Question 1 (1 point)
12.0 mL of a 0.50 M Na2CO3 solution is added to a large test tube. Enough 0.50 M NaHCO3 solution is added to the test tube to give a final volume of 30.0 mL. What is the pH of the resulting buffer solution? H2CO3 has Ka1 = 4.3×10-7 and Ka2 = 5.6×10-11.
Question 3 (1 point)
A buffer solution is made by adding 15.0 mL of a 0.50 M Na2CO3 solution to 15.0 mL of a 0.50 M NaHCO3 solution in a test tube. 2.8 mL of a 1.0 M HCl solution is added to this buffer solution. What is the final pH of the solution in the test tube?
H2CO3 has Ka1 = 4.3×10-7 and Ka2 = 5.6×10-11.
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Question - 3
Question 1 (1 point) 12.0 mL of a 0.50 M Na2CO3 solution is added to a...
Question 3 (1 point) A buffer solution is made by adding 15.0 mL of a 0.50 M Na2CO3 solution to 15.0 mL of a 0.50 M NaHCO3 solution in a test tube. 2.4 mL of a 1.0 M HCl solution is added to this buffer solution. What is the final pH of the solution in the test tube? H2CO3 has Ka1 = 4.3×10-7 and Ka2 = 5.6×10-11. Question 4 (1 point) A buffer solution is made by adding 10.0 mL...
A buffer solution is made by adding 20.0 mL of a 0.50 M Na2CO3 solution to 10.0 mL of a 0.50 M NaHCO3 solution in a test tube. The pH of this buffer was found to be 10.20. After 2.0 mL of 1.0 M HCl solution is added to this buffer solution, the pH is measured to be 9.95. What is the buffering capacity with respect to a strong acid, βa, of this buffer solution, in units of mol/L per pH unit?...
0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine what volume, in ml, of a 1.00 M NaOH solution should be added to 1.00 L of the acid solution to create a buffer with pH = 3.94. acid base pairs to use: K på, HCO2H/NaHCO2 H2CO3 NaHCO3 H3B03 NaH2B03 NaHCO3/Na2CO3 1.8*10-4 3.74 4.2x10-7 6.38 7.3x10-10 9.14 4.8x10-11 10.32 HCO2H/NaHCO2 H2CO3 NaHCO3 H3B03 NaH2B03 NaHCO3/Na2CO3 ml NaOH
The next three (3) problems deal with the titration of 431 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.7 M KOH. What is the pH of the solution at the 2nd equivalence point? What will the pH of the solution be when 0.2045 L of 1.7 M KOH are added to the 431 mL of 0.501 M carbonic acid? How many mL of the 1.7 M KOH are needed...
To make 1.0 L of buffered solution of a 10.0 pH and a total [ ] of carbonate and hydrocarbonate is 0.10 M, how many grams of Na2CO3 and NaHCO3 are needed? Carbonic acid Ka1 = 4.3 * 10-7 and Ka2 = 5.6 * 10-11
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.
You need 100.00 mL of a buffer at pH 10.50 based on carbonate (H2CO3; ka1 = 4.3 x 10^-7, ka2 = 5.6 x 10^-11). you have available the following materials: solid sodium bicarbonate (84.006 g/mol), 2.000 M HCl, and 2.000 M NaOH and of course di water. To ensure adequate buffering capacity, the buffer component present at lower concentration should be at 0.200 M. provide a recipie indicating volumes of liquids and/or masses of solids for technician to use in...
A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3] = 1.000 M. Determine how much strong acid 1.00M HCI or strong base 1.000 M NaOH must be added to change the pH to 7.40. The step-wise acid dissociation constants for carbonic acid are Ka1= 4.2*10^-7 ; Ka2= 4.8*10^-11.
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×10-7 and Ka2 = 5.6 × 10-11.10)A) 10.44 B) 5.50 C) 4.31 D) 11.00 E) 3.56
Calculate the concentration of all species in a 0.165 M solution of H2CO3 (Ka1 is 4.3×10−7 and Ka2 is 5.6×10−11).