MISSED THIS? Read Section 18.4 (Pages 803-817); Watch KCV 18.48 Consider the curve shown here for the titration of a weak monoprotic acid with a strong base. E 14 12- 10- 8 6- 4- 2- 0 40 10 20 30 Volume of base added (mL) 0 ▸ Part B ▼ Part C At what volume of added base is the pH calculated by working an equilibrium problem based on the initial concentration and K, of the weak acid? Express your answer in milliliters as an integer. ΟΙ ΑΣΦ V= Submit Previous Answers Request Answer ? mL

MISSED THIS? Read Section 18.4 (Pages 803-817); Watch KCV 18.48 Consider the curve shown here for the titration of a weak monoprotic acid with a strong base. E 14 12- 10- 8 6- 4- 2- 0 40 10 20 30 Volume of base added (mL) 0 ▸ Part B ▼ Part C At what volume of added base is the pH calculated by working an equilibrium problem based on the initial concentration and K, of the weak acid? Express your answer in milliliters as an integer. ΟΙ ΑΣΦ V= Submit Previous Answers Request Answer ? mL

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...

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Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. NEXT > A solution is prepared with 0.55 M HNO2 and 0.75 M KNO2. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) 1 2 HNO₂(aq) + H₂O(l) 1 3 H3O+ (aq) + NO₂ (aq)
Determine the concentration of CH NH¸* in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of CH NH+. The Kb for CH NH₂ is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 2 1 2 3 NEXT > 2 A buffer solution contains dissolved CH NH and CH NH Cl. The initial concentration of CH NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of CH NH+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CH NH2(aq) + H₂O(I) = OH(aq) + C HẠNH, (aq) RESET 0 0.50 x 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x + 6.3 x 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10
Answer Questions #27 through #31 about the titration curves below (labeled a and b) for two different bases. The titrant acid used in both cases was 0.100 M HCl and the volume of the base solutions in both cases was 75.0 mL mL. 14 14 12 12 - 10- 10 8- 6. 4. 2- 2- 20 40 60 80 100 20 40 60 80 100 Volume of acid added (mL) (a) (b) Volume of acid added (mL) 2014 Pearson Education Inc P Type here to search 11:17 AM (? 3/18/2021 -> ort sc 80 6. ece num ER/TY || на 0 04 2C Hd
A buffer is made with 0.50 M weak acid and 0.50 M sodium salt of the conjugate base. The pKa of the weak acid is 9.30 After the addition of a small amount of strong concentrated acid, the new equilibrium concentrations are 0.6 M weak acid and 0.4 M base. Calculate the new pH. Enter result with 2 decimal places, digits only.
A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. The Ka for CH3COOH is 1.8 x 10-5. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0] [0.300 -x] 1.8 x 10-² [0.300] 0 [0.0300 + x] 5.6 x 10-1⁰ 2.75 Kb 1.30 x 10-² [0.0300] [0.0300 -x] 5.6 x 10-8 5.04 [0.150] [0.150 + x] 0.523 8.96 A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information…
Use the References to access important values if needed for this question. A 30.0 mL sample of 0.316 M diethylamine, (C₂H5)2NH, is titrated with 0.245 M hydroiodic acid. At the titration midpoint, the pH is Use the Tables link in the References for any equilibrium constants that are required. Submit Answer Retry Entire Group 8 more group attempts remaining Previous Email Instructor Nex Sav
MISSED THIS? Read Section 18.4 (Page); Watch KCV 18.4B. Consider the curve shown here for the titration of a weak monoprotic acid with a strong base. Hd 14 12 10 8 6420 80 120 160 40 Volume of base added (mL) The figure shows pH as a function of volume of base added. The pH is measured from 0 to 14 on the y-axis, while the volume of base added is measured from 0 to 160 milliliters on the x-axis. The curve of the plot goes up gradually from pH 2.3 at 0 milliliters to pH 5.8 at 49 milliliters, next the plot goes up steeply to pH 11.8 at 51 milliliters, and finally the plot goes up gradually to pH 12.2 at 160 milliliters. ✓ Correct An equilibrium problem based on the initial concentration and Ka of a weak acid should be solved for aqueous solution of the weak acid. This is true for the initial state of titration, when no base has been addition of a small amount of a strong base turns this solution into a buffer whose pH is calculated in way. Part D At what volume of added base does pH =…
Use the following two titration curves to answer each of the following statements. Select the choice that completes the statement correctly. 14 pH 7 0 Graph A 25 volume of titrant added (mL) In graph A, the end point occurs at a In graph B, the equivalence point occurs at a + 141 pH 7 0 Graph B 25 volume of titrant added (mL)
What is the effective pH range for a sodium acetate/acetic acid buffer? Ka = 1.80 x 105. %3D Enter your answer to three decimals. to
12.0 10.0 8.0 A pH 6.0 4.0 2.0 0.0 C 0 5 10 15 20 25 30 mL of 0.1 M NaOH The graph above shows the titration curves of four monoprotic acids of varying strengths. All of the acids start out at 0.1 M concentration and 25.0 mL volume. Choose all of the correct statements about these titration curves from the choices below. The titration curve labelled "D" is generated by the strongest acid in the series. In the curves shown above the stronger the acid the less NaOH required for neutralization. The stronger the acid the more important is the pKa of the Indicator used for titration. The Ka of the acid which generates curve "C" is about 103 The weaker the acid the lower the pH of the neutralization point. The acid which generates curve "D" has the highest neutralization-point pH in the series.
2. Fill in the following table to show the theoretical results for the titration of 1.0 L of 0.20 M acetic acid by adding the designated amount of solid (no volume change) potassium hydroxide, KOH. Show sample calculation of your work. Amount of NaOH added 0.0 mol 0.010 mol 0.020 mol 0.030 mol 0.040 mol Amount of acetic acid remaining pH [H+]
Answer using this data for the remaining questions on this page: For 1.0L of an acetic acid solution: Ka = 1.8 x 10-5 and [HA] = 0.250M 2. Calculate the pH of the solution. 3. What is the pka? 4. Calculate the pH of the solution if you make it a buffer by adding enough solid sodium acetate to make the concentration of acetate ion equal to 0.35M. The volume of the solution does not change. 5. What is the new concentration of [HA] if 2.0mL of 5.00M of HCI is added to 1.000L of the solution above? 6. What is the new pH?