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 HCl. (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
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
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 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...
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...
A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after the addition of 0.20 moles of solid LiOH. Assume no volume change upon the addition of base. The K a for HF is 3.5 × 10 -4. 3.63 3.46 4.24 2.85 4.41
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...
A buffer is prepared by mixing 75.0 mL of 0.40 M aqueous HF and 25.0 mL of 0.80 M aqueous NaF. At 25oC, Ka = 3.5 x 10-4 for HF. SHOW WORK (a). (4 points) Calculate the pH of the buffer. (b). (4 points) Your instructor accidentally dropped the bottle containing the buffer in part (a) in a bucket of water, that initially contained 4.00 L of water. What is the pH of the resulting solution?