Molarity - Fundamentals of Chemistry - page 313

General Problems

11.63 Calculate the concentration of each type of ion in solu-
tion after 37.22 mL of 1.000 M HCl is added to 19.29 mL
of 4.107 M NaOH. Use a net ionic equation in solving
this problem. Assume that the final volume is equal to
the sum of the volumes of the two original solutions.
11.64 Calculate the number of milligrams of

11.76 The label has fallen off a bottle of a solid organic acid. If
26.2 mL of 2.00 M NaOH is needed to completely neu-
tralize 2.36 g of the acid, determine if the acid is oxalic
acid (H 2 C 2 O 4 ), benzoic acid (HC 7 H 5 O 2 ), or bromoben-

zoic acid
11.77 Calculate the acetic acid concentration and the acetate
ion concentration (a) after 0.150 mol of acetic acid and
0.100 mol of sodium acetate are dissolved in enough wa-
ter to make 1.00 L of solution and (b) after 0.250 mol of
acetic acid and 0.100 mol of sodium hydroxide are dis-
solved in enough water to make 1.00 L of solution.
11.78 Calculate the hydrogen ion concentration and the chloride
ion concentration (a) after 0.150 mol of hydrochloric acid
and 0.100 mol of sodium chloride are dissolved in enough
water to make 1.00 L of solution, (b) after 0.250 mol of
hydrochloric acid and 0.100 mol of sodium hydroxide are
dissolved in enough water to make 1.00 L of solution and
(c) compare your results to those of Problem 11.77.
11.79 Calculate the concentration of each ion in solution after
94.3 mL of 2.14 M is mixed with 82.8 mL of
0.700 M and then diluted to 500.0 mL.
11.80 When lithium nitride is treated with water, it reacts with the
water to form hydroxide ions and ammonia. What concen-
tration of hydroxide ions is present if 0.110 mol of solid
is treated with water and then diluted to 100.0 mL?
11.81 Calculate the percentage of in a 5.000-g sample
of limestone if 24.24 mL of 2.500 M HCl is required to
react completely with the

(HC 7 H 4 O 2 Br).

Na 2 CO 3 in 725 mL

of 715 mM solution.
11.65 Calculate the concentration of ion produced when
is bubbled into 0.300 M solution, causing pre-
cipitation of all the copper(II) ion as CuS. Assume no
change in the volume of the solution.

H

Cu 2

H 2 S

Cu 2 (aq) H 2 S(g) £ CuS(s) 2 H (aq)

11.66 Calculate the concentration of acetic acid produced by
reaction in 1.00 L of solution of
(a)
(b)
11.67 Calculate the concentration of each ion in solution after
47.33 mL of 1.807 M NaOH is mixed with 39.19 mL of
0.5093 M and then diluted to 100.0 mL.
11.68 Calculate the concentration of formaldehyde

2.0 mol KC 2 H 3 O 2 (aq) 1.0 mol HCl(aq)

3.0 mol KC 2 H 3 O 2 (aq) 2.0 mol HCl(aq)

MgCl 2

H 2 SO 4 AlCl 3

(CH 2 O) in

a solution prepared by mixing 125 mL of 6.13 M
and 175 mL of 4.34 M

CH 2 O

CH 2 O and diluting the mixture to

Li 3 N

500.0 mL with water.
11.69 Calculate the concentration of in a solution prepared
by mixing 1.25 L of 3.00 M and 719 mL of 1.75 M
and diluting the mixture to 2.50 L with water.
11.70 If 5.033 g of potassium hydrogen phthalate, an acid salt
having one ionizable hydrogen atom and a molar mass of
204.2 g/mol, is used to neutralize 39.17 mL of NaOH so-
lution, calculate the concentration of the base.
11.71 Calculate the concentration of each ion in solution after
30.8 mL of 4.65 M NaOH is mixed with 21.9 mL of
0.750 M and then diluted to 100.0 mL.
11.72 Calculate the sodium ion concentration after 20.0 mL of
3.00 M NaOH is mixed with 30.0 mL of 1.00 M HCl and
diluted to 100.0 mL.
11.73 Calculate the final sugar concentration after 2.25 L of
3.00 M sugar solution is diluted to 5.00 L with (a) water
and (b) 1.00 M NaCl solution.
11.74 Vinegar contains several acids. Calculate the total con-
centration of acids in a 20.0-mL sample of vinegar if it
takes 37.88 mL of 0.2000 M NaOH to neutralize the
acids. Assume that each acid contains only one ionizable
hydrogen atom per formula unit.
11.75 Calculate the concentration of each of the ions in solu-
tion with concentrations greater than 0.500 M after
(a) 1.25 M HCl is mixed with an equal volume of 1.25 M
NaCl.
(b) 1.25 M is mixed with an equal volume of
1.25 M NaC 2 H 3 O 2 .

CaCO 3

CH 2 O

CH 2 O

CaCO 3 . Assume that the rest of

CH 2 O

the limestone sample is inert.
11.82 In a certain experiment, 10.00 mL of 1.500 M was
titrated to a certain end point with 27.61 mL of 1.630 M
NaOH. Write the equation for the chemical reaction that
occurred.
11.83 After a 10.0-g sample containing and inert sub-
stances was treated with 32.74 mL of 5.000 M HCl, it
took 4.20 mL of 1.000 M NaOH to neutralize the excess
HCl. Calculate the percent of in the sample.
11.84 After a 10.00-g sample containing and inert
substances was treated with 41.04 mL of 3.000 M HCl, it
took 4.22 mL of 1.000 M NaOH to neutralize the excess
HCl. Calculate the percent of in the sample.
11.85 When an alkali metal oxide is treated with water, it reacts
with the water to form hydroxide ions. What concentra-
tion of hydroxide ions is present if 0.250 mol of solid
is treated with water and the final volume is
500.0 mL?
11.86 In a certain experiment, 25.00 mL of 2.500 M
was titrated to a certain end point with 39.66 mL of
3.152 M NaOH. Write the equation for the chemical re-
action that occurred.
11.87 What volume of 3.152 M NaOH would be required
to completely neutralize the

H 3 PO 4

Na 2 CO 3

H 3 PO 4

Na 2 CO 3

Na 2 CO 3

Na 2 CO 3

Li 2 O

H 3 PO 4

HC 2 H 3 O 2 H 3 PO 4 in the previous

problem.