If you titrate 25.00 ml of a 460 mg/L ascorbic acid solution, boil it for 15 minutes and then titrate it with 10.75 mL of 0.00135 M KIO3. What is the concentration of Vitamin C in mg/g ascorbic acid ( original) (mg/g)?
Chemistry acid and base titration. please help me to understand this question
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If you titrate 25.00 ml of a 460 mg/L ascorbic acid solution, boil it for 15 minutes and then titrate it with 10.75 mL of 0.00135 M KIO3. What is the concentration of Vitamin C in mg/g ascorbic acid ( original) (mg/g)?
An aqueous solution of Ca(OH)2with a concentration of 0.143 M was used to titrate 25.00 mL...
An aqueous solution of Ca(OH)2with a concentration of
0.143 M was used to titrate 25.00 mL of aqueous HCl. 14.73
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
How many moles of base were required to react completely with the
acid in this reaction?
How many moles of HCl were present in the original 25.00 mL of
acid?
What is the molarity of the original HCl solution?
04 Question (a points) aSee page 166 Watch the...
Acid-Base Titration: A 0.15 M solution of NaOH is used to titrate 200.0 mL of 0.15...
Acid-Base Titration: A 0.15 M solution of NaOH is used to titrate 200.0 mL of 0.15 M HCN. What is the pH at the equivalence point? Ka = 4.9 x 10-10. Please include steps/work so I can see and understand how this problem is solved.
3. In the lab you are going to titrate a weak acid solution (25.00 mL of...
3. In the lab you are going to titrate a weak acid solution (25.00 mL of 0.100 M HCHO2, formic acid) with a strong base (0.100 M NaOH). Carry out the following calculations to determine the pH for four key points throughout the titration. Part a. Calculate the volume of 0.100 M NaOH required to reach the equivalence point for the titration. Ans. 25.00 mL Part b. Calculate the initial pH of 0.100 M HCHO2 (before adding any NaOH). Ans....
An aqueous solution of Ca(OH)2with a concentration of 0.161 M was used to titrate 25.00 mL...
An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
Ascorbic Acid Concentration (g/L) Volume of DCPIP in Full Syringe Used (mL) Volume of DCPIP in...
Ascorbic Acid Concentration (g/L)
Volume of DCPIP in Full Syringe Used (mL)
Volume of DCPIP in Final Syringe (mL)
Total Volume of DCPIP Used (mL)
0.0
5 mL
4.9 mL
0.1 mL
0.50
5 mL
2 mL
3 mL
1.00
5 mL
1.2 mL
3.8 mL
1.50
5 mL
3.6 mL
6.4 mL
2.00
5 mL
2.8 mL
7.2 mL
Unknown Trial 1
5 mL
2.0 mL
3.0 mL
Unknown Trial 2
5 mL
2.2 mL
2.8 mL
Unknown Trial...
We’re going to titrate formic acid with the strong base, NaOH. There is initially 100. mL...
We’re going to titrate formic acid with the strong base, NaOH. There is initially 100. mL of 0.50 M formic acid and the concentration of NaOH is 1.0 M. What is the initial pH of the formic acid solution? 2) What is the percent ionization under initial conditions? 3) After the addition of 10 mL of NaOH, what is the pH? 4) After the addition of 25 mL of NaOH, what is the pH? Think about where in the titration...
Please help with 9-13 Beginning with your 50 mL solution of sulfuric acid, begin to titrate...
Please help with 9-13
Beginning with your 50 mL solution of sulfuric acid, begin to titrate in your 0.1 M solution of NaOH slowly. When the solution turns pink, stop and record the amount of NaOH used To begin the procedure click next 3 29mL NaOH MacBook Air 5 9 0 Question #9: Using the amount of Base used in step three, determine the concentration of the acid. Using the equations below, pick the correct option for this specific acid....
Weak acid/strong base titration question: 21.80 mL of 0.1164 M NaOH (0.00253752 mol) is added to...
Weak acid/strong base titration question: 21.80 mL of 0.1164 M NaOH (0.00253752 mol) is added to 20.00 mL of 0.127 M unknown weak acid HA (0.00254 mol). The resultant pH is 7.57. I am trying to calculate the Ka without the Henderson-Hasselbach equation but I cannot get an answer that matches my other calculated Ka values. Please help.
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...
please help l, will rate! thabk you!! Why does a solution of a weak acid and...
please help l, will rate! thabk you!!
Why does a solution of a weak acid and its conjugate base act as a better buffer than does a solution of the weak acid alone? The presence of both the acid and the base provides a significant concentration of both an acid and a base, making it harder to change the pH A solution of a weak acid alone has no base present to absorb added acid. The presence of both the...
An aqueous solution of Ca(OH)2with a concentration of
0.143 M was used to titrate 25.00 mL of aqueous HCl. 14.73
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
How many moles of base were required to react completely with the
acid in this reaction?
How many moles of HCl were present in the original 25.00 mL of
acid?
What is the molarity of the original HCl solution?
04 Question (a points) aSee page 166 Watch the...
An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
Ascorbic Acid Concentration (g/L)
Volume of DCPIP in Full Syringe Used (mL)
Volume of DCPIP in Final Syringe (mL)
Total Volume of DCPIP Used (mL)
0.0
5 mL
4.9 mL
0.1 mL
0.50
5 mL
2 mL
3 mL
1.00
5 mL
1.2 mL
3.8 mL
1.50
5 mL
3.6 mL
6.4 mL
2.00
5 mL
2.8 mL
7.2 mL
Unknown Trial 1
5 mL
2.0 mL
3.0 mL
Unknown Trial 2
5 mL
2.2 mL
2.8 mL
Unknown Trial...
Please help with 9-13
Beginning with your 50 mL solution of sulfuric acid, begin to titrate in your 0.1 M solution of NaOH slowly. When the solution turns pink, stop and record the amount of NaOH used To begin the procedure click next 3 29mL NaOH MacBook Air 5 9 0 Question #9: Using the amount of Base used in step three, determine the concentration of the acid. Using the equations below, pick the correct option for this specific acid....
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...
please help l, will rate! thabk you!!
Why does a solution of a weak acid and its conjugate base act as a better buffer than does a solution of the weak acid alone? The presence of both the acid and the base provides a significant concentration of both an acid and a base, making it harder to change the pH A solution of a weak acid alone has no base present to absorb added acid. The presence of both the...
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