Consider a buffer composed of the weak acid HA and its conjugate base A?.
Part A
Which pair of concentrations results in the most effective buffer?
Which pair of concentrations results in the most effective buffer?
0.90 M HA; 0.10 M A? | |
0.50 M HA; 0.50 M A? | |
0.10 M HA; 0.10 M A? | |
0.10 M HA; 0.90 M A? |
Consider a buffer composed of the weak acid HA and its conjugate base A?. Part A...
Consider a buffer composed of the weak acid acetic acid (CH3COOH) and the conjugate base sodium acetate (NaCH3COO). Which pair of concentrations results in the most effective buffer (i.e. has the highest buffer capacity)? A. 0.10 M CH3COOH; 0.10 M NaCH3COO B. 0.90 M CH3COOH; 0.10 M NaCH3COO C. 0.10 M CH3COOH; 0.90 M NaCH3COO D. 0.50 M CH3COOH; 0.50 M NaCH3COO
A buffer containing 0.50 M of an acid (HA) and 0.10 M of its conjugate base (A–) has a pH of 10.30. Which of the following solutions will make a buffer with a pH of 11.30? A. A solution with [HA] = 0.25 M and [A–] = 0.10 M. B. A solution with [HA] = 0.50 M and [A–] = 0.50 M. C. A solution with [HA] = 0.10 M and [A–] = 0.50 M. D. A solution with [HA]...
What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.45×10–8), and the conjugate base, A–, after 2.71 mL of 0.135 M HCl solution is added. The initial concentrations of the 142 mL buffer solution are [HA]=0.7 M and [A–]=0.37 M. Enter your value to two (2) decimal places.
What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.58×10–5), and the conjugate base, A–, after 1.83 mL of 0.094 M HCl solution is added. The initial concentrations of the 133 mL buffer solution are [HA]=0.38 M and [A–]=0.67 M. Enter your value to two (2) decimal places.
Which concentration of a weak acid (HA) and its conjugate base (A-) will make a buffer solution whose pH value is equal to its pKa? (HA) = 0.05 M, (A-) = 0.07 M HA = 0.05 M, (A-) = 0.05 M more than one answer is correct HA = 0.05 M, (A-) = 0.01 M
19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If the value of K, for HA is 1.0 x 10-5, what is the pH of the buffer?
a buffer is a solution that has a Weak acid in equlibirum with its conjugate base. So can a buffer solution has a weak base in equlibirum with its conjugate acid? So basically, to create a buffer, you can mix a weak acid with its conj. base OR a weak acid + strong base OR a weak base with a strong acid? Am i Correct?
u lal g uid. 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A . If the value of K, for HA is 1.0 x 10-5, what is the pH of the buffer? ale polution2
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...
A buffer is composed of formic acid and its conjugate base, the formate ion. K for formic acid is 1.8 x 10. a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH