(2). For the buffer system in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCI and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer?
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- A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?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. 4.0
- For the buffer system in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer?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)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.
- A 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.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✔For the titration of 10.0 mL of 0.200 M acetic acid with 0.150 M sodium hydroxide, determine the pH when: (a) 10.0 mL of base has been added.(b) 13.3 mL of base has been added. (c) 16.6 mL of base has been added.
- Chemistry A 94.0 mL sample of 0.0300 M HIO, is titrated with 0.0600 M NaOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.1 mL pH = (d) 47.9 ml pH- (b) 46.1 mL pH = (e) 90.7 ml pH = (c) 47.0 mL pH =(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.Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 46 g of NHĄCI dissolved in 1.00 L of 0.920 M NH3? pH = i (b) How many moles of acid are required to change the pH of this solution by 0.07 pH units? i mol (c) Suppose 4.8 mL of 11.8 M HCI solution is added to 146 mL of the solution of Part (a). Calculate the new pH. pH = i