Methyl acetate, CH 3 COOCH 3 , reacts in basic solution to give acetate ion, CH 3 COO − , and methanol, CH 3 OH. CH 3 COOCH 3 ( a q ) + OH − ( a q ) → CH 3 COO − ( a q ) + CH 3 OH ( a q ) The overall order of the reaction was determined by starting with methyl acetate and hydroxide ion at the same concentrations, so [CH 3 COOCH 3 ] = [OH − ] = x . Then Rate = k [ CH 3 COOCH 3 ] m [ OH − ] n = k x m + n Determine the overall order and the value of the rate constant by plotting the following data assuming first- and then second-order kinetics. Time (min) [CH 3 COOCH 3 ] (mol/L) 0.00 0.01000 3.00 0.00740 4.00 0.00683 5.00 0.00634 10.00 0.00463 20.00 0.00304 30.00 0.00224
Methyl acetate, CH 3 COOCH 3 , reacts in basic solution to give acetate ion, CH 3 COO − , and methanol, CH 3 OH. CH 3 COOCH 3 ( a q ) + OH − ( a q ) → CH 3 COO − ( a q ) + CH 3 OH ( a q ) The overall order of the reaction was determined by starting with methyl acetate and hydroxide ion at the same concentrations, so [CH 3 COOCH 3 ] = [OH − ] = x . Then Rate = k [ CH 3 COOCH 3 ] m [ OH − ] n = k x m + n Determine the overall order and the value of the rate constant by plotting the following data assuming first- and then second-order kinetics. Time (min) [CH 3 COOCH 3 ] (mol/L) 0.00 0.01000 3.00 0.00740 4.00 0.00683 5.00 0.00634 10.00 0.00463 20.00 0.00304 30.00 0.00224
Solution Summary: The author explains that the order of the reaction is second-order, and the rate constant is 135 .
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Methyl acetate, CH3COOCH3, reacts in basic solution to give acetate ion, CH3COO−, and methanol, CH3OH.
CH
3
COOCH
3
(
a
q
)
+
OH
−
(
a
q
)
→
CH
3
COO
−
(
a
q
)
+
CH
3
OH
(
a
q
)
The overall order of the reaction was determined by starting with methyl acetate and hydroxide ion at the same concentrations, so [CH3COOCH3] = [OH−] = x. Then
Rate
=
k
[
CH
3
COOCH
3
]
m
[
OH
−
]
n
=
k
x
m
+
n
Determine the overall order and the value of the rate constant by plotting the following data assuming first- and then second-order kinetics.
Predict whether aqueous solutions of the following substances are acidic, basic, or neutral and write hydrolysis equations for the acidic and basic solutions.
(a) CsBr; (b) Al(NO3)3; (c) KCN; (d) CH3NH3Cl
For the following acid-base reaction, (1) predict the products, showing both reactants and products
complete Lewis structures and arrows showing electron flow; (2) label each structure with the
lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a
ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer.
HC0OH + CH3 Nta
PRん106Y
pkb = 3.36
9)
a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs.
HCO; + H;O* H¿CO; + H2O (aqueous solution)
b) Phenol (HC&H50) is a weak acid (Ka= 1.5 x 10*). Write the equilibrium chemical equation,
equilibrium constant expression, and calculate the pH of a 0.25 M solution of phenol.
10)
Blood is mainly buffered by HCO; /H2CO; (H2CO3, Carbonic Acid, K= 4.4x10 -") buffer system.
Calculate the pH of human blood for a carbonic acid concentration of 0.091M and HCO;
concentration of 1.00M.
Chapter 13 Solutions
General Chemistry - Standalone book (MindTap Course List)
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