Question

Find the pH and percent dissociation for each of the following aqueous solutions at T = 25. °C.

a) A 0.0150 M solution of HBr, a strong acid.

b) A 0.0150 M solution of hypobromous acid, HOBr, a weak
acid. For this acid, K_{a} = 2.0 x
10^{-9}

Answer #1

a. Find the pH of a 0.100 M solution of a weak
monoprotic acid having Ka= 1.1×10−5.
b.Find the percent dissociation of this solution.
c. Find the pH of a 0.100 M solution of a weak
monoprotic acid having Ka= 1.8×10−3
d. Find the percent
dissociation of this solution.
e.Find the
pH of a 0.100 M solution of a weak monoprotic
acid having Ka= 0.16.
f.Find the percent dissociation of this solution.

Find the pH and fraction of dissociation (α) of a 0.0900 M
solution of a weak acid
HA with Ka = 1.00 x 10-5.

Calculate the pH of each of the following strong acid
solutions.
(a) 0.00809 M HBr
pH = _____
(b) 0.260 g of HNO3 in 36.0 L of solution
pH = _____
(c) 70.0 mL of 8.90 M HBr diluted to 1.80 L
pH = _____
(d) a mixture formed by adding 63.0 mL of 0.00678 M HBr to
84.0 mL of 0.00612 M HNO3
pH = _____

1) Find the pH and fraction of dissociation (α) of the
following:
a) 0.116 M solution of the weak acid HA with Ka = 1.16 ✕ 10−5.
(Assume Kw = 1.01 ✕ 10−14. Enter unrounded values.)
b) 0.900 M solution of the weak base B with
Kb = 9.00 ✕ 10−5. (Assume
Kw = 1.01 ✕ 10−14. Enter unrounded
values.)

Calculate the pH and pOH in each of the following aqueous
solutions. In each case, indicate whether the solution is acidic or
basic. a) [OH-] = 1.33 x 10-8 M b) [OH-] = 1.06 x 10-9 M

For each of the following solutions, calculate the initial pH
and the final pH after adding 0.0150 mol of NaOH.
For 270.0 mL of pure water, calculate the initial pH and the
final pH after adding 0.0150 mol of NaOH.
For 270.0 mL of a buffer solution that is 0.240 M in
HCHO2 and 0.310 M in KCHO2, calculate the initial pH and
the final pH after adding 0.0150 mol of NaOH(Ka=1.8⋅10−4).
For 270.0 mL of a buffer solution that...

Find the pH for the following solutions:
a) A solution that is 0.115 M in HBr and 0.130 M in HCHO2
b) A 0.25 M CH3NH3I solution? (Kb = 4.4 x
10-4 M for CH3NH2)
c) A 0.0180 M solution of HClO2? (Ka = 1.1
x 10-2 M)
d) A 0.0180 M solution of Sr(OH)2
e) A 0.170 M solution
of KOCl? (For HOCl, Ka = 3.5 x 10-8 M)
f) A solution that is 3.00×10−2M in HI and 9.00×10−3M...

Calculate the pH at the equivalence point in titrating 0.093 M
solutions of each of the following with 0.098 M NaOH.
(a) hydrobromic acid (HBr)
pH =
(b) phenol (HC6H5O), Ka =
1.3e-10
pH =
(c) ascorbic acid (HC6H7O6),
Ka = 8e-05
pH =

Calculate the percent dissociation of each of the following
solutions. (a) 0.154 M propanoic acid (HC3H5O2, Ka = 1.3 x10^-5)
(part A solved, 0.92%dissociation) (b) a mixture containing 0.154 M
HC3H5O2 and 0.154 M NaC3H5O2

Determine the pH of each of the following
solutions.
(a) 0.821 M hydrogen peroxide (weak acid with Ka
= 2.4e-12).
(b) 0.306 M boric acid (weak acid with Ka =
5.8e-10).
(c) 0.309 M pyridine (weak base with Kb =
1.7e-09).

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