability as a primary standard. Once the NaOH solution is standardized, it can be accurately used in titrations with citric acid to determine its concentration or in other analytical procedures.
Sodium hydoxide cannot be used as a primary standard because of its hygroscopic properties as a solid. Because it is so prone to absorbing water, it is impossible to accurately measure the mass of a solid sample, so instead it must be put into solution and tirated with a known acidic solution, such as HCl. This makes it a secondary standard as opposed to a primary standard. By. Kuatsienu Divine
Sodium Carbonate (Na2CO3) is most commonly used to standardise acids as it is non-hygroscopic (doesn't absorb water from the atmosphere).Oxalic Acid (HOOCCOOH or H2C2O4) used to standardise bases
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To standardize 1N HCl (hydrochloric acid), you would typically use a primary standard base, such as sodium hydroxide (NaOH), of known concentration to titrate the HCl solution. By carefully titrating the HCl with the NaOH, you can determine the exact concentration of the HCl solution. This information can then be used to adjust the concentration of the HCl solution as needed to make it accurately 1N.