What is the pH of a buffer prepared by mixing 20.00 mL of 0.0300 M ammonium chloride with 40.00 mL of 0.0450 M ammonia?...
What is the pH of a buffer prepared by mixing 20.00 mL of 0.0300 M ammonium chloride with 40.00 mL of 0.0450 M ammonia? What is the resulting pH if 1.00 mL of 0.10 M HCl is added to this solution?
Homework Answers
Buffer solution is a solution which resist in its pH change is
small amount of acid or base or water is added to it.
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What is the pH of a buffer prepared by mixing 20.00 mL of 0.0300 M ammonium chloride with 40.00 mL of 0.0450 M ammonia?...
3- What is the pH of a solution prepared by mixing 50 mL of 0.0219 M ammonium chloride with 50 mL of 0.0292 M ammonia?...
3- What is the pH of a solution prepared by mixing 50 mL of 0.0219 M ammonium chloride with 50 mL of 0.0292 M ammonia? Report your answer to three decimal places. ANS:.. . .. . ......... ... ... ..... ..... 4- Calculate the pH if you add 1 ml of 0.01 M HCl to the buffer from question #3. Repost you answer to three decimal places. ANS:.. . . ... 5- Calculate the pH if you added 1 mL...
4) A buffer solution is prepared by dissolving 5.40 g of ammonium chloride in 20.0 mL...
4) A buffer solution is prepared by dissolving 5.40 g of ammonium chloride in 20.0 mL of water a mixing it with 35.0 mL of 10.0 Mammonia. Ky for ammonia is 1.8x10° a) What is the pH of this buffer solution b) This buffer solution is diluted with water to volume of 100.0 mL and 5.00 mL of 0.500 M HCl are added to the 100.0 mL of buffer. What is the expected pH of the buffer solution after the...
1- Suppose 15 mL of 0.50 M ammonium chloride are added to the 40.00 mL of...
1- Suppose 15 mL of 0.50 M ammonium chloride are added to the 40.00 mL of 1.0 M ammonia and 15 mL of water. (A) Blank # 1: Calculate the pH of the buffer solution. (B) Blank # 2: Suppose 10.00 mL of 0.10 M NaOH are added to the buffer. Calculate the moles of ammonia remaining in solution. Report your answer using decimal notation (not scientific notation). (C) Blank # 3: Suppose 10.00 mL of 0.10 M NaOH are...
Consider a buffer prepared by mixing 75ml of 0.03640 M ammonia (NH3) solution with 28ml of...
Consider a buffer prepared by mixing 75ml of 0.03640 M ammonia (NH3) solution with 28ml of 0.02454 M ammonium chloride solution (pKb of ammonia is 4.75) 1. What will the pH be? 2. If you add 1 mL of 0.1780 M HCl, what will the new pH be?
Consider a buffer prepared by mixing 75ml of 0.03640 M ammonia (NH3) solution with 28ml of...
Consider a buffer prepared by mixing 75ml of 0.03640 M ammonia (NH3) solution with 28ml of 0.02454 M ammonium chloride solution (pKb of ammonia is 4.75) 5. If you added 1 mL of 0.2550 M NaOH to 103 mL of pure water, what would the pH be?
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of...
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydroiodic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining A buffer solution contains 0.443 M ammonium chloride and 0.314 M ammonia. If 0.0313 moles of potassium hydroxide are added to 225...
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)
A buffer solution contains 0.392 M ammonium chloride and 0.498 M ammonia. If 0.0206 moles of...
A buffer solution contains 0.392 M ammonium chloride and 0.498 M ammonia. If 0.0206 moles of perchloric acid are added to 150 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding perchloric acid)
ANS:. . 4 3-What is the pH of a solution prepared by mixing 50 mL of 0.02 19 M ammonium chloride with 50 mL of 0.02...
ANS:. . 4 3-What is the pH of a solution prepared by mixing 50 mL of 0.02 19 M ammonium chloride with 50 mL of 0.0292 M ammoni Report your answer to three decimal places ANS:. 4- Calculate the pH if you add 1 ml of 0.01 M HCI to the buffer from question #3. Repost you answer to three decimal places. ANS:.. 5-Calculate the pH if you added 1 mL of 0.01 M NaOH to the buffer from question...
3- What is the pH of a solution prepared by mixing 50 mL of 0.0219 M ammonium chloride with 50 mL of 0.0292 M ammonia? Report your answer to three decimal places. ANS:.. . .. . ......... ... ... ..... ..... 4- Calculate the pH if you add 1 ml of 0.01 M HCl to the buffer from question #3. Repost you answer to three decimal places. ANS:.. . . ... 5- Calculate the pH if you added 1 mL...
4) A buffer solution is prepared by dissolving 5.40 g of ammonium chloride in 20.0 mL of water a mixing it with 35.0 mL of 10.0 Mammonia. Ky for ammonia is 1.8x10° a) What is the pH of this buffer solution b) This buffer solution is diluted with water to volume of 100.0 mL and 5.00 mL of 0.500 M HCl are added to the 100.0 mL of buffer. What is the expected pH of the buffer solution after the...
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydroiodic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining A buffer solution contains 0.443 M ammonium chloride and 0.314 M ammonia. If 0.0313 moles of potassium hydroxide are added to 225...
ANS:. . 4 3-What is the pH of a solution prepared by mixing 50 mL of 0.02 19 M ammonium chloride with 50 mL of 0.0292 M ammoni Report your answer to three decimal places ANS:. 4- Calculate the pH if you add 1 ml of 0.01 M HCI to the buffer from question #3. Repost you answer to three decimal places. ANS:.. 5-Calculate the pH if you added 1 mL of 0.01 M NaOH to the buffer from question...
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