![8. [-/19 Points] DETAILS 27.0 mL of 0.160 M HClO is titrated with 0.140 M NaOH. a) What volume of base is required to reach t](http://img.homeworklib.com/questions/930d80e0-f4e5-11eb-be55-69b40543f1b1.png?x-oss-process=image/resize,w_560)
Homework Answers
The answer is given in the attachment.
![al Vis, = V₂ S 2 z) V₂ = Visi 270mLx 0.160M² S₂ 0-140M : Volume of base = 30.86 ml [Answer] b) Here, we must we Henderson Has](http://img.homeworklib.com/questions/4648ef60-f4e6-11eb-a037-235e6d5d9b97.png?x-oss-process=image/resize,w_560)
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8. [-/19 Points] DETAILS 27.0 mL of 0.160 M HClO is titrated with 0.140 M NaOH....
At 25.0 mL sample of 0.100 M HClO (aq) is titrated with NaOH (aq). What is...
At 25.0 mL sample of 0.100 M HClO (aq) is titrated with NaOH (aq). What is the pH of the solution after the addition of 25.00 mL of 0.100 M NaOH? Ka of HClO=3.5*10^-8. The answer might be 4.70 but I don't know. Can anyone explain this problem to me? Full explanation please.
33.0 mL of 0.170 M KN3 is titrated with 0.250 M HCl. acid-base table a) What...
33.0 mL of 0.170 M KN3 is titrated with 0.250 M HCl. acid-base table a) What volume of acid is required to reach the equivalence point? volume of acid = mL b) What is the pH of the solution after addition of 11.6 mL of acid? pH = c) What is the pH of the solution after addition of 24.2 mL of acid? pH = d) What is the pH at the equivalence point? pH =
A 50.0-mL sample of 0.15 M butanoic acid, CH3CH2CH2COOH, is titrated with 0.30 M NaOH(aq). Ka...
A 50.0-mL sample of 0.15 M butanoic acid, CH3CH2CH2COOH, is titrated with 0.30 M NaOH(aq). Ka for butanoic acid is 1.52 x 10-5 a) How many mL of NaOH(aq) are required to reach the equivalence point? b)What is the pH of the solution after 27.0 mL of NaOH(aq) have been added?
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH....
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
45.00 mL of a 0.250 M H2SO4 solution is titrated with 0.100 M NaOH. a. What...
45.00 mL of a 0.250 M H2SO4 solution is titrated with 0.100 M NaOH. a. What is the chemical equation that describes this neutralization reaction? b. What is the volume in mL of NaOH required to reach the equivalence point? c. At the equivalence point, what are the sodium and sulfate ion concentrations? d. At the equivalence point, what are the pH and pOH
Calculate the pH for each case in the titration of 50.0 mL of 0.140 M HClO(aq)...
Calculate the pH for each case in the titration of 50.0 mL of 0.140 M HClO(aq) with 0.140 M KOH(aq). Use the ionization constant for HClO. What is the pH before addition of any KOH? pH= What is the pH after addition of 25.0 mL KOH? pH= What is the pH after addition of 40.0 mL KOH? pH= What is the pH after addition of 50.0 mL KOH? pH= What is the pH after addition of 60.0 mL KOH? pH=...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30 M NaOH(aq) (adding NaOH...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30 M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base. K of CH3CH2COOH is 1.3 x 10-5 Henderson-Hasselbalch equation: pH =pK+ log NaOH CH3CH2COOH Parta): 1) After adding 18.0 mL of the NaOH solution, the mixture is before the equivalence point on the titration curve. 2) The pH...
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl...
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl to its equivalence point. A 25.0 mL solution of a 0.200 M solution of the salt was titrated. The pK, for the unknown conjugate acid is 4.31. (a) Will the equivalence point be acidic or basic for this titration? i.e. pH less than 7.0 or greater than 7.0? (b) What is the volume in mL needed of HCl to reach the equivalence point? (c)...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30 M NaOH(aq) (adding NaOH...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30 M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base. K of CH3CH2COOH is 1.3 x 10-5. base Henderson-Hasselbalch equation: pH = pK+ log NaOH CH3CH2COOH Parta): 1) After adding 18.0 mL of the NaOH solution, the mixture is (Select) equivalence point on the titration curve. 2) The...
Calculate the pH for each case in the titration of 50.0 mL of 0.160 M HClO(aq) with 0.160 M KOH(aq). ionization constant...
Calculate the pH for each case in the titration of 50.0 mL of
0.160 M HClO(aq) with 0.160 M KOH(aq).
ionization
constant=4.0×10^–8
What is the pH before addition of any KOH? pH = What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 40.0 mL KOH? pH = What is the pH after addition of 50.0 mL KOH? pH = What is the pH after addition of 60.0 mL KOH? pH...
33.0 mL of 0.170 M KN3 is titrated with 0.250 M HCl. acid-base table a) What volume of acid is required to reach the equivalence point? volume of acid = mL b) What is the pH of the solution after addition of 11.6 mL of acid? pH = c) What is the pH of the solution after addition of 24.2 mL of acid? pH = d) What is the pH at the equivalence point? pH =
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30 M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base. K of CH3CH2COOH is 1.3 x 10-5 Henderson-Hasselbalch equation: pH =pK+ log NaOH CH3CH2COOH Parta): 1) After adding 18.0 mL of the NaOH solution, the mixture is before the equivalence point on the titration curve. 2) The pH...
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl to its equivalence point. A 25.0 mL solution of a 0.200 M solution of the salt was titrated. The pK, for the unknown conjugate acid is 4.31. (a) Will the equivalence point be acidic or basic for this titration? i.e. pH less than 7.0 or greater than 7.0? (b) What is the volume in mL needed of HCl to reach the equivalence point? (c)...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30 M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base. K of CH3CH2COOH is 1.3 x 10-5. base Henderson-Hasselbalch equation: pH = pK+ log NaOH CH3CH2COOH Parta): 1) After adding 18.0 mL of the NaOH solution, the mixture is (Select) equivalence point on the titration curve. 2) The...
Calculate the pH for each case in the titration of 50.0 mL of
0.160 M HClO(aq) with 0.160 M KOH(aq).
ionization
constant=4.0×10^–8
What is the pH before addition of any KOH? pH = What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 40.0 mL KOH? pH = What is the pH after addition of 50.0 mL KOH? pH = What is the pH after addition of 60.0 mL KOH? pH...
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