Calculate the pH of the following buffer solutions: c) Dilute 57 mL of concentrated NH3 (29.0%...
Calculate the pH of the following buffer solutions:
c) Dilute 57 mL of concentrated NH3 (29.0% w / w; 0.90 g / mL) and
7 g of NH4Cl in sufficient
water to give 100 mL of solution.
Homework Answers
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Calculate the pH of the following buffer solutions:
c) Dilute 57 mL of concentrated NH3 (29.0%...
analytical chemistry: Calculate pH of this solution Calculate PH (concentrated) 57 ml of NH3 are diluted...
analytical chemistry: Calculate pH of this solution
Calculate PH (concentrated) 57 ml of NH3 are diluted in enough water (29.0% w/w; 0-90g/mL) and 79 of NH4Cl to prepare a 108 ml Solution
calculate the pH of a buffer that is created by mixing 2.0 mL of .10M NH3...
calculate the pH of a buffer that is created by mixing 2.0 mL of .10M NH3 with 10 mL of .10M NH4CL and 20 mL of distilled water in a 50 mL beaker
a) Calculate the pH of a buffer system that contains o.200 M of NH3(aq) and o.200...
a) Calculate the pH of a buffer system that contains o.200 M of NH3(aq) and o.200 M of NH4Cl(aq). The Kb of NH3(aq) is 18 x 10-5. Consult Textbook Numerical Answer pH b) Calculate the change in pH when 6.00 mL of 100 M HCl is added to 100.0 mL of the buffer solution. Numerical Answer: c) Calculate the change in pH when 6.00 mL of o.100 M NaOH is added to 100.0 mL of the buffer solution. Numerical Answer:
What is the pH of a buffer formed from 50 mL of 15.0 M NH3 and...
What is the pH of a buffer formed from 50 mL of 15.0 M NH3 and 53.5 g of NH4Cl in enough water to make 500 mL of solution? (Kb = 1.8 x 10-5)
Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 4.550 g...
Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 4.550 g KH2PO4 and 1.871 g K2HPO4 in water to give 350. mL of solution. (b) a solution made by mixing 35.00 mL 0.35 M N2H4 with 15.00 mL 0.21 M N2H5Cl. The base dissociation constant Kb is 8.50 x 10-7 for N2H4 . Assume that the final volume is the sum of the volunes of the two solutions that are mixed.
Calculate the pH at 25°C of 189.0 mL of a buffer solution that is 0.420 M...
Calculate the pH at 25°C of 189.0 mL of a buffer solution that is 0.420 M NH4Cl and 0.420 M NH3 before and after the addition of 2.80 mL of 6.0 M HNO3. (The pKa for NH4+ = 9.75) pH before= pH after=
Your supervisor asks you to prepare 474.00 mL of ammonium buffer solution 0.1 M with pH=...
Your supervisor asks you to prepare 474.00 mL of ammonium buffer solution 0.1 M with pH= 9.00, from a concentrated ammonia solution (16%w/w, d=0.98g/mL) and solid ammonium chloride (97% w/w). (MW of NH3 = 17.031 g/mol and FW of NH4Cl = 53.491 g/mol and pKa NH4+/NH3 =9.24). How many grams of the solid ammonium chloride do you need? Consider two decimal places for the answer.
6. (a) Calculate the pH of the 0.39 M NH3/ 0.73 M NH4Cl buffer system. pH...
6. (a) Calculate the pH of the 0.39 M NH3/ 0.73 M NH4Cl buffer system. pH = (b) What is the pH after the addition of 20.0 mL of 0.075 M NaOH to 80.0 mL of the buffer solution? pH =
Calculate the pH at 25°C of 220.0 mL of a buffer solution that is 0.350 M...
Calculate the pH at 25°C of 220.0 mL of a buffer solution that is 0.350 M NH4Cl and 0.350 M NH3 before and after the addition of 2.40 mL of 6.0 M HNO3. (The pKa for NH4+ = 9.75)
Calculate the pH at 25°C of 246.0 mL of a buffer solution that is 0.450 M...
Calculate the pH at 25°C of 246.0 mL of a buffer solution that is 0.450 M NH4Cl and 0.450 M NH3 before and after the addition of 1.90 mL of 6.0 M HNO3. (The pKa for NH4+ = 9.75) Part 1: pH before= Part 2: pH after=
analytical chemistry: Calculate pH of this solution
Calculate PH (concentrated) 57 ml of NH3 are diluted in enough water (29.0% w/w; 0-90g/mL) and 79 of NH4Cl to prepare a 108 ml Solution
a) Calculate the pH of a buffer system that contains o.200 M of NH3(aq) and o.200 M of NH4Cl(aq). The Kb of NH3(aq) is 18 x 10-5. Consult Textbook Numerical Answer pH b) Calculate the change in pH when 6.00 mL of 100 M HCl is added to 100.0 mL of the buffer solution. Numerical Answer: c) Calculate the change in pH when 6.00 mL of o.100 M NaOH is added to 100.0 mL of the buffer solution. Numerical Answer:
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