Calculate the pH of the following acid–base buffers. Be sure to state and justify any assumptions you make in solving the problems. a. 100.0 mL of 0.025 M formic acid and 0.015 M sodium formate b. 50.00 mL of 0.12 M NH3 and 3.50 mL of 1.0 M HCl c. 5.00 g of Na2CO3 and 5.00 g of NaHCO3 diluted to 0.100 L 4. (10 Points) Calculate the pH of the buffers in problem 3 after adding 5.0 mL of 0.10 M HCl. Be sure to state and justify any assumptions you make in solving the problems. 5. (10 points) Calculate the pH of the buffers in problem 3 after adding 5.0 mL of 0.10 M NaOH. Be sure to state and justify any assumptions you make in solving the problems. I found that the pH of problem 3a is 3.53 and the pKa is 3.75. For 3b I found the pH to be 9.10 and the pKa of HCL to be 9.24. For problem 3c I found the pH to be 10.22 and the pKa to be 10.3. Hopefully you can use this info to find 4) and 5).
QUESTION 3A
QUESTION 3B
QUESTION 3C
QUESTION 4
QUESTION 5
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Calculate the pH of the following acid–base buffers. Be sure to state and justify any assumptions...
Calculate the pH of the following acid–base buffers. Be sure to state and justify any assumptions you make in solving the problems. a. 100.0 mL of 0.025 M formic acid and 0.015 M sodium formate b. 50.00 mL of 0.12 M NH3 and 3.50 mL of 1.0 M HCl c. 5.00 g of Na2CO3 and 5.00 g of NaHCO3 diluted to 0.100 L
7. Use the systematic approach to equilibrium problems to calculate the pH of the following solutions. Be sure to state and justify any assumptions you make in solving the problems. a. 0.050 M HClO4 b. 1.00 × 10–7 M HCl c. 0.025 M HClO d. 0.010 M HCOOH e. 0.050 M Ba(OH)2 f. 0.010 M C5H5N
Use the systematic approach to solving equilibrium problems to calculate the pH of 0.1 M solutions of (a) malonic acid, H2A; (b) sodium hydrogenmalonate, NaHA; and (c) sodium malonate, Na2A. Be sure to state and justify any assumptions you make in solving the problems.
1) Calculate the pH of a solution produced by mixing 100.0 mL of 0.10 M HCl(aq) and 100.0 mL of 0.20 M NaOH(aq). 2) Calculate the pH of an aqueous solution made by mixing 100.0 mL of 0.40 M NH4Cl and 50.0 mL of 0.40 M NaOH. The pKa of NH4+ is 9.24.
Post-Lab Assignment: pH and Buffers 1. A buffer is prepared from a weak acid with a Ka - 7.1 x 104 and its conjugate base. a. What pH would provide maximum buffer capacity? b. What would be the buffer range for this acid? (Your answer should show the lowest and the highest pH that would provide a reasonably effective buffer.) 2. If you were provided with a 0.1 M solution of an unknown weak acid and a 0.1 M solution...
26. Calculate the pH of 0.25 M HNO2 (K, -4.0 x 10). Justify any assumptions made regarding you (hint: check assumption with % ionization). Show all work for full credit. (6 pts)
This problem deals with Acid-base titrations and pH scale for a weak acid and a weak base. Calculate the pH of the solution that results from adding 7.5 [ml] of Ammonia (NH3) to a beaker that contains, 100 ml of distilled water and 15 ml of 0.1 M Acetic acid (HC2H3O2). A buret containing 50 mL of 0.1 M Ammonia (NH3) is being used as the titrant. The beaker containing 100 ml of distilled water, and 15 ml of 0.1...
Phosphoric acids have three pKa. You can find their value from appendix 11 in the textbook (2.148, 7.199, 12.35) . Calculate the pH of a buffer that is 0.10 M in KH2PO4 and 0.050 M in Na2HPO4. What is the pH after adding 5.0 mL of 0.20 M HCl to 0.10 L of this buffer?
26. Calculate the pH of 0.25 M HNO2 (K. = 4.0 x 10). Justify any assumptions made regarding (hint: check assumption with % ionization). Show all work for full credit. (6 pts)
Calculate the pH of each of the following strong acid solutions. 5.00 mL of 1.00 M HCl diluted to 0.550 L . A mixture formed by adding 52.0 mL of 2.5×10−2M HCl to 160 mL of 1.0×10−2M HI.