A buffer solution contains 0.21 mol of propionic acid (HC3H5O2) and 0.65 mol of sodium propionate (NaC3H502) in 7.70 L. The K of propionic acid (HC3H5O2) is Ka = 1.3e-05. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.09 mol of NaOH? (assume no volume change) pH =

A buffer solution is created containing 3.25 M acetic acid and 0.550 M sodium acetate. The Ka of acetic acid is 1.77 x 10-5. What is the pH of the solution?

A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.

A chemistry graduate student is given 125. mL of a 0.90M benzoic acid (HC,H,CO2) solution. Benzoic acid is a weak acid with K,=6.3 × 10 °. - 5 What mass of NaC,H,CO, should the student dissolve in the HC,H,CO, solution to turn it into a buffer with pH = 3.97? You may assume that the volume of the solution doesn't change when the NaCH,CO, is dissolved in it. Be sure your answer has a unit symbol, and round it 2. to 2 significant digits. x10

A chemistry graduate student is given 125. mL of a 1.30M dimethylamine ((CH,) NH solution. Dimethylamine is a weak base with K,=5.4 × 10 . What mass of (CH,), NH, Cl should the student dissolve in the (CH,) NH solution to turn it into a buffer with pH =10.80? You may assume that the volume of the solution doesn't change when the (CH, NH, Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 10

A buffer solution contains 0.316 M KHCO3 and 0.357 M K₂CO3. If 0.0170 moles of sodium hydroxide are added to 125 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding sodium hydroxide) pH =

(a) Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate in muscles during intense exercise. A chemist prepares a buffer using 225 mL of 85 M lactic acid (Ka = 1.38 x 10-4) and 435 mL of 0.68 M sodium lactate. What is the pH of the buffer?             What is the pH of the lactate buffer if 0.25 moles of gaseous HCl is added?

A buffer solution consisting of 0.50 mol L-1 acetic acid, CH3COOH and 0.50 mol L-1 sodium acetate, CH3COONa has a pH of 4.74. What will be the pH of the buffer solution if we add 0.020 mol of solid NaOH to 1.0 L of the solution?

Three buffers are prepared with equal concentrations of formic acid and sodium formate (Buffer 1), hydrofluoric acid and sodium fluoride (Buffer 2), and acetic acid and sodium acetate (Buffer 3). Rank the three buffers from highest to lowest pH at which they can buffer a solution (i.e., their buffering pH).(a) 1, 2, 3(b) 3, 2, 1(c) 2, 1, 3(d) 3, 1, 2

A buffer solution contains 0.89 mol of hypoiodous acid (HIO) and 0.57 mol of sodium hypoiodite (NaIO) in 3.40 L.The Ka of hypoiodous acid (HIO) is Ka = 2.3e-11.(a) What is the pH of this buffer?pH =  (b) What is the pH of the buffer after the addition of 0.17 mol of NaOH? (assume no volume change)pH =  (c) What is the pH of the original buffer after the addition of 0.24 mol of HI? (assume no volume change)pH =