A 0.60M solution of a hypothetical weak acid (HB) has a pH of 2.80. a.) Write th
ID: 828103 • Letter: A
Question
A 0.60M solution of a hypothetical weak acid (HB) has a pH of 2.80.
a.) Write the chemical equation for the reaction of this acid with water. identify the bronsted acids and bases in the reaction.
b.) Determine the Ka of the this acid.
c.) If 50.0 ml of this weak acid is titrated with 1.00M NaOH, what is the pH after 10.0ml of the base added?
d.) what did the pH of the soultion at the eqivalence point of the titration described in C above ?
e.) A buffer solution is created using 0.15moles of a salt NaB ('B' being the anion of the weak acid HB) and 50.0 ml of 2.0M acid HB ( assume no change in volume ). what would be the pH of that soultion ?
Explanation / Answer
1- HB + H20 ------> H30+ + B-
HB -----> bronsted acid
H30+ --> conjugate acid
H20 ------> bronsted bases
B- -----> conjugate base
2 - pH = 2.80
pH = pKa
=> 2.80 = - log [Ka]
=> Ka = 10 ^-2.80
= 1.58 * 10^-3
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