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Lorico [155]
3 years ago
14

A 1 liter solution contains 0.304 M acetic acid and 0.228 M sodium acetate. Addition of 0.114 moles of perchloric acid will:____

___ (Assume that the volume does not change upon the addition of perchloric acid.)
Raise the pH slightly
Lower the pH slightly
Raise the pH by several units
Lower the pH by several units
Not change the pH
Exceed the buffer capacity
Chemistry
1 answer:
Papessa [141]3 years ago
5 0

Answer:

Lower the pH slightly

Explanation:

A buffer is defined as the mixture between weak acid and conjugate base. In the problem, acetic acid is the weak acid and sodium acetate the conjugate base.

When a strong acid as perchloric acid is added to a buffer, <em>the pH decreases slightly</em> because the acid reacts with conjugate base producing weak acid and not affecting directly the concentration of H⁺ ions.

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natita [175]

Explanation:

Equation of the reaction:

Br2(l) + Cl2(g) --> 2BrCl(g)

The enthalpy change for this reaction will be equal to twice the standard enthalpy change of formation for bromine monochloride, BrCl.

The standard enthalpy change of formation for a compound,

ΔH°f, is the change in enthalpy when one mole of that compound is formed from its constituent elements in their standard state at a pressure of 1 atm.

This means that the standard enthalpy change of formation will correspond to the change in enthalpy associated with this reaction

1/2Br2(g) + 1/2Cl2(g) → BrCl(g)

Here, ΔH°rxn = ΔH°f

This means that the enthalpy change for this reaction will be twice the value of ΔH°f = 2 moles BrCl

Using Hess' law,

ΔH°f = total energy of reactant - total energy of product

= (1/2 * (+112) + 1/2 * (+121)) - 14.7

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ΔH°rxn = 101.8 kJ/mol.

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4 years ago
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Explanation:

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scoray [572]

Answer:

C. Hydrogen Ions.

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