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calculate the ph of the following solutions there is 3 different problems so make sure to...
2) Calculate the pH of each of the following solutions. a) 0.35 M H2SO4 b) 0.35 M HCN c) 0.35 M KOH d) 0.35 M CaBr2 e) 0.35 M KCN f) 0.35 M CH3CH2NH2 g) 0.35 M NaHSO4 h) 0.35 M CH3CH2NH3Br
f) pH of 0.35 M CH3CH2NH2 g) pH of 0.35 M NaHSO4 h) pHos 0.35 M CH3CH2NH3Br
Please write out equation used and indicate the values used where in each equation. ICE tables, where applicable. 2) Calculate the pH of each of the following solutions. (5 pts each) a) 0.35 M H2SO4 b) 0.35 M HCN c) 0.35 M KOH d) 0.35 M CaBr2 e) 0.35 M KCN f) 0.35 M CH3CH2NH2 g) 0.35 M NaHSO4 h) 0.35 M CH3CH2NH3Br
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.
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...
3. Measure the pH of the solutions described in the Data Table below. Make sure the electrode bulb is fully immersed before measuring. pH Data for Acetate Buffers mL of 0.60 M HC HOA mL of 0.60 M NaC2H302 Solution pH 30 2 30 3 30 10 4 10 30 5 20 20 4. Explain the pH for the five solutions. Consider the relative amounts of acid and base in each.
For each of the following solutions, calculate the initial pH and the final pH after adding 0.0100 mol of NaOH. For 300.0 mL of a buffer solution that is 0.220 M in HCHO2 and 0.295 M in KCHO2, calculate the initial pH and the final pH after adding 0.0100 mol of NaOH(Ka=1.8⋅10−4). For 300.0 mL of a buffer solution that is 0.3187 M in CH3CH2NH2 and 0.2987 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding...
In this experiment you will be measuring pH for several different solutions. A pH probe will be used rather than pH paper as it will be more accurate. You will be testing the pH of six solutions: deionized water, 0.1 M HCl, 0.1 M HCH3COO, 0.1 M NaCH3COO, 0.1 M NaOH, and a buffer made by mixing equal parts of HCH3COO and NaCH3COO. You will measure the pH of each solution three times: Neat - just the solution After the...
For each of the following solutions, calculate the initial pH and the final pH after adding 0.010 mol of NaOH. 12A. For 280.0 mL of a buffer solution that is 0.205 M in HCHO2 and 0.315 M in KCHO2, calculate the initial pH and the final pH after adding 0.010 mol of NaOH. 12B. For 280.0 mL of a buffer solution that is 0.325 M in CH3CH2NH2 and 0.295 M in CH3CH2NH3Cl, calculate the initial pH and the final pH...