4. What is the pH of a solution containing 0.2 M acetic acid (pK₂ = 4.7) and 0.7 M sodium acetate? Show detailed calculations. Draw the titration curve, point arrow at the position on this curve that corresponds to this pH. How many equivalents of NaOH were added to weak acid? 5. A compound has pKa= 7.2 To 150ml of 1M of this compound at pH=8.0, is added 10 ml of 1M HCI. What is the pH of resulted solution? Show detailed calculations Draw the titration curve, point arrows at the original pH and the pH after addition of HCI on this curve.

4. What is the pH of a solution containing 0.2 M acetic acid (pK₂ = 4.7) and 0.7 M sodium acetate? Show detailed calculations. Draw the titration curve, point arrow at the position on this curve that corresponds to this pH. How many equivalents of NaOH were added to weak acid? 5. A compound has pKa= 7.2 To 150ml of 1M of this compound at pH=8.0, is added 10 ml of 1M HCI. What is the pH of resulted solution? Show detailed calculations Draw the titration curve, point arrows at the original pH and the pH after addition of HCI on this curve.

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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1. Identify each move below as attack, leave, protonate (or deprotonate), or rearrang e. A. B. н- но- O-H н.8н н,о° +] D.[ E. F.
3. If you didn't have a pH meter, how would you make 1.00 L of 40.0 mM potassium phosphate buffer at pH 6.96, given ONLY potassium phosphate monobasic (KH₂PO4) and potassium phosphate dibasic (K₂HPO4)? These are the only two chemical available -no strong acid or base are needed. Include details such as masses and when/how you would bring the volume up to 1L. Show your calculations. Use pka2=7.20 for phosphoric acid.
10. Calculate the pH of a solution in which 32.0 ml of 0.150 M KOH has been added to 28.0 ml of 0.100 M HCI. 11. Calculate the pH of a buffer consisting of 1.25 M acetic acid and 0.75 M potassium acetate. Ka = 1.8 x 10 for acetic acid. %3D 12. Calculate the pH of a buffer consisting of 0.590 moles of ammonia and 1.57 moles ammonium chloride. K, = 1.8 x 10 for ammonia.
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. 3 A 50.0 mL solution of 0.300 M CH3COOH was titrated with 0.300 M NaOH. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction.. Before (mol) Change (mol) After (mol) 0.150 Initial (M) Change (M) Equilibrium (M) 0.0150 - x CH3COOH(aq) + OH (aq) 0 -0.150 0 1 0.150 -0.150 0.300+ x 0 0.0200 + x 0.300 CH3COO (aq) + 0.0150 0.150 -X 2 0.150 - x 0.300 0.300 - x 0.0200 - x -0.300 -0.0150 2 0.150 A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence…
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
Part 3: pH after addition of 0.145mol HCl: Round your answer to 2 decimal places
Bicarbonate Buffer Prepare 100 mL of 0.200 bicarbonate buffer, pH 10, by calculating the mass of sodium bicarbonate and sodium carbonate. Use the Henderson-Hasselbalch equation to calculate the volume of each stock solution needed. pH = pKa + log [conjugate base] / [weak acid]1 3. Check your calculations with other students. See the instructor if there is uncertainty.
4. Use the following steps to determine how to make 600 mL of a 0.1M acetate buffer, pH 5.0, using 0.1M acetic acid and 0.1M sodium acetate. a. Consider the Henderson-Hasselbalch equation. pH =pKa+ log [base] [actd] Using the desired pH (5.0) and pKą of acetic acid, use the Henderson Hasselbach equation to determine a ratio of [base] [acid] required for this buffer. (For example, your answer should look something like this: [base] [acid] =2.3 Note that this is NOT the ratio you will obtain - it is just an example) b. Given the example above, we can set [acid] = x and [base] =2.3x. Remember that the concentration of acid and base should equal the desired molarity, which 0.1. Based on this, a second equation can be obtained - given the example above, the equation would. be x + 2.3x = 0.1. Use this to solve for x, which represents the concentration of acid. ([acid]), and for [base].
Please please solve exact and accurate answers solve three sub-parts I'll rate
5. Calculate the pH of a Buffer of Lactic Acid (HC2H502) 0.12M and Potassium Lactate (KC2H502) 0.11M. The Ka = 1.4x10-4
2. Three buffers are made by combining a 1 M solution of acetic acid with a 1 M solution of sodium acetate in the ratios shown below. Buffer 1: Buffer 2: Buffer 3: 1 M acetic acid 10 mL 50 mL 90 mL (i) (ii) (iii) 1 M sodium acetate 90 mL 50 mL 10 mL a. Which of these statements is true of the resulting buffers? pH of buffer 1 pH of buffer 2 > pH of buffer 3 b. Which solution resists changes in pH most effectively?
Calculate the pH of 1.00 L of the buffer Part 1 of 3 Note: Reference the pK of acids at 25 °C table for additional information. a 4.73 pH of starting buffer: Be sure your answer has the correct number of significant digits. Part 2 of 3 ×... 4.76 Part 3 of 3 x10 × pH after addition of 0.040 mol NaOH: Be sure your answer has the correct number of significant digits. 4.61 x10 X Ś x10 0.99 M CH3COONa 1.02 M CH₂COOH X before and after the addition of the following species. (Assume there is no change in volume.) Ś pH after further addition of 0.133 mol HCl: Be sure your answer has the correct number of significant digits. Ś