Calculate the pH of a buffer that is 0.040 M HF and 0.020 M LIF. The Ka for HF is 3.5 x 10-4.
Calculate the pH of a buffer that is 0.020 M HF and 0.040 M LiF. The K a for HF is 3.5 × 10 -4. 2.76 2.06 3.46 4.86 3.76
Calculate the pH of a buffer that is 0.040 M HF and 0.020M LiF. The Ka for HF is 3.5 x 104
What is the pH of a buffer that is 0.379 M HF and 0.374 M LiF? The Ka for HF is 3.5 x 10-4. If the ΔH = 109 kJ/mol and ΔS = 100 J/K mol, at what temperature does this reaction become spontaneous?
Determine the pH of 1.33 M LiF. For HF, Ka is 6.8 x 10^-4.
A.) Calculate the pH of 0.100 L of a buffer solution that is 0.29M in HF (Ka = 3.5 x 10-4 ) and 0.55M in NaF. B.) What is the pH after adding 0.004mol of HNO3 to the buffer described in Part A? C.) What is the pH after adding 0.002mol of KOH to the buffer described in Part A?
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
Calculate the pH and [H3O+] of a buffer solution consisting of 0.50 M HF (Ka = 6.8 × 10-4) and 0.45 M KF.
help with 5 and 6 please
5. Choose the effective pH range of a HF/Naf buffer. For HF, Ka = 3.5 x 10-4 6. If a small amount of a strong acid is added to buffer made up of a weak acid, HA, and the sodium salt of its conjugate base, NaA, the pH of the buffer solution does not change appreciably because a) the Ka of HA is changed. b) the strong acid reacts with Ato give HA, which...
The Ka value for HF is 3.5×10?4. Part A Calculate the change in pH when 2.0×10?2mol of NaOH is added to 0.50 L of a buffer solution that is 0.15 M in HF and 0.20 M in NaF. Note: can you break it down in steps so i can understand how it was solved? Thanks
Question 1 -- / 1 Calculate the pH of a buffer that is 0.058 mol L-1 HF and 0.058 mol L-1 LiF. The ka for HF is 3.5 x 10-4. 9.31 2 10.54 3 3.46 4 4.69 © 2.86