Question

Calculate the pH at 25 degrees C of 211 mL of a buffer solution that is...

Calculate the pH at 25 degrees C of 211 mL of a buffer solution that is 0.230 M NH4Cl and 0.230 M NH3 before and after the addition of 1.6 mL of 6.0 M HNO3. The pKa for NH4+ is 9.75.

Homework Answers

Answer #1

Before addition:

pH= pKa + log [NH3]/[NH4+]

pH= 9.75 + log 0.23/0.23= 9.75

After addition:

The acid HNO3 will react with NH3 to form NH4+.

mol of acid= 6M x 1.6x10-3L = 9.6x10-3 mol

mol NH4+= mol NH3= 0.23M x 211x10-3L= 0.04853 mol

final mol NH4+= 0.04853 mol + 9.6x10-3 mol= 0.05813 mol

final mol NH3= 0.04853 mol - 9.6x10-3 mol= 0.03893 mol

[NH4+]final= 0.05813mol/212.6x10-3L= 0.273M

[NH3]final= 0.03893mol/212.6x10-3L= 0.183M

pH= 9.75 + log 0.183/0.273= 9.58

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
Calculate the pH at 25°C of 217.0 mL of a buffer solution that is 0.210 M...
Calculate the pH at 25°C of 217.0 mL of a buffer solution that is 0.210 M NH4Cl and 0.210 M NH3 before and after the addition of 1.80 mL of 6.0 M HNO3. (The pKa for NH4+ = 9.75)
Calculate the pH at 25°C of 264.0 mL of a buffer solution that is 0.410 M...
Calculate the pH at 25°C of 264.0 mL of a buffer solution that is 0.410 M NH4Cl and 0.410 M NH3 before and after the addition of 2.60 mL of 6.0 M HNO3. (The pKa for NH4+ = 9.75) Part 1: pH before= Part 2: pH after=
calculate the ph at 25°C of 199mL of a buffer solution that is 0.440M NH4Cl and...
calculate the ph at 25°C of 199mL of a buffer solution that is 0.440M NH4Cl and 0.44M NH3 before and after the addition of 1.5mL of 6.0M HNO3. The pKa for NH4+ is 9.75. please I need the answer asap..... pH after addition is not 9.16
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?
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 =
Calculate the pH of 100.0 mL of a buffer that is 0.070 M NH4Cl and 0.155...
Calculate the pH of 100.0 mL of a buffer that is 0.070 M NH4Cl and 0.155 M NH3 before and after the edition of 1.00 mL of 5.90 M HNO3.
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 solution is prepared by mixing 50.0 mL of 0.300 M NH3(aq) with 50.0 mL...
A buffer solution is prepared by mixing 50.0 mL of 0.300 M NH3(aq) with 50.0 mL of 0.300 M NH4Cl(aq). The pKb of NH3  is 4.74. 7.50 mL of 0.125 M NaOH is added to the 100.0 mL of the original buffer solution prepared in Question 1 (no HCl added). Calculate the new NH3 concentration for the buffer solution. Calculate the new NH4Cl concentration for the buffer solution. Calculate the new pH of the solution.
Solution C is made by mixing 58.7 mL of 0.16 M ammonium chloride (NH4Cl) with 60.1...
Solution C is made by mixing 58.7 mL of 0.16 M ammonium chloride (NH4Cl) with 60.1 mL of 0.26 M ammonia solution. pKa (NH4+) = 9.24 a. Calculate the pH of Solution C. b. Calculate the pH of the buffer Solution C if 0.12 g of NaOH (molar mass = 40.0 g/mol) is added (assuming no change in volume).
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?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT