The Ka of lactic acid, HC3H5O3, is 1.4 ✕ 10−4.
(a) Suppose buffer #1 is prepared using 40.0 mL 0.1 M HC3H5O3 and 60.0 mL 0.1 M C3H5O3− to give a final volume of 100.0 mL. What is the pH of this buffer? WebAssign will check your answer for the correct number of significant figures.
4.19 Incorrect: Your answer is incorrect.
(b) Suppose a buffer #2 is prepared using 60.0 mL 0.1 M HC3H5O3 and 40.0 mL 0.1 M C3H5O3− to give a final volume of 100.0 mL. What is the pH of this buffer? WebAssign will check your answer for the correct number of significant figures.
5.37 Incorrect: Your answer is incorrect.
(c) Why is buffer #2 more acidic than buffer #1? It has a higher acid concentration. It has a greater volume of base. It was prepared after buffer #1. It has a greater final volume. Correct: Your answer is correct.
(d) Calculate the pH of each buffer if 0.001 moles of OH − are added to each.
The Ka of lactic acid, HC3H5O3, is 1.4 ✕ 10−4. (a) Suppose buffer #1 is prepared using 40.0 mL 0.1 M HC3H5O3 and 60.0 mL...
You prepared a phosphate buffer solution by mixing 40.0 mL of 0.250 M KH_2PO_4 and 60.0 mL ol 0.450 M K_2HPO_4 solution. (a) What are the molar concentrations of H_2PO_4 and HPO_4^2-, respectively, in the final buffer solution? (b) Calculate the pH of the solution. (c) Write a net ionic equation when a strong acid, such as HCl(aq) is added to the phosphate buffer solution. (d) Calculate the final pH when 0.0060 mol of HCl is added to the buffer...
11a) 1.00 moles of lactic acid (HC3H5O3, Ka = 1.4 x 10-4) and 1.00 moles of sodium lactate (NaC3H5O3) are dissolved in water resulting in a solution with a final volume of 550 mL. What is the pH of the solution after the addition of 0.080 moles of HCI? a. 0.80 b. 1.8 C. 2.8 d. 3.8
4.20) and 40.0 mmol Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of benzoic acid (pKa of benzoate. Calculate the pH of this buffer. pH = What volume of 6.00 M NaOH would be required to increase the pH to 4.93 ? volume: mL
10Consider a buffer prepared by mixing 15 mL of a .300 M lactic acid (Ka= 1.4x10^-4) and 15 mL of .300 M potassium lactate. Calculate the pH. 2) Calculate the pH of a buffer when 15mL of a 0.150 M sodium hydroxide is mixed with 15 mL of a .300 M lactic acid
A buffer made with 100.00 mL of 0.95 M lactic acid (Ka=1.4x10-4) and 200.00 mL of 0.50 M lactate has a final volume of 1.0 L. What is the pH of this buffer?
Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pKa = 4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer. pH = What volume of 5.00 M NaOH would be required to increase the pH to 4.93? volume: 1 volume: mL TOOLS x10
A buffer is prepared by combining 80.0 mL of 0.50M HClO and 40.0 mL of 1.0M NaClO. The Ka of hypochlourous acid is 3.5X10-8. a.) if one adds 0.080 mol of solid KOH to the solution, what will be the new pH? assume no change in volume. b.) If instead, one adds 20.0 mL of 1.0 M HCl to the orginal buffer, what will be the new pH?
4) A solution is prepared by adding 60.0 mL of 0.070 M HCIO, and 40.0 mL of 0.060 M HBr. (a) Calculate the concentrations of all ions in solution. (b) Calculate the pH of this solution. 5.) A solution is neared hvaddin 400 ml of 0.060 M NaOH and 400 ml. of.Aso MCQH
What is the pH of a buffer solution prepared by mixing 30.0 mL of 0.10 M of HOAC and 40.0 mL of a 0.1 M NaOAc Pka of the acid is 4.74
Suppose there is 1 .00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pKa = 4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer pH= | 4.58 What volume of 2.00 M NaOH would be required to increase the pH to 4.93? TOOLS x10