A) How many milliliters of 0.15 M HCl would have to be added to 1.0 L of a buffer containing 0.25 M NH3 and 0.45 M NH4 to make the pH decrease by 0.05 pH unit? The Ka value = 5.6 x 10^-10.
B) How many milliliters of the same HCl solution would, if added to 0.204 L of pure water, make the pH decrease by 0.05 pH unit?
A) How many milliliters of 0.15 M HCl would have to be added to 1.0 L...
How many milliliters of 10.0 M HNO3 solution must be added to a 1.0 L buffer that is .01 M acetic acid ( HC2H3O2) and .2M sodium acetate (NaC2H3O2) to bring the pH to 5.6? the pKa of acetic acid is 4.75
How many milliliters of 0.45 M NaOH must be added to 0.434 L of 0.015 M HCl to give a mixture with a pH of 3.00? mL
How many milliliters of 1.0 M NaOH should be added to a 100 mL solution containing 12.212g of benzoic acid (F.W. 122.12g ; Ka = 6.28 x 10-5) to get a pH of 4.8?
Question 1 a. How many mol of solid LiA would have to be added to 1.0 L of a 4.974 M HA solution in order to obtain a buffer of 2.68? (The Ka for HA is 3.51⋅10^-7). b. Calculate the pH at the equivalence point for the titration of 2.480 M B: (a weak base with pKb = 6.28) with 2.480 M HCl. c. What volume of water must be added to a 10.14 mL solution of a pH =...
How many mL of a 4.00 M HCl solution must be added to 250 mL of a 0.250 M NH3 solution to make a buffer with pH = 9.10? Look up Ka or Kb in a suitable source.
How many grams of sodium acetate, NaC2H3O2, would have to be added to 1.0 L of 0.90 M acetic acid (pKa = 4.74) to make the solution a buffer for pH 4.00?
How many grams of sodium acetate, NaC2H3O2, would have to be added to 1.0 L of 0.30 M acetic acid (pKa = 4.74) to make the solution a buffer for pH 4.00? _____g NaC2H3O2
What volume of 0.200 M HCl must be added to 500.0 mL of 0.250 M NH3 to have a buffer with a pH of 8.81? Ka for NH4+ is 5.6x10-10. Volume =. L
How many milliliters of 12.0 M HCl should be added to 5.00 x 102 mL of 0.100 M Na2SO3 to produce a pH 7.00 buffer solution. For H2SO3 Ka1 = 1.39 x 10-2 and Ka2 = 6.73 x 10-8.
A solution is prepared by adding 20.0 mL of 0.15 M HCl to 80.0 mL of 0.20 M NH3. Ka(NH4+)= 5.8 x 10-10 a. Is this solution a buffer? Why or why not? b. What is the pH of the solution?