Homework Answers
![mass of NH₃ cl is 0,4870 g is 53.5 g/mol morar mass of why a more of NMy cl in 0.4870 m Moly 53.5 = 0.00 g 10 mors [NHGC1] =](http://img.homeworklib.com/questions/535d7a10-d2c2-11eb-84c9-a1506c3042ca.png?x-oss-process=image/resize,w_560)
![Aslo, Ento] = 0.2799 M pH = pka + log Enth - 9.26 + log (6.2799 ) = 10.7479 0.08910 MANUELINE cs Scanned with the pH in, pha](http://img.homeworklib.com/questions/54b4cdb0-d2c2-11eb-8201-234451123772.png?x-oss-process=image/resize,w_560)
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Question 15 (2 points) A basic buffer is prepared by adding 0.4870 g of NH4Cl to...
Question 13 (2 points) A basic buffer is prepared by adding 0.7185 g of NH4Cl to...
Question 13 (2 points) A basic buffer is prepared by adding 0.7185 g of NH4Cl to 1.00 L of 0.4490 M NH3. Kb (NH3) = 1.8 x 10-5. Calculate the pH of the buffer. Provide your answer to two places after the decimal. Your Answer: Answer Hide hint for Qugstion 13 You must convert the mass of ammonium chloride into molarity. Also, you need to calculate the K, of ammonium ion from the Kb value of ammonia.
Question 9 (2 points) A basic buffer is prepared by adding 0.4565 g of NH4Cl to...
Question 9 (2 points) A basic buffer is prepared by adding 0.4565 g of NH4Cl to 1.00 L of 0.3361 M NH3. Kb (NH3) = 1.8 x 10-5. Calculate the pH of the buffer. Provide your answer to two places after the decimal. Your Answer: Answer
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250...
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250 ml of 1.00 M ammonium chloride. What is the pH of the buffer? ( Ka of NH4+=5.6*10^-10, Kb of NH3= 1.8*10^-5)
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250...
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250 ml of 1.00 M ammonium chloride. What is the pH of the buffer? ( Ka of NH4+=5.6*10^-10, Kb of NH3= 1.8*10^-5)
Calculate the pH of a buffer prepared by dissolving 0.10 mol of NH4Cl in 1.00 L...
Calculate the pH of a buffer prepared by dissolving 0.10 mol of NH4Cl in 1.00 L of 0.15 M NH3. Kb = 1.8 x 10 % for NH3. O a. 11.34 O b. 2.72 O ü O ö Oe. 4.56
A buffer solution is prepared by dissolving 1.600 g of ammonium chloride (NH,CI) into 100.00 mL...
A buffer solution is prepared by dissolving 1.600 g of ammonium chloride (NH,CI) into 100.00 mL of a 0.160 M solution of ammonia (NH3). The Kb of ammonia is 1.8 x 10-5. What is the pH of the solution?
If you needed to perform a reaction in a controlled pH environment that was fairly basic,...
If you needed to perform a reaction in a controlled pH environment that was fairly basic, you might choose to use the ammonium and ammonia buffer system. How many grams of solid ammonium chloride would you have to add to 250 liters of 0.165M NH3 to obtain a buffered solution of pH = 8.85? (Kb of NH3 = 1.8 x 10-5)
If you needed to perform a reaction in a controlled pH environment that was fairly basic,...
If you needed to perform a reaction in a controlled pH environment that was fairly basic, you might choose to use the ammonium and ammonia buffer system. How many grams of solid ammonium chloride would you have to add to 1.250 liters of 0.165M NH3 to obtain a buffered solution of pH = 8.85? (Kb of NH3 = 1.8 x 10-5)
A pH 9.56 buffer was prepared by dissolving 2.00 mole ammonia (Kb 1.8 x 10-5) and...
A pH 9.56 buffer was prepared by dissolving 2.00 mole ammonia (Kb 1.8 x 10-5) and 1.00 mol ammonium chloride in water to form a total solution volume of 1.00 L. Which is the final pH when 200.0 mL of the above buffer is treated with 10.0 mL 10.0 M NaOH? O A. 9.28 B. 9.86 C. 9.95 O D. 13.7
Calculate the pH of a solution prepared by adding 20.0 mL of 0.100 M HCl to...
Calculate the pH of a solution prepared by adding 20.0 mL of 0.100 M HCl to 80.0 mL of a buffer that is comprised of 0.25 M NH3 and 0.25 M NH4Cl. Kb of NH3 = 1.8 x 10-5. ОА. 9.17 ОВ. 4.83 0 o С. 9.34 OD.9.26 OE. 4.66
Question 13 (2 points) A basic buffer is prepared by adding 0.7185 g of NH4Cl to 1.00 L of 0.4490 M NH3. Kb (NH3) = 1.8 x 10-5. Calculate the pH of the buffer. Provide your answer to two places after the decimal. Your Answer: Answer Hide hint for Qugstion 13 You must convert the mass of ammonium chloride into molarity. Also, you need to calculate the K, of ammonium ion from the Kb value of ammonia.
Question 9 (2 points) A basic buffer is prepared by adding 0.4565 g of NH4Cl to 1.00 L of 0.3361 M NH3. Kb (NH3) = 1.8 x 10-5. Calculate the pH of the buffer. Provide your answer to two places after the decimal. Your Answer: Answer
Calculate the pH of a buffer prepared by dissolving 0.10 mol of NH4Cl in 1.00 L of 0.15 M NH3. Kb = 1.8 x 10 % for NH3. O a. 11.34 O b. 2.72 O ü O ö Oe. 4.56
A buffer solution is prepared by dissolving 1.600 g of ammonium chloride (NH,CI) into 100.00 mL of a 0.160 M solution of ammonia (NH3). The Kb of ammonia is 1.8 x 10-5. What is the pH of the solution?
A pH 9.56 buffer was prepared by dissolving 2.00 mole ammonia (Kb 1.8 x 10-5) and 1.00 mol ammonium chloride in water to form a total solution volume of 1.00 L. Which is the final pH when 200.0 mL of the above buffer is treated with 10.0 mL 10.0 M NaOH? O A. 9.28 B. 9.86 C. 9.95 O D. 13.7
Calculate the pH of a solution prepared by adding 20.0 mL of 0.100 M HCl to 80.0 mL of a buffer that is comprised of 0.25 M NH3 and 0.25 M NH4Cl. Kb of NH3 = 1.8 x 10-5. ОА. 9.17 ОВ. 4.83 0 o С. 9.34 OD.9.26 OE. 4.66
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