if the endpoint for the titration of an aspirin sample with NaOH titrant is surpassed, will...
if the endpoint for the titration of an aspirin sample with NaOH titrant is surpassed, will the percent purity of the aspirin sample be reported too high or too low? Please explain. i believe %purity=(calculated weight/given weight) x100 but idk how that will change the %purity
Homework Answers
Since aspirin is acidic in nature and on it's titration with NaOH... If the endpoint is surpassed, it means more acid is available there to be neutralised by NaOH.
more acid means purer aspirin sample and hence the product quantity will also increase leading to the increase in %purity via calculations.
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if the endpoint for the titration of an aspirin sample with NaOH
titrant is surpassed, will...
i need all answers Data Table 1: Titration of Vinegar with Sodium Hydroxide Vinegar Sample 1...
i
need all answers
Data Table 1: Titration of Vinegar with Sodium Hydroxide Vinegar Sample 1 Vinegar Sample 2 Vinegar Sample 3 Mass of Vinegar (6) Volume of Vinegar (ml) Density - 1.005 g/ml Initial NaOH volume in syringe (ml) Final NaOH volume in syringe (ml) Volume of NaOH delivered (mL) Volume of NaOH delivered (L) Molarity of NaOH Moles of NaOH delivered Reaction of NaOH with Acetic Acid Moles of Acetic Acid in vinegar sample Molar mass of Acetic...
9. In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin...
9. In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin and the excess was then back titrated with HCl. Suppose a 0.4567 g sample of aspirin was reacted with 18.12 ml/of 0.1345 M NaOH and back titrated with 12.15 mL of 0.1124 M HCl to reach the endpoint. Calculate the weight percent of aspirin (Asp) in the sample. 8.457% 37.90% 21.14% 42.28% none of the above
In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin and...
In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin and the excess was then back titrated with HCl. Suppose a 0.4567 g sample of aspirin was reacted with 18.12 mL of 0.1345 M NaOH and back titrated with 12.15 mL of 0.1124 M HCl to reach the endpoint. Calculate the weight of aspirin (Asp) in the sample.
4. As a result of adding the NaOH titrant too rapidly and an unwillingness to allow...
4. As a result of adding the NaOH titrant too rapidly and an unwillingness to allow the pH meter to equilibrate before reading its pH, the stoichiometric point is ill defined. As a result of this technique error a. Will the K, of the weak acid be reported as too high or too low? Explain! b. Will the pka of the weak acid be reported as too high or too low? Explain!
For a titration experiment: I am using 1.025 M of NaOH(aq) as my titrant. My titration...
For a titration experiment: I am using 1.025 M of NaOH(aq) as my titrant. My titration solution is 4.0 g of potassium hydrogen tartrate, with 300 mL of distilled water. After 4 trials, my average NaOH used was 1.680 mL. I am having problems figuring out how to calculate my findings. Each trial started with 50 mL of potassium hydrogen tartrate solution, and 2 drops of phenophthalein. Then I added 1.680 mL of NaOH (on average) to get titration to...
1. If the undissolved KHT is not filtered out before the titration with NaOH, will the...
1. If the undissolved KHT is not filtered out before the titration with NaOH, will the calculated value of Ksp be too high, too low, or unaffected? Briefly explain. If the buret is rinsed with distilled water but not conditioned with NaOH, will the 2. calculated value of Ksp be too high, too low, or unaffected? Briefly explain.
Standardization of NaOH solution experiment: A 0.75 g sample of pure acid KHP was titrated to...
Standardization of NaOH solution experiment: A 0.75 g sample of pure acid KHP was titrated to phenolphthalein endpoint using 45.34 ml NaOH of unknown concentration. The formula weight of pure KHP is 204.22g/mol. Write the chemical equation for the neutralization reaction, indicate the color change of the indicator at the endpoint, and calculate molarity of the NaOH solution. Show your work. 1. Chemical equation ------------- 2. Endpoint color change ---- 3. NaOH molarity --------- Determine percent purity of impure KHP...
A student determines that 37.2mL of 0.1543 M NaOH is required to titrate 25.0mL HCl. What...
A student determines that 37.2mL of 0.1543 M NaOH is required to titrate 25.0mL HCl. What is the concentration of the acid? The student consistently titrates to a dark pink endpoint. Will the reported value for the concentration of acid be too high, too low, or unaffected by the dark pink endpoint? Another student performs the titration and does not notice the air bubbles trapped in the tip of the buret. How will the reported value for the concentration of...
1. How is the molar solubility of a slightly soluble salt affected by the addition of an ion common to the salt equili...
1. How is the molar solubility of a slightly soluble salt affected by the addition of an ion common to the salt equilibrium? 2. A 3.11 mL volume of a standardized 0.0025 M HCl solution titrated 25.0 mL of a saturated Mg(OH)2 solution to the methyl orange endpoint. Calculate the Ksp of Mg(OH)2. 3. If the endpoint in the titration of a saturated Ca(OH)2 solution with a standardized HCI solution is surpassed, will the reported Kap of Ca(OH)2 be reported...
I'm determining the % Purity of KHP in an unknown sample. I have done two titrations:...
I'm determining the % Purity of KHP in an unknown sample. I have done two titrations: one with pure KHP titrated against a NaOH 0.1M solution, and the other is an unknown purity of KHP also titrated against a NaOH 0.1M solution. I am having trouble finding the percent purity of KHP, my professor said to recalculate my results because mine were too high (47.5%). Please help!!! Unknown Titration Trial Weight Initial Volume (mL) Final Volume (mL) 1 1.2030 1.37...
i
need all answers
Data Table 1: Titration of Vinegar with Sodium Hydroxide Vinegar Sample 1 Vinegar Sample 2 Vinegar Sample 3 Mass of Vinegar (6) Volume of Vinegar (ml) Density - 1.005 g/ml Initial NaOH volume in syringe (ml) Final NaOH volume in syringe (ml) Volume of NaOH delivered (mL) Volume of NaOH delivered (L) Molarity of NaOH Moles of NaOH delivered Reaction of NaOH with Acetic Acid Moles of Acetic Acid in vinegar sample Molar mass of Acetic...
9. In the back titration of aspirin, an excess amount of NaOH was reacted with aspirin and the excess was then back titrated with HCl. Suppose a 0.4567 g sample of aspirin was reacted with 18.12 ml/of 0.1345 M NaOH and back titrated with 12.15 mL of 0.1124 M HCl to reach the endpoint. Calculate the weight percent of aspirin (Asp) in the sample. 8.457% 37.90% 21.14% 42.28% none of the above
4. As a result of adding the NaOH titrant too rapidly and an unwillingness to allow the pH meter to equilibrate before reading its pH, the stoichiometric point is ill defined. As a result of this technique error a. Will the K, of the weak acid be reported as too high or too low? Explain! b. Will the pka of the weak acid be reported as too high or too low? Explain!
1. If the undissolved KHT is not filtered out before the titration with NaOH, will the calculated value of Ksp be too high, too low, or unaffected? Briefly explain. If the buret is rinsed with distilled water but not conditioned with NaOH, will the 2. calculated value of Ksp be too high, too low, or unaffected? Briefly explain.
Standardization of NaOH solution experiment: A 0.75 g sample of pure acid KHP was titrated to phenolphthalein endpoint using 45.34 ml NaOH of unknown concentration. The formula weight of pure KHP is 204.22g/mol. Write the chemical equation for the neutralization reaction, indicate the color change of the indicator at the endpoint, and calculate molarity of the NaOH solution. Show your work. 1. Chemical equation ------------- 2. Endpoint color change ---- 3. NaOH molarity --------- Determine percent purity of impure KHP...
1. How is the molar solubility of a slightly soluble salt affected by the addition of an ion common to the salt equilibrium? 2. A 3.11 mL volume of a standardized 0.0025 M HCl solution titrated 25.0 mL of a saturated Mg(OH)2 solution to the methyl orange endpoint. Calculate the Ksp of Mg(OH)2. 3. If the endpoint in the titration of a saturated Ca(OH)2 solution with a standardized HCI solution is surpassed, will the reported Kap of Ca(OH)2 be reported...
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