anyone can help me with it...? biochemistry
(A) pH = 3.86 + log 0.050/ 0.010=4.56
(B)
moles H+ added = 5 x 10^-3 L x 0.5 M=0.0025
moles lactic acid = 0.010 + 0.0025=0.0125
moles lactate = 0.050 - 0.0025 = 0.0474
pH = 3.86 + log 0.0474/ 0.0125 =4.44
change = 4.56 - 4.44 =0.12
(C)
pH water = 7.0
Total volume = 1005 mL = 1.005 L
[H+]= 0.0025/ 1.005=0.00249 M
pH = 2.6
change = 7.0 - 2.6 =4.4
anyone can help me with it...? biochemistry 2. A buffer contains 0.01 mole of lactic acid...
A buffer contains 0.010 mol of lactic acid (pKa = 3.86) and 0.050 mol of sodium lactate per liter. (a) Calculate the pH of the buffer. (b) Calculate the change in pH when 5.0 mL of 0.50 M HCl is added to 1.0 L of the buffer. (c) What pH change would you expect if you added the same quantity of HCl to 1.0 L of pure water?
A buffer contains 0.020 mol of lactic acid (pKa = 3.86) and 0.100 mol sodium lactate per liter of aqueous solution. a. Calculate the pH of this buffer. b. Calculate the pH after 8.0 mL of 1.00 M NaOH is added to 1 liter of the buffer (assume the total volume will be 1008 mL).
2.) Consider a 1.00L of buffer that is 0.139M in lactic acid (C3H5O3H) and 0.134M in sodium lactate (C3H5O3- Na+). Calculate the pH of the buffer after adding 0.0500 mol of HCl into the buffer solution. (Assume no volume change) pKa of lactic acid is 3.86
Calculate the pH of a buffer solution prepared by mixing 75 mL of 1.0 M lactic acid and 25 mL of a 1.0M sodium lactate. (pka of lactic acid = 3.86) Calculate the change in pH that occurs when 0.01moles of OH are added to a 1L buffered solution that contains 0.5M acetic acid (HC_2H_3O_2) and 0.5M acetate ion (C_2H_3O_2). Acetic acid pka = 4.76.
A buffer contains 0.010 mol of lactic acid and 0.050 mol of sodium lactate per liter. (a) calculate the pH of the buffer. (b) calculate the pH when 100ml of 0.02 M NaOH is added to 500mL of the buffer. (c) What pH would you expect if you added the same quantity of NaOH to 500mL of pure water?
4. What molar ratio of HPO4 2-to H2PO4-in solution would produce a pH of 7.0? Phosphoric acid (H3PO4), a triprotic acid, has 3 pKa values: 2.14, 6.86, and 12.4. Hint: Only one of the pKa values is relevant here. 5. For a weak acid with a pKaof 6.0, calculate the ratio of conjugate base to acid at a pH of 5.0. 6. Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa 3.8), acetic acid...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
3. One liter of buffer solution was prepared by mixing 0.1 mole of acetic acid CH3COOH and 0.05 mole of sodium acetate CH3COONa. Calculate a. pH of that solution b. How much of a strong base, say NaOH, in mol/L needs to be added to that solution to change its pH to 6.0? Notes and useful data: For acetic acid pK4.75 For carbonic acid pKa 6.3 and pKa 10.3 Sodium acetate CH3COONa dissociates entirely to Na'CH3COO
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Data Sheet Titration and Buffers Name Date Part One: Buffer Solution (record the results from the video) Lab Section Number of Drops of HCl added to "water": Color changed from to Number of Drops of HCl added to "buffer": Color changed from to to Number of Drops of NaOH added to "water": Number of Drops of NaOH added to "buffer": _Color changed from Color changed from to Part Two: Titration Results for Acid-Base Neutralization (record the results from the...
Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and bate components of the buffer. A 0.5 M buffer can "absorb" five time as much acid or lease as a 0.1 M buffer tor a given pH change. In this problem you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity...