11.0 M NH3 solution used
You are asked to bring the pH of 0.500 Lof 0.450 M NH4Cl to 7.00.
How many drops (1 drop 0.05 mL) of this solution would you use?
Express your answer as an integer.
11.0 M NH3 solution used You are asked to bring the pH of 0.500 Lof 0.450...
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=
How many grams of dry NH4Cl need to be added to 2.10 L of a 0.500 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.76? Kb for ammonia is 1.8×10−5. Express your answer with the appropriate units.
you are asked to prepare a pH= 9.43 buffer starting from 60.0mL of 0.10M solution of ammonia, NH3, And 0.1M NH4Cl. (Kb for NH3= 1.8x10^-5) How many mL of NH4Cl should be added to prepare buffer solution?
How many grams of dry NH4Cl need to be added to 2.50 L of a 0.500 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.74? Kb for ammonia is 1.8*10^-5.
How many grams of dry NH4Cl need to be added to 1.50 L of a 0.500 M solution of ammonia, NH3,to prepare a buffer solution that has a pH of 8.79? Kb for ammonia is 1.8*10^-5.
(a) How many milliliters of a stock solution of 11.0 M HNO, would you have to use to prepare 500 mL of 0.200 M HNO,? ml (b) If you dilute 21.0 mL of the stock solution from part a) to a final volume of 3.00 L, what will be the concentration of the diluted solution? (Watch the 7. -13 points My (a) How many milliliters of a stock solution of 12.0 M HNO, would you have to use to prepare...
Calculate the pH for 100. mL of a 0.500 M solution of ammonia, (NH3 Kb=1.8x10-5) being titrated with 0.500 M HCl at the following positions in the titration. i) The initial pH (before any HCl has been added). A. 9.44 B. 10.81 C. 11.48 D. 12.00 E. 11.75
A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 27.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 MM CH3COOH (Ka=1.8×10−5Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 15.0 mL of NaOH. and Imagine that you are in chemistry lab and need to make 1.00 LL of a solution with a pH of 2.80. You have in front...
A solution is prepared by mixing 200 ml of 0.1M NH3 and 300 mL of 0.05 NH4Cl. Water is added to bring total solution volume to 750 mL. Kb for nH3 is 1.8x10^-5 please solve, the answer is 9.4 Please do it without the use of Handerson's equation and apply more of an ice table approach. Thank you
A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10?5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 28.0 mL of HNO3. Express your answer numerically.