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acid solution What is the concen 4. You are titrating an acid into a base to...
2. You are titrating an acid into a base to determine the concentration of the base....
2. You are titrating an acid into a base to determine the concentration of the base. The endpoint of the neutralization is reached but the stopcock on the buret sticks slightly and allows a few more drops of acid to fall into the solution. How will this affect your calculations for the concentration of the base?
A student carefully pipets 25.0 mL of 0.525 M NaOH into a test tube. She places...
A student carefully pipets 25.0 mL of 0.525 M NaOH into a test tube. She places the test tube into a small beaker to keep it from spilling and then pipets 75.0 mL of 0.355 M HC 5. into another test tube. When she reaches to put this test tube of acid into the beaker along with test tube of base she accidentally knocks the test tubes together hard enough to break them and their respective contents combine in the...
9. You titrate an acid into a base to determine the concentration of the base. The endpoint of the neutralization is rea...
9. You titrate an acid into a base to determine the concentration of the base. The endpoint of the neutralization is reached but the stopcock on the buret sticks slightly and allows a few more drops of acid to fall into the solution. How will this affect your calcs for the concentration of the base? Be specific. (2-4 sentences) 10. A few small drops of water are left in a buret that is then used to titrate a base into...
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2....
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
3. If 15.0 mL of 0.125 M phosphoric acid is titrated with 0.100 M NaOH, what...
3. If 15.0 mL of 0.125 M phosphoric acid is titrated with 0.100 M NaOH, what volume of the titrant (in mL) must be added to completely neutralize the acid? Show all of your work (including the chemical equation). (1 point) Post-lab Questions: Experiment #9: Acid-Base Titrations Student Learning Objectives : Students will gain practice with the accurate preparation of solutions. Students will perform acid-base titrations and prepare titration curves. Students will identify strong and weak acids by the shapes...
Question 4 Status: Not yet answered | Points possible: 1.00 Suppose you are titrating an acid...
Question 4 Status: Not yet answered | Points possible: 1.00 Suppose you are titrating an acid of unknown concentration with a standardized base. At the beginning of the titration, you read the base titrant volume as 2.86 mL. After running the titration and reaching the endpoint, you read the base titrant volume as 21.17 mL. What volume, in mL, of base was required for the titration? Type answer: Question 6 Status: Not yet answered Points possible: 1.00 Suppose you are...
You standardize your NaOH solution by titrating a known quantity of sulfamic acid (H2NSO3H) standard. It...
You standardize your NaOH solution by titrating a known quantity of sulfamic acid (H2NSO3H) standard. It requires 36 mL of the solution to reach the endpoint with 0.2913 g of sulfamic acid. What is the concentration of your NaOH solution? I got 0.08333, but it is wrong.
please help with my pre lab additional information Pre-Lab Questions: 1. What is the definition of...
please help with my pre lab
additional information
Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
During a titration of a weak base with a strong acid, you are slowing converting molecules...
During a titration of a weak base with a strong acid, you are slowing converting molecules of the weak base into molecules of its conjugate acid. For the hypothetical weak base, B we see the following: B (aq) + H30+ (aq) - BH+ (aq) + H20 (1) In the problem below you will be adding some strong acid, but not enough to reach the endpoint of the titration. 2.00 mL of hydrochloric acid added to the weak base 2.00M hydrochloric...
Part A You are given a solution of HCOOH (formic acid) with an approximate concentration of...
Part A You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1105 M NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the end point? You are given a solution of (formic acid) with an approximate concentration of 0.20 and you will titrate this with a 0.1105 . If you add 20.00 of to the beaker before...
2. You are titrating an acid into a base to determine the concentration of the base. The endpoint of the neutralization is reached but the stopcock on the buret sticks slightly and allows a few more drops of acid to fall into the solution. How will this affect your calculations for the concentration of the base?
A student carefully pipets 25.0 mL of 0.525 M NaOH into a test tube. She places the test tube into a small beaker to keep it from spilling and then pipets 75.0 mL of 0.355 M HC 5. into another test tube. When she reaches to put this test tube of acid into the beaker along with test tube of base she accidentally knocks the test tubes together hard enough to break them and their respective contents combine in the...
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
3. If 15.0 mL of 0.125 M phosphoric acid is titrated with 0.100 M NaOH, what volume of the titrant (in mL) must be added to completely neutralize the acid? Show all of your work (including the chemical equation). (1 point) Post-lab Questions: Experiment #9: Acid-Base Titrations Student Learning Objectives : Students will gain practice with the accurate preparation of solutions. Students will perform acid-base titrations and prepare titration curves. Students will identify strong and weak acids by the shapes...
Question 4 Status: Not yet answered | Points possible: 1.00 Suppose you are titrating an acid of unknown concentration with a standardized base. At the beginning of the titration, you read the base titrant volume as 2.86 mL. After running the titration and reaching the endpoint, you read the base titrant volume as 21.17 mL. What volume, in mL, of base was required for the titration? Type answer: Question 6 Status: Not yet answered Points possible: 1.00 Suppose you are...
please help with my pre lab
additional information
Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
During a titration of a weak base with a strong acid, you are slowing converting molecules of the weak base into molecules of its conjugate acid. For the hypothetical weak base, B we see the following: B (aq) + H30+ (aq) - BH+ (aq) + H20 (1) In the problem below you will be adding some strong acid, but not enough to reach the endpoint of the titration. 2.00 mL of hydrochloric acid added to the weak base 2.00M hydrochloric...
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