Question

Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka for $CH_3COOH$ is $1.8 \times 10^{-5}$. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT The buffer was prepared by dissolving 20.0 g $NaCH_3COO$ into a 500.0 mL solution of 0.150 M of $CH_3COOH$. Assume the volume of the solution does not change. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. $CH_3COOH(aq) + H_2O(l) = H_3O^+(aq) + CH_3COO^-(aq)$ Initial (M) Change (M) Equilibrium (M) RESET 0 20.0 0.150 0.244 0.488 0.678 $+x$ $20.0 + x$ $20.0 - x$ $0.150 + x$ $0.150 - x$ $0.244 + x$ $0.244 - x$ $0.488 + x$ $0.488 - x$ $0.678 + x$ $0.678 - x$ $+

          Determine the pH of a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the pH. The
Ka for $CH_3COOH$ is $1.8 \times 10^{-5}$. Complete Parts 1-3 before submitting your answer.
1
2
3
NEXT
The buffer was prepared by dissolving 20.0 g $NaCH_3COO$ into a 500.0 mL solution of 0.150 M of
$CH_3COOH$. Assume the volume of the solution does not change. Fill in the ICE table with the
appropriate value for each involved species to determine concentrations of all reactants and products.
$CH_3COOH(aq) + H_2O(l) = H_3O^+(aq) + CH_3COO^-(aq)$
Initial (M)
Change (M)
Equilibrium (M)
RESET
0
20.0
0.150
0.244
0.488
0.678
$+x$
$20.0 + x$
$20.0 - x$
$0.150 + x$
$0.150 - x$
$0.244 + x$
$0.244 - x$
$0.488 + x$
$0.488 - x$
$0.678 + x$
$0.678 - x$
$+

Determine the pH of a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the pH. The
Ka for CH3COOH is 1.8 × 10^-5. Complete Parts 1-3 before submitting your answer.
1
2
3
NEXT
The buffer was prepared by dissolving 20.0 g NaCH3COO into a 500.0 mL solution of 0.150 M of
CH3COOH. Assume the volume of the solution does not change. Fill in the ICE table with the
appropriate value for each involved species to determine concentrations of all reactants and products.
CH3COOH(aq) + H2O(l) = H3O^+(aq) + CH3COO^-(aq)
Initial (M)
Change (M)
Equilibrium (M)
RESET
0
20.0
0.150
0.244
0.488
0.678
+x
20.0 + x
20.0 - x
0.150 + x
0.150 - x
0.244 + x
0.244 - x
0.488 + x
0.488 - x
0.678 + x
0.678 - x
+

Added by Michael L.

Question

Please give Ace some feedback