Which statement is wrong regarding the two titration curves (A) and (B) shown below? 12 12 (B) (A) 10 10 4 10 20 30 40 50 60 70 20 40 60 Titrant volume (mL) Titrant volume (mL) A. The titrand is a weak base in case of (A), but a strong acid in case of (B) B. The half-equivalence point in case of (B) 10 mL, but it is 25 mL in case of (B) C. The equivalence point 50 mL in both cases D. The titrant is a strong acid in case of (A), but a strong base in case of (B) Hd

Which statement is wrong regarding the two titration curves (A) and (B) shown below? 12 12 (B) (A) 10 10 4 10 20 30 40 50 60 70 20 40 60 Titrant volume (mL) Titrant volume (mL) A. The titrand is a weak base in case of (A), but a strong acid in case of (B) B. The half-equivalence point in case of (B) 10 mL, but it is 25 mL in case of (B) C. The equivalence point 50 mL in both cases D. The titrant is a strong acid in case of (A), but a strong base in case of (B) Hd

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

I need help with part c
A 10.0-mL sample of 0.200 M hydrocyanic acid (HCN) is titrated with 0.0998 M NaOH. What is the pH at the equivalence point? For hydrocyanic acid, pKa = 9.31.a) 7.00 b) 8.76 c) 9.31 d) 11.07
Consider the titration of the diprotic weak acid H2A with NaOH. The acid's pKa values are 2.81 and 5.74. 1) What is the predominant form of the acid when the solution has pH=3.6. H2A HA- A^2- none of the above 2)What will be the pH of the solution when it is 1.5M in H2A and 1M in HA^-? What will be the pH of 1.0 L of that solution from part b after addition of 0.4mol NaOH? Thank you!!
2. Draw a graph of pH vs Vh for the titration of a strong acid with a strong base and compare it to a graph for the titration of a weak acid of the same concentration with the same strong base. Comment on the differences and the similarities.
(b) Shown in the graph below is the titration curve that results when 25.0 mL of 0.200 M HCIO is titrated with 0,200 M NaOH, Carefully draw a second curve on the graph that would result from the titration of 25.0 mL. of 0.200 M HCIO, with 0.200 M NaOH. 14- 13 12 11 10- 9. 8 명 7- 6- 5- 4 3 2. 1 35 Volume of 0:200 M NAOH Added (mL.) 10 15 20 25 30 40 45
Needs helpppppppp
Please match the following titration curves for running a base into an acid. pH 7.0 pH 7.0 A graph (A) (C) Equivalence point Volume of the Base Equivalence point Volume of the Base Hd 7.0 (B) Equivalence point Volume of the Base [Choose ] weak acid - weak base titration strong acid - strong base titration weak acid - strong base titration strong acid - weak base titration [Choose ]
What is the silver ion concentration in a solution prepared by mixing 389 mL 0.385 M silver nitrate with 461 mL 0.468M sodium chromate? The ?sp of silver chromate is 1.2×10−12. [Ag+] = ?M
Consider the titration of 40.0 mL of 0.0600 M C6H5NH2 (a weak base; Kb = 4.30e-10) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mLpH = (b) 6.0 mLpH = (c) 12.0 mLpH = (d) 18.0 mLpH = (e) 24.0 mLpH = (f) 45.6 mLpH =
Which of the following indicators is best suited to determine the equivalence point of a titration of 0.25 M ammonium chloride (NH4CI) with a 0.25 M solution of a strong base? The titration curve is shown below. Data: pka (NH4CI) = 9.26 14 12 10 6 4 10 20 30 40 Volume of strong base (mL) Indicator pK HIn Phenolphthalein 9.3 Alizarin Yellow R11.2 Bromothymol blue 7.1 Bromocresol green 4.7 Hd
I need help with fill the blanks spaces
A 25.0 mL sample of a 0.20 M solution of a weak monoprotic acid is titrated with a 0.10 M KOH solution. What volume of base is needed to reach the equivalence point? (A) 20.0 mL (B) 25.0 mL (C) 35.0 mL (D) 50.0 mL