Homework Answers
By doing this mistake he has delivered some more amount of NaOH than required for neutralisation.
When he would calculate the Molarity of NaOH by applying concentration equation , then he will consider this extra volume and thus the Molarity of NaOH will come out to be less than the actual molarity .
As molarity of NaOH will =(molarity of acid × volume of acid) ÷ volume of NaOH .
As volume of NaOH is more , so molarity will be less .
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1) A student overshot the end point of their titration, resulting in a dark pink solution...
1. A student prepared a base solution using 7 mL of 6M NaOH diluted with distilled...
1. A student prepared a base solution using 7 mL of 6M NaOH diluted with distilled water to a final volume of approximately 400 ml. The student titrated a standardized solution of HCI to determine the exact concentration of the prepared base solution. In the first titration she found that it took 22.47 mL of the base solution to neutralize 20.00 mL of a 0.98861 M HCl solution. In the second titration, she found that it took 20.12 mL of...
1. While titrating, a student added 50 mL of NaOH solution without ever seeing a color...
1. While titrating, a student added 50 mL of NaOH solution without ever seeing a color change. Suggest at least two pos sible reasons that this might occur. 2. A student completed two trials of titration with a very faint pink color, and one that was a very bright, intense pink color. What should the student do at that point? 3. A student asserts that the AG calculated from K is not AG n since the reaction did not take...
LABORATORY 8 Post-Lab 1. Explain how each of the following errors would have altered your results....
LABORATORY 8 Post-Lab 1. Explain how each of the following errors would have altered your results. Clearly explain why your calculated answer would be high, low, or unchanged. (A single word answer is not acceptable.) a. You decided to take the pH after each addition of 5.0 mL of NaOH rather than after every 0.5 mL during the neutralization of your acid sample. b. While using the Half Volume method, your solution was dark pink (you overshot the endpoint) and...
Questions 1. Why do you want to stop the titration of want to stop the titration...
Questions 1. Why do you want to stop the titration of want to stop the titration of the solution at the lightest pink color you can detect? Because it's the equvilant point 2. How would this experiment change if the HCI was the standard solution and NaOH was the unknown? 3. What is the proper way to dilute acids with water? water then acid 4. In this experiment, you diluted the HCI given to you and then titrated the samples....
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...
2 why is it important to keep the NAOH solution covered at all times? 0 How...
2 why is it important to keep the NAOH solution covered at all times? 0 How will the molarity of the NaOH solution be affected by its continued exposure to the atmosphere? 3. The pale pink color of the titration solution at the end point will fade to colorless after several minutes when exposed to the atmosphere. Account for this color change 4. What volume (in mL) of 0.0293 M Ba(OH)2 is required to neutralize 25.00 mL of 0.200 M...
please answer all the parts Supplemental Questions - Titration Lab, 1. Indicate how each of the...
please answer all the parts
Supplemental Questions - Titration Lab, 1. Indicate how each of the following would affect the values of K, for the weak acid unknown and for the dibasic salt and the value of the molar mass for the dibasic salt (Would the determined values be higher or lower than the actual values?). Use larger, smaller or no change. And as always....Explain. a. The titrant (either the NaOH or the HCI) molarity is actually HIGHER than that...
2) In preparing the KHP solution, a student did find a 100 ml volumetric flask and instead used a 200 mL size to di...
2) In preparing the KHP solution, a student did find a 100 ml volumetric flask and instead used a 200 mL size to dissolve the same weight of solid to be dissolved in 100 mL solution. In comparison to preparing a 100 mL solution as described in the procedure, explain how the student's action will affect (if any): a) The number of moles of KHP in a 25.00 mL aliquot of the solution. b) The equivalence point of the titration?...
Determine how many liters (l) of stock HCl were used in titration #1. Please fill all...
Determine how many liters (l) of stock HCl were used
in titration #1.
Please fill all questions under "Data Analysis"
Page 1 is just instruction for Page 2
EXPT 10: TITRATION OF STRONG ACID WITH STRONG BASE Note to Students: when you see the symbol (), this means there is something you must add into the mock data yourself. You may handwrite or type your answers directly on these pages for submission to a Blackboard link. Remember to show all...
In the titration of 50.00 mL of 1.00 M HC2H3O2 with 1.00 M NaOH, a student...
In the titration of 50.00 mL of 1.00 M HC2H3O2 with 1.00 M NaOH, a student was considering using bromcresol as an indicator. Ka HC2H3O2 = 1.8 x 10-5 Kb for C2H3O2-1 = 5.6 x 10-10 (1)How many milliliters of NaOH would it take to reach the endpoint with this titration? (2)What is the pH of the solution at the end point? (2)What indicator would be a better choice than bromcresol green for this titration?
1. A student prepared a base solution using 7 mL of 6M NaOH diluted with distilled water to a final volume of approximately 400 ml. The student titrated a standardized solution of HCI to determine the exact concentration of the prepared base solution. In the first titration she found that it took 22.47 mL of the base solution to neutralize 20.00 mL of a 0.98861 M HCl solution. In the second titration, she found that it took 20.12 mL of...
1. While titrating, a student added 50 mL of NaOH solution without ever seeing a color change. Suggest at least two pos sible reasons that this might occur. 2. A student completed two trials of titration with a very faint pink color, and one that was a very bright, intense pink color. What should the student do at that point? 3. A student asserts that the AG calculated from K is not AG n since the reaction did not take...
LABORATORY 8 Post-Lab 1. Explain how each of the following errors would have altered your results. Clearly explain why your calculated answer would be high, low, or unchanged. (A single word answer is not acceptable.) a. You decided to take the pH after each addition of 5.0 mL of NaOH rather than after every 0.5 mL during the neutralization of your acid sample. b. While using the Half Volume method, your solution was dark pink (you overshot the endpoint) and...
Questions 1. Why do you want to stop the titration of want to stop the titration of the solution at the lightest pink color you can detect? Because it's the equvilant point 2. How would this experiment change if the HCI was the standard solution and NaOH was the unknown? 3. What is the proper way to dilute acids with water? water then acid 4. In this experiment, you diluted the HCI given to you and then titrated the samples....
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...
2 why is it important to keep the NAOH solution covered at all times? 0 How will the molarity of the NaOH solution be affected by its continued exposure to the atmosphere? 3. The pale pink color of the titration solution at the end point will fade to colorless after several minutes when exposed to the atmosphere. Account for this color change 4. What volume (in mL) of 0.0293 M Ba(OH)2 is required to neutralize 25.00 mL of 0.200 M...
please answer all the parts
Supplemental Questions - Titration Lab, 1. Indicate how each of the following would affect the values of K, for the weak acid unknown and for the dibasic salt and the value of the molar mass for the dibasic salt (Would the determined values be higher or lower than the actual values?). Use larger, smaller or no change. And as always....Explain. a. The titrant (either the NaOH or the HCI) molarity is actually HIGHER than that...
2) In preparing the KHP solution, a student did find a 100 ml volumetric flask and instead used a 200 mL size to dissolve the same weight of solid to be dissolved in 100 mL solution. In comparison to preparing a 100 mL solution as described in the procedure, explain how the student's action will affect (if any): a) The number of moles of KHP in a 25.00 mL aliquot of the solution. b) The equivalence point of the titration?...
Determine how many liters (l) of stock HCl were used
in titration #1.
Please fill all questions under "Data Analysis"
Page 1 is just instruction for Page 2
EXPT 10: TITRATION OF STRONG ACID WITH STRONG BASE Note to Students: when you see the symbol (), this means there is something you must add into the mock data yourself. You may handwrite or type your answers directly on these pages for submission to a Blackboard link. Remember to show all...
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