8. What is the pH of a weak acid with [HA] = 0.125 mol/L and Ka = 5.4×107?9. A buffer is created by adding 0.35 mol of sodium benzoate to 1.00 L of a 0.40 mol/L benzoic acidsolution. The Ka of benzoic acid is 6.3×105. Determine the pH of the buffer. 13. Draw the following galvanic cell including the flow of electrons, half cell reactions, and potentialdifferenceFes|Fe(NO3)2(aq) || Cu(NO3)2(aq) |Cu(s)14. Determine the shape of the following molecules and identify what intermolecular forces exist ina pure sample of the compound.a. SO-b. BeF2c. PF15. Draw the short form electron configuration for Potassium.

ANSWER 13ANSWER 15-ANSWER 8 ANSWER 9

Answered: 8. What is the pH of a weak acid with…

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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What quantity in moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 2.80? (Ka for HF is 6.8 × 10⁻⁴)
A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system. Choices: HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol) NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)
a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF.The Ka for HF is 7.2×10-4. pH = b) Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0014 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3×10-7 Сoncentration = M c) You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH , the pH is 5.50. What is the Ka value of HA ? = d) Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. 40.0 mL pH = 50.0 mL pH =
Consider the titration of a 60.0 mL of 0.321 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH. 1. What is the pH before any base has been added? 2. After 30.0 mL of KOH have been added, identify the primary species left in the solution. 3. After 30.0 mL of KOH have been added, what would the pH of the solution be? 4. After 75.0 mL of KOH have been added, identify the primary species left in the solution. 5. After 75.0 mL of KOH have been added, what would the pH of the solution be?
A beaker with 1.0 x 10^2 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.80 mL of a 0.360 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740.
A buffer solution contains 1.250 mol of phenol, C6H5OH, and 0.950 mol of sodium phenoxide, C6H5ONa, in 1.00 L of solution. Ka = 1.30 x 10-10. a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.525 mol of NaOH? (assume no volume change upon the addition of the NaOH) c. To the buffer produced in part a, what is the pH of the buffer after the addition of 0.225 mol of HCI? (assume no volume change up the addition of the HCI)
Consider a buffer made by dissolving 0.140 mol cyanic acid, HCNO, and 0.11 mol potassium cyanate, KCNO, in enough water to make a 1-L solution. Assuming that the volume does not change, what is the pH of the buffer before any acid or base is added? Ka = 3.5 x 10-4 O 3.46 O 3.25 3.36 O None of the above
1a. How many grams of solid sodium cyanide should be added to 1.50 L of a 0.108 M hydrocyanic acid solution to prepare a buffer with a pH of 10.043 ?grams sodium cyanide = 1b. How many grams of solid ammonium bromide should be added to 1.00 L of a 0.244 M ammonia solution to prepare a buffer with a pH of 9.820 ? grams ammonium bromide = 1c. How many grams of solid sodium hypochlorite should be added to 1.00 L of a 0.206 M hypochlorous acid solution to prepare a buffer with a pH of 8.249 ?grams sodium hypochlorite =
A buffer solution contains 0.448 M NH4Cl and 0.319 M NH3 (ammonia). Determine the pH change when 0.092 mol KOH is added to 1.00 L of the buffer.pH after addition − pH before addition = pH change = 2.
8. What is the pH of a weak acid with [HA] = 0.125 mol/L and Ka = 5.4×107? 9. A buffer is created by adding 0.35 mol of sodium benzoate to 1.00 L of a 0.40 mol/L benzoic acid solution. The Ka of benzoic acid is 6.3×105. Determine the pH of the buffer.

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