Acid Base Equilibria (Common Ion Effect) Determine the pH of (a) a 0.20 M NH3 solution, (b) a solution that is 0.20 M in NH3 and 0.30 M NH4Cl.
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Acid Base Equilibria (Common Ion Effect)
Determine the pH of (a) a 0.20 M NH3 solution, (b) a solution that is 0.20 M in NH3 and 0.30 M NH4Cl.
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- A mixture of 100 ml of 0.025 M NH3 and 150 mL of 0.025 M NH4Cl was made. For this problem you need to show your calculation for each number. (A) What is the resulting concentration of the two solutes after mixing the solutions?(B) What is the pH of the solution produced?(C) What will happen if additional 100 mL water is added to the mixture?You are asked to prepare a pH = 3.00 buffer solution startingfrom 1.25 L of a 1.00 M solution of hydrofluoric acid(HF) and any amount you need of sodium fluoride (NaF).(a) What is the pH of the hydrofluoric acid solution priorto adding sodium fluoride? (b) How many grams of sodiumfluoride should be added to prepare the buffer solution?Neglect the small volume change that occurs when the sodiumfluoride is added.Calculate the pH change that results when 11 mL of 5.1 M NaOH is added to 790. mL of each the following solutions. Use the Acid-Base Table. (a) pure water 4.0 5.84 (b) 0.10 M NH4CI 4.0 5.43 (c) 0.10 M NH3 4.0✔ X (d) a solution that is 0.10 M in each NH4+ and NH3 4.0✔
- Calculate the pH change that results when 15 mL of 2.7 M HCI is added to 600. mL of each of the following solutions. Use the Acid-Base Table. (a) pure water 4.0 -5.82 (b) 0.10 M CH3COO- 4.0 4.43 (c) 0.10 M CH3COOH 4.0 X (d) a solution that is 0.10 M in each CH3COO and CH3COOH. 4.0Calculate the pH change that results when 15 mL of 2.0 M HCI is added to 580. mL of each of the following solutions (a) pure water 4.0-5.70 (b) 0.10 M CH3COO 4.04.28 (c) 0.10 M CH3COOH 4.0 (d) a solution that is 0.10 M in each CH3COO and CH3COOH. 4.01.56 g of sodium acetate, NaCH;CO, has been 0.20 M ammonia, NH3, and 0.20 M ammonium 4. What is the pH of 0.15 M acetic acid to which 3. What is the pH of a solution that consists of aqueous solution of NH3? the same when you (c) add solid NaCl to a dilute aqueous solution of (b) add solid sodium acetate to a dilute a (a) add solid ammonium chloride to a dilute 1. Does the pH of the solution increase, decrease, or 17.1 and 17.2.) stay solution of acetic acid? aqueous NaOH? 2 Does the pH of the solution increase, decrease, or stay the same when you (a) add solid sodium oxalate, Na,C,O4, to 50.0 mL of 0.015 M oxalic acid, H,C,O4? (b) add solid ammonium chloride to 75 mL of 0.016 M HCl? (c) add 20.0 acetate, NaCH;CO2? of NaCl to 1.0 L of 0.10 M sodium *What is the pH of a solution that consists of chloride, NH4CI? added?
- 2.0 g of NaOH is dissolved in distilled water to prepare 100 mL solution. 20.0 mL of this solution reaches to the equivalence point when 25 mL of an acid solution containing 1.22 monoprotic weak acid is added. (a) Calculate the molar mass of the unknown acid. (b) After 15.0 mL of NaOH solution had been added during the titration, the pH was determined to be 4.7. What is the Ka of the unknown acid? (NaOH = 40.0 g/mol) unknownThe compound dimethylamine is a weak base like ammonia. A solution contains 0.263 M (CH3)2NH₂+ and 0.365 M dimethylamine, (CH3)2NH. The pH of this solution isA buffer is made by adding 0.300 mol CH3COOH and 0.300 mol CH3COONa to enough water to make 1.000 L of solution. ThepH of the buffer is 4.74. (a) Calculate the pH of this solution after 5.0 mL of 4.0 M NaOH(aq) solutionis added. (b) For comparison, calculate the pH of a solution made by adding 5.0 mL of 4.0 M NaOH(aq) solution to 1.000 L ofpure water.
- (a) Calculate the pH in a solution prepared by dissolving 0.050 mol of acetic acid and 0.020 mol of sodium acetate in water and adjusting the volume to 500 mL.(b) Suppose 0.010 mol of NaOH is added to the buffer from part (a).Calculate the pH of the solution that results.(7) Calculate the pH of each of the following solutions: (a) 0.1000M Propanoic acid( HC H O,,K=1.3x105) (b) 0.1000M sodium propanoate (Na C HỎ) (c) 0.1000M HC₂H₂O, and 0.1000M Nа С¸¸0₂ 3 5 52 (d) After 0.020 mol of HCl is added to 1.00 L solution of (a) and (b) above. (e) After 0.020 mol of NaOH is added to 1.00 L solution of (a) and (b) above.3) 2.0 g of NaOH is dissolved in distilled water to prepare 100 mL solution. 20.0 mL of this solution reaches to the equivalence point when 25 mL of an acid solution containing 1.22 g unknown monoprotic weak acid is added. (a) Calculate the molar mass of the unknown acid. (b) After 15.0 mL of NaOH solution had been added during the titration, the pH was determined to be 4.7. What is the Ka of the unknown acid? (NaOH = 40.0 g/mol)