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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.
What else can I help you with?
How many grams of K HP are needed to neutralize 18.64 ml of a 0.1004 M Na OH solution?
Molarity = mols of solute/L of solution .1004 = mols of NaOH/.01864 moles of NaOH = .00187 Moles of NaOH = Moles of KHP Now, multiply .00187 by the molar mass of KHP .00187*204.22 = .38 g KHP
Why do we standardize the NaOH solution that we made by dissolving a measured mass of solid NaOH?
Standardizing the NaOH solution by dissolving a measured mass of solid NaOH ensures that the concentration of the solution is accurately known and consistent for use in experiments or analyses.
How do you standardize a solution of NaOH and what reagents to be used?
If you have a standard solution of an acid, like hydrochloric or sulfuric, you can perform a titration in the presence of phenolphtalein or methyl orange and calculate the solution's normality or, you can weigh a sample of a strong solid acid ( orthoiperiodic acid or even oxalic acid), titrate the acid with the hydroxide solution, again in the presence of phenolphtalein or methyl orange and calculate the concentration of NaOH. If you want to have a solution with an exact concentration, let's say 1 molar, and the actual concentration is 1,33 molar, you simply calculate how much water you need to ad in a specific quantity of solution, to dilute it to exactly 1 molar.
How can one standardize NaOH?
To standardize NaOH, one must titrate it against a known concentration of an acid, such as HCl, using an indicator to determine the endpoint of the reaction. The volume and concentration of the NaOH can then be calculated based on the volume of acid used in the titration. This process ensures that the concentration of the NaOH solution is accurately determined for future use in experiments.
How many ml of 0.1200 M NaOH is needed to titrate 0.5100 g KHP (MW 204.22 gmol) to the phenolphthalein end point?
To begin, calculate the number of moles of KHP using its molar mass. Next, use the stoichiometry of the reaction to determine the moles of NaOH required for complete titration. Finally, use the concentration of NaOH to calculate the volume needed in milliliters using the formula: volume (mL) = moles needed / molarity.
How many grams of K HP are needed to neutralize 18.64 ml of a 0.1004 M Na OH solution?
Molarity = mols of solute/L of solution .1004 = mols of NaOH/.01864 moles of NaOH = .00187 Moles of NaOH = Moles of KHP Now, multiply .00187 by the molar mass of KHP .00187*204.22 = .38 g KHP
Why do we standardize the NaOH solution that we made by dissolving a measured mass of solid NaOH?
Standardizing the NaOH solution by dissolving a measured mass of solid NaOH ensures that the concentration of the solution is accurately known and consistent for use in experiments or analyses.
How do you standardize a solution of NaOH and what reagents to be used?
If you have a standard solution of an acid, like hydrochloric or sulfuric, you can perform a titration in the presence of phenolphtalein or methyl orange and calculate the solution's normality or, you can weigh a sample of a strong solid acid ( orthoiperiodic acid or even oxalic acid), titrate the acid with the hydroxide solution, again in the presence of phenolphtalein or methyl orange and calculate the concentration of NaOH. If you want to have a solution with an exact concentration, let's say 1 molar, and the actual concentration is 1,33 molar, you simply calculate how much water you need to ad in a specific quantity of solution, to dilute it to exactly 1 molar.
How can one standardize NaOH?
To standardize NaOH, one must titrate it against a known concentration of an acid, such as HCl, using an indicator to determine the endpoint of the reaction. The volume and concentration of the NaOH can then be calculated based on the volume of acid used in the titration. This process ensures that the concentration of the NaOH solution is accurately determined for future use in experiments.
How many ml of 0.1200 M NaOH is needed to titrate 0.5100 g KHP (MW 204.22 gmol) to the phenolphthalein end point?
To begin, calculate the number of moles of KHP using its molar mass. Next, use the stoichiometry of the reaction to determine the moles of NaOH required for complete titration. Finally, use the concentration of NaOH to calculate the volume needed in milliliters using the formula: volume (mL) = moles needed / molarity.
What can do NaOH use as primary standard?
Sodium hydroxide easily absorb water and carbon dioxide.
How do you standardization 1N hcl?
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.
How do you prepare 0.02m Naoh from 1M Naoh solution?
To prepare 0.02M NaOH from 1M NaOH solution, you will need to dilute the 1M solution. Use the formula: C1V1 = C2V2, where C1 is the concentration of the stock solution (1M), V1 is the volume of the stock solution you will use, C2 is the desired concentration (0.02M), and V2 is the final volume of the diluted solution. Calculate the volume of 1M NaOH solution (V1) needed to make the desired 0.02M concentration and dilute it with water to reach the desired volume (V2).
How do you calculate of NaOH in solution procedure?
To calculate the concentration of NaOH in a solution, you would typically measure the volume of the solution and the amount of NaOH used to prepare it. Then, you can use the formula: Concentration (in mol/L) = amount of NaOH (in mol) / volume of solution (in L) to determine the concentration. Make sure to convert any given amount of NaOH from grams to moles before calculating.
How do you prepare a 6N NaOH solution from a 10N NAOH solution?
To prepare a 6N NaOH solution from a 10N NaOH solution, you would dilute the 10N solution by adding water. Use the dilution formula: C1V1 = C2V2, where C1 is the initial concentration (10N), V1 is the volume of stock solution needed, C2 is the final concentration (6N), and V2 is the final volume of the solution you want to make. Calculate the volume of the 10N solution needed and add water to reach the final desired volume for a 6N NaOH solution.
What is the concentratuon of a hcl solution if 25.0 ml is required to neutralize 38.5 ml of a 0.500m solution of naoh?
To find the concentration of HCl, you can use the formula: moles of NaOH = moles of HCl. From the given information, you can calculate the moles of NaOH used to neutralize the acid. Then, use the volume and concentration of NaOH to determine the concentration of HCl.
Did the volume of water you used to dissolve your KHP affect the results of your standardization?
Yes, the volume of water used can affect the concentration of KHP solution, which in turn can impact the accuracy of the standardization results. It is important to use a consistent volume of water to ensure reproducibility in the experiment.
