A solution is prepared by dissolving 0.23 mol of chloroacetic acid and 0.27 mol of sodium chloroacetate in water sufficient to y
ield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the _______ present in the buffer solution. The 
of chloroacetic acid is 1.36 x 10⁻³.
a. H₂O
b. Na⁺
c. chloroacetate ion
d. chloroacetic acid
e. This is a buffer solution: the pH does not change upon addition of acid or base.
a. H₂O
b. Na⁺
c. chloroacetate ion
d. chloroacetic acid
e. This is a buffer solution: the pH does not change upon addition of acid or base.
1 answer:
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The enthalpy change : -196.2 kJ/mol
<h3>Further explanation </h3>The change in enthalpy in the formation of 1 mole of the elements is called enthalpy of formation
The enthalpy of formation measured in standard conditions (25 ° C, 1 atm) is called the standard enthalpy of formation (ΔHf °)
(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)
The value of ° H ° can be calculated from the change in enthalpy of standard formation:
∆H ° rxn = ∑n ∆Hf ° (product) - ∑n ∆Hf ° (reactants)
Reaction
2 H₂O₂(l)-→ 2 H₂O(l) + O₂(g)
∆H ° rxn = 2. ∆Hf ° H₂O - 2. ∆Hf °H₂O₂