Exercises 819B 0.25 mole of potassium acetate is added to 0.50 mole of
acetic acid and diluted to 1.00 liter. (a) Which solution is
expected to have the lower pH? (b) Explain how you can
reach your conclusion without calculating the pH of each
solution.
*15.Compare the pH of a 0.15 Macetic acid solution to the
pH of a solution composed of 0.15 Macetic acid to which
0.15 mole of sodium acetate per liter has been added.
*16.Calculate the mass of sodium acetate that must be added
to one liter of a 0.125 Macetic acid solution to produce a
buffer with the pH of 4.75. Assume that there is no vol-
ume change.
*17.A solution is produced by dissolving 0.075 mole of formic
acid and 0.075 mole of sodium formate in sufficient water
to produce 1.00 L of solution. (a) Calculate the pH of this
buffer solution. (b) Calculate the pH of the solution after
an additional 0.010 mole of sodium formate is dissolved.Buffering Action
*18.Consider the ionization of formic acid, HCOOH.HCOOHH 2 O 34 HCOOH 3 OWhat effect does the addition of sodium formate,
NaHCOO, have on the fraction of formic acid molecules
that undergo ionization in aqueous solution?
*19.Briefly describe why the pH of a buffer solution remains
nearly constant when small amounts of acid or base are
added. Over what pH range do we observe the best buffer-
ing action (nearly constant pH)?
*20.What is the pH of a solution that is 0.10 Min HClO 4 and
0.10 MKClO 4? Is this a buffer solution?
*21.(a) Find the pH of a solution that is 0.50 Min formic acid
and 0.40 Min sodium formate. (b) Find the pH after
0.050 mol HCl has been added to 1.0 liter of the solution.
*22.One liter of 0.400 MNH 3 solution also contains 12.78 g
of NH 4 Cl. How much will the pH of this solution change
if 0.142 mole of gaseous HCl is bubbled into it?
*23.(a) Find the pH of a solution that is 0.12 Min nitrous
acid and 0.15 Min sodium nitrite. (b) Find the pH after
0.15 mol of NaOH has been added to 1.0 liter of the
solution.
*24.(a) Find the pH of a solution that is 1.00 Min NH 3 and
0.80 Min NH 4 Cl. (b) Find the pH of the solution after
0.10 mol of HCl has been added to 1.0 liter of the solu-
tion. (c) A solution was prepared by adding NaOH to pure
water to give 1.00 liter of solution whose pH9.34. Find
the pH of this solution after 0.10 mol of HCl has been
added to it.
*25.(a) Calculate the concentrations of CH 3 COOH and
CH 3 COOin a solution in which their total concentra-
tion is 0.200 mol/L and the pH is 4.50. (b) If 0.0100 mol
of solid NaOH is added to 1.00 L of this solution, how
much does the pH change?*26.A solution contains bromoacetic acid, BrCH 2 COOH, and
sodium bromoacetate, NaBrCH 2 COO, with a total con-
centration of 0.30 mol/L. If the pH is 3.10, what are the
concentrations of the acid and the salt? Ka2.0 10 ^3
for BrCH 2 COOH.
*27.Calculate the concentration of propionate ion,
CH 3 CH 2 COO, in equilibrium with 0.020 M
CH 3 CH 2 COOH (propionic acid) and 0.10 MHfrom
hydrochloric acid. Ka1.3 10 ^5 for CH 3 CH 2 COOH.
*28.Calculate the concentration of C 2 H 5 NH 3 in equilibrium
with 0.015 MC 2 H 5 NH 2 (ethylamine) and 0.0010 MOH
ion from sodium hydroxide. Kb4.7 10 ^4 for ethylamine.
*29.When chlorine gas is dissolved in water to make “chlorine
water,” HCl (a strong acid) and HOCl (a weak acid) are
produced in equal amounts.Cl 2 (g)H 2 O()88nHCl(aq)HOCl(aq)What is the concentration of OClion in a solution con-
taining 0.010 mol of each acid in 1.00 L of solution?Preparation of Buffer Solutions
*30.A buffer solution of pH 5.30 is to be prepared from pro-
pionic acid and sodium propionate. The concentration of
sodium propionate must be 0.50 mol/L. What should be
the concentration of the acid? Ka1.3 10 ^5 for
CH 3 CH 2 COOH.
*31.We need a buffer with pH 9.00. It can be prepared from
NH 3 and NH 4 Cl. What must be the [NH 4 ]/[NH 3 ] ratio?
*32.What volumes of 0.150 Macetic acid and 0.100 MNaOH
solutions must be mixed to prepare 1.00 L of a buffer solu-
tion of pH 4.50 at 25°C?
*33.One liter of a buffer solution is prepared by dissolving
0.150 mol of NaNO 2 and 0.070 mol of HCl in water. What
is the pH of this solution? If the solution is diluted twofold
with water, what is the pH?
*34.One liter of a buffer solution is made by mixing 500. mL
of 1.25 Macetic acid and 500. mL of 0.500 Mcalcium
acetate. What is the concentration of each of the follow-
ing in the buffer solution? (a) CH 3 COOH; (b) Ca^2 ;
(c) CH 3 COO; (d) H. (e) What is the pH?
*35.What must be the concentration of benzoate ion,
C 6 H 5 COO, in a 0.045 Mbenzoic acid, C 6 H 5 COOH,
solution so that the pH is 5.00?
*36.What must be the concentration of chloroacetic acid,
ClCH 2 COOH, in a 0.015 MNaCH 2 ClCOO solution so
that the pH is 3.00? Ka1.4 10 ^3 for ClCH 2 COOH.
*37.What must be the concentration of NH 4 in a 0.075 M
NH 3 solution so that the pH is 8.80?Acid–Base Indicators
*38.(a) What are acid–base indicators? (b) What are the essen-
tial characteristics of acid–base indicators? (c) What