Caproic acid, HC g H 11 O 2 , found in small amounts in coconut and palm oils, is used in making artificial flavors. A saturated aqueous solution of the acid contains 11 g/L and has pH=2.94. Calculate K g for the acid. HC 6 H 11 O 2 +H 2 O ⇌ H 3 O+C 6 H 11 O 2 - − K a =?
Caproic acid, HC g H 11 O 2 , found in small amounts in coconut and palm oils, is used in making artificial flavors. A saturated aqueous solution of the acid contains 11 g/L and has pH=2.94. Calculate K g for the acid. HC 6 H 11 O 2 +H 2 O ⇌ H 3 O+C 6 H 11 O 2 - − K a =?
Solution Summary: The author explains that the pH and concentration of the saturated aqueous solution of caproic acid is 2.94 and 11 g/L respectively.
Caproic acid,
HC
g
H
11
O
2
, found in small amounts in coconut and palm oils, is used in making artificial flavors. A saturated aqueous solution of the acid contains 11 g/L and has pH=2.94. Calculate
K
g
for the acid.
HC
6
H
11
O
2
+H
2
O
⇌
H
3
O+C
6
H
11
O
2
-
−
K
a
=?
. The odor of spoiled butter is due in part to butanoic acid (HC4H7O2) which results from the breakdown of the fat in butter. A 0.100M solution of butanoic acid is 1.23% ionized.
Write the chemical equation for the ionization of this acid in water.
Write the Ka expression for this acid.
What is the equilibrium concentration of each product and the reactant?
1. In each of the equations below, label the acids, bases and their conjugates.
HCOOH
+
H2O
↔
HCOO-
+
H3O+
HPO42-
+
H2O
↔
H2PO4-
+
OH-
NH3
+
H2O
↔
OH-
+
NH4+
2.
Decide which of the following statements are True and which are False about equilibrium systems:
A large value of K means the equilibrium position lies far to the left. For a reaction with K >> 1, the rate of the forward reaction is greater than the rate of the reverse reaction at equilibrium. For the following reaction: H2(g) + F2(g) ⇌ 2HF(g) the values of K and Kp are the same. For the following reaction: CaCO3(s) ⇌ CaO(s) + CO2(g) the [CaCO3] appears in the denominator of the equilibrium expression. The value of K at constant temperature does not depend on the amounts of reactants and products that are mixed together initially.
3.
Given the following equilibrium constants at 427°C:…
1) Vinegar sold commercially is typically 0.8−1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00 M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures?
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