Part (a).
According to the Henderson-Hasselbulch equation:
pH = pKa + Log{(nconjugate base + nadded base)/(nweak acid - nadded base)} ('n' corresponds to moles)
i.e. pH = 3.82 + Log{(0.4*0.5 + 0.025)/(0.2*0.5 - 0.025)}
Therefore, pH = 4.3
Part (b).
According to the Henderson-Hasselbulch equation:
pH = pKa + Log{(nconjugate base - nadded acid)/(nweak acid + nadded acid)} ('n' corresponds to moles)
i.e. pH = 3.82 + Log{(0.4*0.5 - 0.05)/(0.2*0.5 + 0.05)}
Therefore, pH = 3.82
28. A 0.50 L buffer solution is 0.20 M in HF and 0.40 M in NaF. The Ka for HF is 1.5 x 10". Show all work for full credit. (a) Calculate the pH of the solution after the addition of 0.025 moles of solid KOH. (3 pts)
28. A 0.50 L buffer solution is 0.20 M in HF and 0.40 M in NaF. The Ka for HF is 1.5 x 10*. Show all work for full credit. (a) Calculate the pH of the solution after the addition of 0.025 moles of solid KOH. (3 pts) (b) Calculate the pH of the solution after the addition of 0.050 moles of HCI. (3 pts)
5) A 1 L buffer solution is 0.520 M in HF and 0.520 M in NaF. Calculate the pH of the solution after adding 0.220 moles of NaOH. Assume no volume change upon the addition of a base. Ka for HF is 3.5 X 10-4
A 1.50 L buffer solution is 0.250 M in HF and0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition. The K_a for HF is 3.5 times 10^-4. 3.63 3.57 3.34 3.46 4.37 Which of the following conjugate pairs would be best for preparing a buffer solution at pH 4.0? HCN K_a = 6.2 times 10^-10 HNO_2 K_a = 7.1 times 10^-4 NaCI and...
37. You have 500.0 mL of a buffer solution that is 0.30 M HF and 0.50 M KF. Ka for HF is 7.1 x 10-4 a) Calculate the pH of the buffer. b) Calculate the pH of the buffer after adding 0.020 moles of HCI. c) Calculate the pH of the buffer after adding 0.030 moles KOH. - -Loel.
A buffer solution contains 1.0 M HF and 1.0 M NaF. The ka for HF is 7.2x10-5. 0.10 moles of HCl are added to 1 liter of the buffer. The pH of the resulting solution is a) 4.05 b) 4.14 c) 4.23 d) 4.74
Consider 1.0 L of a solution which is 0.80 M HF and 0.55 M NaF (K for HF - 7.2x104). Part 1 Calculate the pH of this solution. pH- Part 2 Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCI. pH- Part 3 Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition...
Determine the pH of a solution that is 1.00 L of 0.100 M HF and 0.100 M NaF after 0.50 mole of solid KOH has been added to the solution. Ka(HF) = 3.5×10-4
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 upon addition of 0.050 mol of solid NaOH to the original buffer solution. Thanks!
3. You have been tasked with making a 0.50 L buffer solution with 0.250 M in HF and 0.250 M in NaF so all of your experiments will have a constant pH value. Under no circumstances can your pH leave the range of 3.2-3.7. A clumsy professor, Dr. Urkel, walks by and accidentally spills 0.100 moles of solid NaOH into your solution. Will your buffer be able to withstand the addition and still stay in the range? Calculate the new...