Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.15 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.15 M...
6. b) A student mixes 8.203 g of NaC,H,O, with 100 mL of 1.0 M HC,H,O2, what is the pH of the buffer? (4 pts) Wall Co, Hº 3) NaHCO₃ H2O H₂CO NOCH ka 2.22x /у- PO4-р 2.22x 100 = [071%.1 [ot] =4,7x10-S 14 Potter pOH = -log[ott 14-4.32-1 OH = 4,32 (pH=9.631 222 x 10 8 b) If you add 5.0 mL of 0.5 M NaOH solution to 20.0 ml to the buffer above, what is the pH of...
4. Your laboratory supervisor has created a buffer by adding 25.0 g HC,H,O, and 30.0 g of NaC,H,O, to enough water to form a 250 mL solution. The K of HC,H,O, is 6.76 x 104 The laboratory supervisor then instructs you to determine the pH of the buffer. (1 point for the correct molarity of HC,H,O, one point for the correct molarity of NaC,H,Og, and one point for the correct pH)
For 300.0 mL of a buffer solution that is 0.325 M in CH3CH2NH2 and 0.300 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.005 mol of NaOH.
A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of the buffer?
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?...
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂ with 0.100 M Sr(OH)₂ after 100.0 mL of the strong base has been added. The value of Ka for HC₄H₇O₂ is 1.5 × 10⁻⁵. HC4H7O2 (aq) + OH- --> H2O (l) +C4H7O2-
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCI must be added to this buffer solution to change the pH by 0.40 units? Assume the total volume remains unchanged at 400 mL. For H2PO4, K = 6.3 x 10-8 0.013 mol 0.25 mol (Your answer) 0.50 mol 0.057 mol (Correct answer) 0.031 mol
QUESTION #1 What is the pH of a buffer by mixing 1.00L of 0.020M benzoic acid, HC,H,O2, with 3.00L of 0.060M sodium benzoate, NaC HO2? Ka for benzoic acid is 6.3 x 10-5. Write the reaction of the buffer when acid is added to the system. Write the reaction of the buffer when base is added to the system. QUESTION #1 What is the pH of a buffer by mixing 1.00L of 0.020M benzoic acid, HC,H,O2, with 3.00L of 0.060M...
a) Calculate the pH of 0.500 L of a buffer solution that contains 0.200 M of benzoic acid C6H5CO2H and 0.100 M sodium benzoate NaC6H5CO2. Ka = 6.3 x 10-5. b) Calculate the pH after .10 mL of 1.00 M H+ has been added. c) Calculate the pH after 10 mL of 1.00 M OH- has been added.
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...