2. i. Find the pH of a solution pre the pH of a solution prepared by adding 15.0 g of tris to 6.05 g of this hydroc...
What is the ph of the of a buffer solution by adding 15.0 g of ammonium chloride to 5 L of 0.20 M ammonia= answer is 9.8 but i need help with what is the ph of the buffer after 90.0mL of 2.00M HCL are added answer is 9.50 help? what is the ph of the buffer after 15.00 g of naoh are added? answer is 12.28
Find the pH of a formic acid solution that was is prepared by adding 0.280 g of formic acid to a volumetric flask and bringing the final volume to 1.44 L by adding water
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
In order to prepare pH = 7.00 of 1.00 L buffer solution, you added 12.43 g tris (MW: 121.135), calculate the mass in g of tris hydrochloride (MW: 157.596) that you will need to add. pKa = 8.072. Show your calculation process.
A buffer solution was prepared by adding 4.72 g of sodium acetate, NaCH, CO2, to 2.50 10 mL of 0.100 M acetic acid, CH3CO,H (K, = 1.8 x 10-6). a What is the pH of the buffer? pH = 5.10 Correct Find the pH using the Henderson-Hasselbalch equation: 4.72 g 1 mol NaCH, CO2 CH,CO2- ] = [NaCH,CO2] = 0.250 L -= 0.230 M 82.03 g [CH, CO2- pH = pK,+ logo = -log(1.8 x 10-5) + log CH, CO2H]...
TReferencer A solution is prepared by adding 49.9 ml concentrated hydrochloric acid and 19.7 ml concentrated nitric acid to 300 ml water More water is added until the final volume is 1.00 L. Calculate H".COH)and the pH for this solution. (Hint: Concentrated HCl is 38% HCI (by mass) and has a density of 1.19 g ml., concentrated HNO, is 70% HNO, (by mass) and has a density of 1.42 g/mL.] OH")= M pH-
1. Calculate the molarity a solution prepared by adding 14.0 g of sodium sulfate to enough water to make 250.00 mL. 1.182 M O 0.471 M 0.0561 M 0.0986 M 0.394 M Taking Pool 6 1. What volume of 0.250 M HCl is required to react with 0.500 moles of calcium hydroxide? 2.00 L 0.500 L 0.250 L O 1.00 L 4.00 L
9. A solution is prepared by adding 15.8 g of HCl to enough water to make a total volume of 400. mL. What is the pH of the solution? How much hydrogen is contributed by autoionization of water?
What is the pH of a solution prepared by adding 1.59 g of sodium nitrite to 195 mL of water? Ka of HNO2 is 4.5 x 10-4.
What is the pH of a buffer that was prepared by adding 3.96 g of sodium benzoate, NaC7H5O2, to 1.00 L of 0.0100 M benzoic acid, HC7H5O2? Assume that there is no change in volume. The K a for benzoic acid is 6.3 × 10–5.