Question

A.) Calculate the pH of the 0.39 M NH3/ 0.73 M NH4Cl buffer system. B.) What...

A.) Calculate the pH of the 0.39 M NH3/ 0.73 M NH4Cl buffer system.

B.) What is the pH after the addition of 20.0mL of 0.075 M NaOH to 80.0mL of the buffer solution?

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
what is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and...
what is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 M NH3 in enough water to make 1.000 L of solution? Kb=1.80 x 10^-5 for NH3. calculate the change in pH after addition of 50.0 mL of 0.15M NaOH.
What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and...
What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12M NH3 in enough water to make 1.000 L of solution? Kb= 1.80 x 10^-5 for NH3. Calculate the change in pH after addition of 50.00 mL of 0.15 NaOH.
b) The pH of a buffer system containing NH3 and NH4Cl is found to be 9.40....
b) The pH of a buffer system containing NH3 and NH4Cl is found to be 9.40. Calculate the ratio NH3/NH4Cl c) Given that the solubility product of PbBr2 is 5.520×10-6 determine the molar solubility of PbBr2 in a 0.139 M KBr solution
1.) A buffer solution contains 0.455 M NH4Cl and 0.295 M NH3 (ammonia). Determine the pH...
1.) A buffer solution contains 0.455 M NH4Cl and 0.295 M NH3 (ammonia). Determine the pH change when 0.085 mol NaOH is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change = 2.) Determine the pH change when 0.044 mol HNO3 is added to 1.00 L of a buffer solution that is 0.462 M in HF and 0.218 M in F-. pH after addition − pH before addition = pH change =
A buffer consists of 0.26 M NH4Cl and 0.36 M NH3. What is the pH of...
A buffer consists of 0.26 M NH4Cl and 0.36 M NH3. What is the pH of the buffer after 0.003 moles of Ca(OH)2 are added to 0.10 L of this buffer solution. Kb for NH3 is 1.8×10‒5.
1.)What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and...
1.)What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25mL of 12 M NH3 in enough water to make 1.00L of solution? Kb=1.80x10-5 for NH3. Calculate the change in pH after addition of 50.0mL of 0.15M NaOH. 2.)What mass of Na2SO4 (molar mass=142.0 g/mol) must be added to 350mL of 0.16M Ag+ to initiate precipitation of Ag2SO4? The Ksp of Ag2SO4 is 1.2x10-5. Assume no volume change occurs upon addition of Na2SO4. 3.)What...
Calculate the pH of 100.0 mL of a buffer that is 0.0500 M NH4Cl and 0.125...
Calculate the pH of 100.0 mL of a buffer that is 0.0500 M NH4Cl and 0.125 M NH3 before and after the addition of 1.00 mL of 5.40 M HNO3. pH before = pH after =
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For...
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. You may want to reference (Pages 648 - 658) Section 16.2 while completing this problem. Part A Calculate the pH of 1.0 L of the original buffer, upon addition of 0.030 mol of solid NaOH. Express the pH to two decimal places.
Calculate the pH of 100 ml of a buffer that is .050 M NH4Cl and .160...
Calculate the pH of 100 ml of a buffer that is .050 M NH4Cl and .160 M NH3 before and after the addition of 1.0 mL of 5.25 M HNO3 Before= 9.75 After?
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For...
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L of the solution, upon addition of 36.00 mL of 1.0 MHCl.