A buffer is formed by adding 1.0 mol of trimethylamine, (CH3),N, and 1.0 mol of trimethylammonium, (CH3)aNH, in a 1.0 L container. If a 10.0 mL sample of this buffer is diluted to 1000 mL with water, what is the pH of the diluted buffer? For trimethylamine, K, = 6.4 x 105 Insert your answer in decimal notation rounded to 2 decimal digits. Answer: Enter Value

A buffer is formed by adding 1.0 mol of trimethylamine, (CH3),N, and 1.0 mol of trimethylammonium, (CH3)aNH, in a 1.0 L container. If a 10.0 mL sample of this buffer is diluted to 1000 mL with water, what is the pH of the diluted buffer? For trimethylamine, K, = 6.4 x 105 Insert your answer in decimal notation rounded to 2 decimal digits. Answer: Enter Value

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A research wishes to prepare a buffer with a pH of 4.74 from weak acid HA (Ka = 2.57 x 105) and the sodium salt, NaA (molar mass = 146.6 g/mol). How many grams of NaA must be added to 500. mL of a 0.188 M solution of HA to prepare the buffer solution? Assume no change in volume with the addition of the NaA. Report your answer to two decimal places.
What is the pH of a buffer solution that is 0.21 M methylamine and 0.20 M methylammonium chloride? K, (methylamine) = 4.4 × 10-4
If you have a solution with 1 mole of acetic acid HC2H3O2, which of the following can be added to make a buffer? Choose all correct answers. 1 mol HCl 0.6 mol HCl 1 mol NaC2H3O2 0.5 mol KC2H3O2 1 mol NaOH 0.4 mol NaOH
Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid (HAc). Ka for HAc is1.8x10 -5. How much NaOH must be added to reach the equivalence point, and what is the pH at the equivalence point?
Let’s build a buffer using hypobromous acid (HBrO, Ka = 2.3×10−9) and hypobromite ion (BrO−). If [HBrO] is 0.100 M, then what concentration of hypobromite ion is needed to achieve pH = 8.50
You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?
You need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.71 M NH4Cl solution, what concentration of NH3 l will you need to also start with? (Kb for NH3 is 1.8x10-5)
Calculate the pH of a buffer solution containing 0.584 mol HA weak acid and 0.703 mol A- in 130.1 mL after 0.158 g of NaOH was added? [Ka= 1.56 ×10-5] Report your answer with three decimals. Enter numbers only; do not enter units.
What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4Cl) in enough water to form 2.50L of solution. The K, of ammonia is 1.76 x 10-5. How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBr is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H5O3, should be added to 1.00L of 0.150M lactic acid, HC3H₂O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. K. of lactic acid is 1.40 x 10-4.
What is the pH of a buffer solution that is 0.602 M in hydrofluoric acid and is 0.455 M is potassium fluoride? The K₂ of hydrofluoric acid is 6.4 x 10-4. (Two decimal places)
An aqueous solution contains 0.496 M hydrocyanic acid. How many mL of 0.250 M potassium hydroxide would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 9.230? mL
4. Consider a buffer made by adding 0.050 mol NaC2H302 and 0.040 mol HC2H3O2 to a liter of water. a) What is the pH of this buffer? b) What is the pH after addition of 0.010 mol NaOH? c) What is the pH after addition of 0.010 mol HCI to the original buffer solution?