Hi, I need help with this question, I'm struggling to find the pH and the two equivalence points. thank you!
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Hi, I need help with this question, I'm struggling to find the
pH and the two...
Hi, I need help with this question, thank you! A 10.00mL sample of 0.1000M an acid...
Hi,
I need help with this question, thank you!
A 10.00mL sample of 0.1000M an acid (pKg) = 2.89; PK 2 = 5.51) was titated with 0.1526M NaOH. Sketch the graph of pH versus Vook for the titration of this acid through the addition of 25.00mL of NaOH. (3 points) Indicate the numerical pH values for the initial (i.e. before addition of NaOH), half-equivalence, and equivalence points; as well as the pH once the full 25.00ml NaOH has been added....
I'm not sure how to solve this! Any help is appreciated! 1.Draw the pH titration curve...
I'm not sure how to solve this! Any help is
appreciated!
1.Draw the pH titration curve for the titration of 35 mL of 0.150 M acetic acid with 0.200 m Include the pH values and NaOH volume requested below on your pH titration curve. Al curve the species that dictates the pH at the requested pH values. For acetic acid, Ka = 1.885 in your pH titration curve. Also, put on the 1) the initial pH 2) the pH after...
1.Determine the pH during the titration of 36.6 mL of 0.304 M ethylamine (C2H5NH2 , Kb...
1.Determine the pH during the titration of 36.6 mL of 0.304 M ethylamine (C2H5NH2 , Kb = 4.3×10-4) by 0.304 M HI at the following points. (a) Before the addition of any HI (b) After the addition of 16.1 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 51.2 mL of HI b.Determine the pH during the titration of 61.4 mL of 0.450 M nitrous acid (Ka = 4.5×10-4) by 0.450 M NaOH...
Question 2 (20pts): A 20 mL sample of 0.01 M propionic acid (CHsCH2COOH; Pk 4.87) is titrated with 0.05 M NaOH A) W...
Question 2 (20pts): A 20 mL sample of 0.01 M propionic acid (CHsCH2COOH; Pk 4.87) is titrated with 0.05 M NaOH A) Write out the chemical reaction for this titration. B) Calculate the initial pH of the sample. C) Calculate the volume of NaOH required to reach the equivalence point. D) Calculate the pH of the solution at the equivalence point. E) Sketch a titration curve for this titration (pH versus volume NaOH added). Note the Jocation of the equivalence...
Question 3: Draw the titration curve (pH versus mL of NaOH added) that would be obtained...
Question 3: Draw the titration curve (pH versus mL of NaOH added) that would be obtained from the titration of 30 mL of a 0.10 M solution of an unknown triprotic acid, H3A (Kat = 1.26 x 10-3; Ka2 = 5.6 x 10-6, Ka3 = 3.32 x 10-10) with 0.10 M NaOH. Indicate the volume needed to reach the first second, and third equivalence points and the pH at the half equivalence points for the three titration regions.
I need help with questions 1-4 please. have not yet gone over pH in lecture yet,...
I need help with questions 1-4 please. have not yet
gone over pH in lecture yet, so I'm a little lost.
Thanks
1. Why is not the pH at the equivalence point always equal to 7 in a neutralization titration? When would it be 7? (Hint: consider the strengths of the acids and bases) 2. What is the pH of the solution obtained by mixing 50.00 mL of 0.250M HCl and 50.00 mL of 0.500M NaOH? 3. What is the...
Titration of 100.00mL of a 0.1000M solution of a strong acid HCl with 0.100M NaOH solution. Determine the pH at the fol...
Titration of 100.00mL of a 0.1000M solution of a strong acid HCl with 0.100M NaOH solution. Determine the pH at the following points and sketch curve a) before addition of NaOH c) after addition of 20.0 ml NaOH e) after addition of 50.Oml NaOH e) after addition of 100 ml NaOH b) after addition of 10.0mL. NaOH d) after addition of 30.0 ml NaOH f) after addition of 80.Oml NaOH h) after addition of 110 ml NaOH Titration of 100...
I'm not sure about how I'm supposed to find NaOH concentration from a strong acid and...
I'm not sure about how I'm supposed to find NaOH
concentration from a strong acid and strong base titration. I'm
thinking that 2.5×10^-8 mol per L that I calculated would make the
moles of NaOH 2.5x10^-8 mol since it's a one to one
ratio.
Hydrochloric acid titration: Confirming the concentration of NaOH Concentration of HCl solution from the stock bottle: _ 0.OSM! Initial pH of HCl solution: 1.66 pH Volume NaOH (mL) Concentration of NaOH (M) Non Phenolphthalein (end point)...
Titration curve for a weak acid l pH-pK, + log(İHAİ IA I 3. After class practice:...
Titration curve for a weak acid l pH-pK, + log(İHAİ IA I 3. After class practice: calculate the pH of 25.0 mL of 0.100 M formic acid solution (HCOOH: pK 3.74) after you add: iet Show calcuktions A. 10.0 mL NaOH added B. 12.5 mL NaOH added C. 15.0 mL NaOH added D. 20.0 mL NaOH added Half-equivalence point (pH pKa) 14 12 10- mol CHO2 0.00100 Volume (mL) 10.0 12.5 15.0 20.0 mol HCHO2 0.00150 0.00125 0.00100 0.00050 pH...
Hi, I need help with this question, thanks! What is the molarity of the initial HCl...
Hi, I need help with this question, thanks!
What is the molarity of the initial HCl solution of 45.78 mL
of 0.50 M HCl after adding 30.3 mL of deionized water?
A student was conducting a titration experiment and was asked to calculate the theoretical pH of the solution at various points in the titration curve. In this experiment, the student added 45.78 ml of a 0.50 M solution of HCI to a 200 ml beaker. The student then added...
Hi,
I need help with this question, thank you!
A 10.00mL sample of 0.1000M an acid (pKg) = 2.89; PK 2 = 5.51) was titated with 0.1526M NaOH. Sketch the graph of pH versus Vook for the titration of this acid through the addition of 25.00mL of NaOH. (3 points) Indicate the numerical pH values for the initial (i.e. before addition of NaOH), half-equivalence, and equivalence points; as well as the pH once the full 25.00ml NaOH has been added....
I'm not sure how to solve this! Any help is
appreciated!
1.Draw the pH titration curve for the titration of 35 mL of 0.150 M acetic acid with 0.200 m Include the pH values and NaOH volume requested below on your pH titration curve. Al curve the species that dictates the pH at the requested pH values. For acetic acid, Ka = 1.885 in your pH titration curve. Also, put on the 1) the initial pH 2) the pH after...
Question 2 (20pts): A 20 mL sample of 0.01 M propionic acid (CHsCH2COOH; Pk 4.87) is titrated with 0.05 M NaOH A) Write out the chemical reaction for this titration. B) Calculate the initial pH of the sample. C) Calculate the volume of NaOH required to reach the equivalence point. D) Calculate the pH of the solution at the equivalence point. E) Sketch a titration curve for this titration (pH versus volume NaOH added). Note the Jocation of the equivalence...
Question 3: Draw the titration curve (pH versus mL of NaOH added) that would be obtained from the titration of 30 mL of a 0.10 M solution of an unknown triprotic acid, H3A (Kat = 1.26 x 10-3; Ka2 = 5.6 x 10-6, Ka3 = 3.32 x 10-10) with 0.10 M NaOH. Indicate the volume needed to reach the first second, and third equivalence points and the pH at the half equivalence points for the three titration regions.
I need help with questions 1-4 please. have not yet
gone over pH in lecture yet, so I'm a little lost.
Thanks
1. Why is not the pH at the equivalence point always equal to 7 in a neutralization titration? When would it be 7? (Hint: consider the strengths of the acids and bases) 2. What is the pH of the solution obtained by mixing 50.00 mL of 0.250M HCl and 50.00 mL of 0.500M NaOH? 3. What is the...
Titration of 100.00mL of a 0.1000M solution of a strong acid HCl with 0.100M NaOH solution. Determine the pH at the following points and sketch curve a) before addition of NaOH c) after addition of 20.0 ml NaOH e) after addition of 50.Oml NaOH e) after addition of 100 ml NaOH b) after addition of 10.0mL. NaOH d) after addition of 30.0 ml NaOH f) after addition of 80.Oml NaOH h) after addition of 110 ml NaOH Titration of 100...
I'm not sure about how I'm supposed to find NaOH
concentration from a strong acid and strong base titration. I'm
thinking that 2.5×10^-8 mol per L that I calculated would make the
moles of NaOH 2.5x10^-8 mol since it's a one to one
ratio.
Hydrochloric acid titration: Confirming the concentration of NaOH Concentration of HCl solution from the stock bottle: _ 0.OSM! Initial pH of HCl solution: 1.66 pH Volume NaOH (mL) Concentration of NaOH (M) Non Phenolphthalein (end point)...
Titration curve for a weak acid l pH-pK, + log(İHAİ IA I 3. After class practice: calculate the pH of 25.0 mL of 0.100 M formic acid solution (HCOOH: pK 3.74) after you add: iet Show calcuktions A. 10.0 mL NaOH added B. 12.5 mL NaOH added C. 15.0 mL NaOH added D. 20.0 mL NaOH added Half-equivalence point (pH pKa) 14 12 10- mol CHO2 0.00100 Volume (mL) 10.0 12.5 15.0 20.0 mol HCHO2 0.00150 0.00125 0.00100 0.00050 pH...
Hi, I need help with this question, thanks!
What is the molarity of the initial HCl solution of 45.78 mL
of 0.50 M HCl after adding 30.3 mL of deionized water?
A student was conducting a titration experiment and was asked to calculate the theoretical pH of the solution at various points in the titration curve. In this experiment, the student added 45.78 ml of a 0.50 M solution of HCI to a 200 ml beaker. The student then added...
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