Lab 5 Aqueous Reactions Onlline
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1
Aqueous Reactions Lab Online
Name: ________________________
Please do not forget to print or type your name out. Thanks
There are many ionic compounds not soluble in water. In this experiment, we will be mixing two aqueous solutions of two different ionic compounds that are soluble in water, and in doing so, a precipitation reaction may take place if one of the cations of one ionic compound forms an ionic compound not soluble in water with the anion of the other ionic compound. For example, both sodium phosphate Na
3
PO
4
and magnesium chloride MgCl
2
are soluble in water. But when one mixes these two aqueous solutions, solid precipitate of magnesium phosphate Mg
3
(PO
4
)
2
will
come out of solution since magnesium phosphate is an ionic compound not soluble in water, and what is left remaining in solution is sodium chloride NaCl or table salt.
2 Na
3
PO
4
(aq) + 3 MgCl
2
(aq) → Mg
3
(PO
4
)
2
(s) + 6 NaCl (aq)
The above chemical reaction shown is the condensed form of this precipitation reaction, which is
also a double replacement reaction. Since this chemical reaction involves only ionic compounds,
and the cations and anions of both compounds separate when dissolved in water, the same reaction shown in complete ionic form bellow.
6 Na
+
(aq) + 2 PO
4
3−
(aq) + 3 Mg
2+
(aq) + 6 Cl
−
(aq) → Mg
3
(PO
4
)
2
(s) + 6 Na
+
(aq) + 6 Cl
−
(aq)
Note that there are two spectator ions in this reaction, which are the sodium cations Na
+
and the chloride anions Cl
−
. Both of these two ions are not taking an active part in the overall chemical reaction. If one subtracts out from both sides of the chemical equations the six sodium cations and six chloride anions, one has the net ionic reaction, the formation of the magnesium phosphate solid precipitating out of an aqueous solution.
3 Mg
2+
(aq) + 2 PO
4
3−
(aq) → Mg
3
(PO
4
)
2
(s)
In addition to precipitation reactions, some chemical reactions involving ionic compounds produce a molecular covalent gas instead of a solid ionic compound not soluble in water. An example of this is the mixing of an aqueous solution of ammonium chloride NH
4
Cl with another aqueous solution of sodium hydroxide NaOH.
NH
4
Cl (aq) + NaOH (aq) → NaCl (aq) + H
2
O (l) + NH
3
(g)
In the complete ionic form, this reaction is the following representation.
NH
4
+
(aq) + Cl
−
(aq) + Na
+
(aq) + OH
−
(aq) → Na
+
(aq) + Cl
−
(aq) + H
2
O (l) + NH
3
(g)
The net ionic reaction is the next representation after removing the two spectator ions Na
+
and Cl
−
, and ammonia gas NH
3
is the gaseous product of this reaction.
NH
4
+
(aq) + OH
−
(aq) → H
2
O (l) + NH
3
(g)
2
In this activity, aqueous solutions of ionic compounds will be mixed together to observe any precipitation taking place, the formation of a gas, or no reaction at all. The reactions are in microscale using plastic well plates. Make sure that the well plate is clean before beginning the experiments. See the Figure 1 below to follow the reaction steps.
5 drops downward into each small well
NaOH HCl Na
3
PO
4
Na
2
CO
3
NaHCO
3
MgCl
2
CaCl
2
FeSO
4
FeCl
3
AgNO
3
Figure 1
The filling of the 24 plastic wells in the downward direction with reactants in solution
For the first column on the left-hand-side going vertically in the downward direction, add five drops of 1 Molar NaOH solution to each of the six wells in the first column. Then, add five drops of 1 Molar HCl downward to each of the six wells in the second column to the left-hand-
side. Afterwards, add five drops of 1 M Na
2
SO
4
downward to each of the six wells in the third column to the left-hand-side. Lastly, repeat the same task by adding five drops of 1 Molar Na
2
CO
3
downward to each of the six wells in the column farthest on the right-hand-side.
Concerning the next step to this experiment, see Figure 2 on the next page. To observe if any gas produced or no reaction at all, go in the horizontal direction and add one to five drops of 1 Molar NaHCO
3
to see if any reaction takes place when mixing NaHCO
3
solution with 1 Molar NaOH, 1 Molar HCl, 1 Molar Na
3
PO
4
, and 1 Molar Na
2
CO
3
in each of the top horizontal four wells, respectively. One of these produces carbon dioxide gas but no reaction in the other three. If a reaction takes place producing carbon dioxide gas in any one of the top four wells, record the
result in the corresponding rectangle in Figure 3 on page 5. Once a reaction observed to take place after only two or three drops added, then it is not necessary to add any more drops of reagent. On the other hand, if no reaction observed, add five drops of reagent to the plastic well going in the horizontal direction.
After adding 1 Molar NaHCO
3
solution in the horizontal direction, then for the second row from the top perform the same tasks by adding 1 Molar MgCl
2
to each of the four horizontal wells and record the results in the second row of rectangles in Figure 3. For this second row, three different
A
B
C
D
1
2
3
4
5
6
3
white ionic compounds not soluble in water precipitate out of solution, and only one cell has no reaction, the HCl cell. Record your results in the corresponding rectangles in Figure 3.
NaOH HCl Na
3
PO
4
Na
2
CO
3
NaHCO
3
MgCl
2
CaCl
2
FeSO
4
FeCl
3
AgNO
3
Figure 2
Adding reactants in solution in the horizontal direction to see if reaction occurs or not
Then carry on the same task by adding 1 Molar CaCl
2
in the horizontal direction of the horizontal
four wells in the third row from the top. For this third row, three different white ionic compounds not soluble in water precipitate out of solution also, and only the HCl cell has no reaction. Again, record results in the corresponding rectangles of Figure 3.
In the next step of this experiment, conduct the same tasks for the four horizontal cells in the fourth row from the top by adding 1 Molar FeSO
4
in the horizontal direction. There will be three
different precipitations of three different green-colored ionic compounds insoluble in water, and only one of these four cells will have no reaction at all, the HCl cell. In the fifth step of this experiment, add one to five drops of 1 M FeCl
3
to each of the four wells in the horizontal direction for the fifth row. Similar to the addition of FeSO
4
, three solid precipitates form, each of the three are different ionic compounds colored red, and again only one of the four cells no reaction occur, the HCl cell as usual. Record results in Figure 3.
For the bottom sixth row from the top, horizontally add one to five drops of 1 Molar AgNO
3
to each of the four wells and record your results in the correct corresponding rectangle of Figure 3. There should be solid precipitate in each of the four wells. One solid will be dark brown, almost black, and the other three will be white. As previously, record results in the corresponding rectangles in Figure 3 on page 5.
If this is an online lab
, use your textbook
, p
ower point projections
, and the Internet
via Google to determine which one of the 24 cells bubbles of carbon dioxide gas occurs, those where
solid precipitates form due to the reaction products that are ionic compounds not soluble in water, or no reaction at all. The top of page 5 gives the instructions on how to record these A
B
C
D
1
2
3
4
5
6
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4
results in 24 rectangles corresponding to the 24 plastic wells. Below is from the power points of a different textbook, which should be useful to figure out which well a solid
compound
forms, due to a precipitation reaction occurring.
Concerning the SO
4
2−
anion, Table 9.7 does not mention the fact that Ag
2
SO
4
is not soluble in water. It also does not mention for the cyanide CN
−
anion that AgCN, Pb(CN)
2
and Hg
2
(CN)
2
are all not soluble in water. In addition to the exceptions of solubility for Cl
−
, Br
−
and I
−
anions, the copper(I) Cu
+
compounds of CuCl, CuBr, and CuI as well as CuCN are insoluble in water.
Obviously compounds as Mg(OH)
2
, Mg
3
(PO
4
)
2
, and MgCO
3
are not soluble in water, because in the above Table, the hydroxide OH
−
, the phosphate PO
4
3−
, and the carbonate CO
3
3−
anions are not
shown. In addition, it should be obvious that Ca(OH)
2
, Ca
3
(PO
4
)
2
,and CaCO
3
are not soluble in water.
Concerning the iron(II) Fe
2+
and iron(III) Fe
3+
cations, Fe(OH)
2
and Fe(OH)
3
are not soluble in water as well as Fe
3
(PO
4
)
2
and FePO
4
and also as well as FeCO
3 and Fe
2
(CO
3
)
2
.
For the silver cation Ag
+
, silver acetate AgC
2
H
3
O
2
is only slightly soluble in water, so it is an exception to the solubility rules given in the above Table stating that all acetates are soluble in water. Most metal hydroxides are insoluble in water, since only the hydroxides soluble in water are the hydroxides of the Group 1A metals (LiOH, NaOH, KOH, RbOH, and CsOH) and the other two hydroxides: thallium(I) hydroxide TlOH and unstable ammonium hydroxide NH
4
OH. The same goes for carbonates (CO
3
2−
) and phosphates (PO
4
3−
). All Group 1A metal carbonates and phosphates are water soluble as well as ammonium carbonate and ammonium phosphate.
Concerning some metal hydroxides, when one tries to synthesize their water insoluble hydroxides, instead one obtains the insoluble oxides of the metal cations instead. A prime example is silver hydroxide AgOH. If one mixes waters soluble AgNO
3
with NaOH, instead of AgOH there is the formation of dark brown solid Ag
2
O, which has the same colors as Ag
2
S when
silver tarnishes due to trace amounts H
2
S gas in the earth’s atmosphere. Even though Ag
+
is a +1
cation as Group 1A metals form in ionic compounds, silver oxide Ag
2
O, silver chloride AgCl, silver phosphate Ag
3
PO
4
, and silver carbonate Ag
2
CO
3
are not soluble in water. Group 1A oxides are the only metal oxide soluble in water, but they all react with water to form the Group 1A metal hydroxides. For example: Na
2
O (aq) + H
2
O (l) → 2 NaOH (aq).
5
Results in Aqueous Reactions.
Name: ___________________________
To see similar experiment go online to https://www.youtube.com/watch?v=DVrfgHMHjS4
Using the “Solubility Rules for Ionic Compounds” on the previous page, Table 9.7 from another Chemistry textbook, or Google search
on the Internet
concerning the rectangles show below, type or write in:
NR
if one thinks there will be no reaction for the two chemicals combined.
Gas
if one thinks that the mixture will have a reaction that produces a gas product such as CO
2
.
Solid
if one thinks that this combination will cause a precipitation of ionic compound not soluble
in water. By Google searching via the Internet, one finds the color of each solid formed.
NaOH (1 M)
HCl (1 M)
Na
3
PO
4 (1 M)
Na
2
CO
3 (1 M)
NaHCO
3 (1 M)
MgCl
2 (1 M)
CaCl
2 (1 M)
FeSO
4
(1 M)
FeCl
3
(1 M)
6
AgNO
3
(1 M)
Figure 3
For recording experimental observations of the chemical reactions that take place
Name: ___________________________
Post Lab Questions
Circle it with pen or pencil, or highlight in yellow for the following multiple-choice questions. Check solubility rules in Table 9.7 on page 4 or Google search on the Internet.
1. The reaction between sodium hydrogen carbonate and hydrochloric acid produces a gas with water and sodium chloride as by-products of the reaction.
NaHCO
3
(aq) + HCl (aq) → NaCl (aq) + H
2
O (l) + Gas
Which one of the following gases is the gas product of this chemical reaction? a) CO
b) CO
2
c) SO
2
d) SO
3
e) NH
3
2. The reaction between sodium hydrogen sulfite and hydrochloric acid produces a gas with water and sodium chloride as by-products of the reaction.
NaHSO
3
(aq) + HCl (aq) → NaCl (aq) + H
2
O (l) + Gas
Which one of the following gases is the gas product of this chemical reaction?
a) CO
b) CO
2
c) SO
2
d) SO
3
e) NH
3
3. The reaction between aqueous solutions of sodium hydroxide and magnesium chloride will produce sodium chloride and an ionic compound not soluble in water.
MgCl
2
(aq) + 2 NaOH (aq) → 2 NaCl (aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) MgCO
3
b) Mg(OH)
2
c) Mg
3
(PO
4
)
2
d) MgO
4. The reaction between aqueous solutions of sodium phosphate and magnesium chloride will produce sodium chloride and an ionic compound not soluble in water.
3 MgCl
2
(aq) + 2 Na
3
PO
4
(aq) → 6 NaCl (aq) + Solid
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7
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) MgCO
3
b) Mg(OH)
2
c) Mg
3
(PO
4
)
2
d) MgO
Name: ___________________________
Post Lab Questions
Circle it with pen or pencil, or highlight in yellow for the following multiple-choice questions. Check solubility rules in Table 9.7 on page 4 or Google search on the Internet.
5. The reaction between aqueous solutions of sodium carbonate and magnesium chloride will produce sodium chloride and an ionic compound not soluble in water.
MgCl
2
(aq) + Na
2
CO
3
(aq) → 2 NaCl (aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) MgCO
3
b) Mg(OH)
2
c) Mg
3
(PO
4
)
2
d) MgO
6. The reaction between aqueous solutions of sodium hydroxide and calcium chloride will produce sodium chloride and an ionic compound not soluble in water.
CaCl
2
(aq) + 2 NaOH (aq) → 2 NaCl (aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) CaCO
3
b) Ca(OH)
2
c) Ca
3
(PO
4
)
2
d) CaO
7. The reaction between aqueous solutions of sodium phosphate and calcium chloride will produce sodium chloride and an ionic compound not soluble in water.
3 CaCl
2
(aq) + 2 Na
3
PO
4
(aq) → 6 NaCl (aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water?
a) CaCO
3
b) Ca(OH)
2
c) Ca
3
(PO
4
)
2
d) CaO
8. The reaction between aqueous solutions of sodium carbonate and calcium chloride will produce sodium chloride and an ionic compound not soluble in water.
8
CaCl
2
(aq) + Na
2
CO
3
(aq) → 2 NaCl (aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) CaCO
3
b) Ca(OH)
2
c) Ca
3
(PO
4
)
2
d) CaO
Name: ___________________________
Post Lab Questions
Circle it with pen or pencil, or highlight in yellow for the following multiple-choice questions. Check solubility rules in Table 9.7 on page 4 or Google search on the Internet.
9. The reaction between aqueous solutions of iron(II) sulfate and sodium hydroxide will produce sodium chloride and an ionic compound not soluble in water.
FeSO
4
(aq) + 2 NaOH (aq) → Na
2
SO
4
(aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) FeCO
3
b) Fe(OH)
2
c) Fe
2
(PO
4
)
3
d) FeO
10. The reaction between aqueous solutions of iron(II) sulfate and sodium phosphate will produce sodium chloride and an ionic compound not soluble in water.
3 FeSO
4
(aq) + 2 Na
3
PO
4
(aq) → 3 Na
2
SO
4
(aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) FeCO
3
b) Fe(OH)
2
c) Fe
3
(PO
4
)
2
d) FeO
11. The reaction between aqueous solutions of iron(II) sulfate and sodium carbonate will produce sodium chloride and an ionic compound not soluble in water.
FeSO
4
(aq) + Na
2
CO
3
(aq) → Na
2
SO
4
(aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) FeCO
3
b) Fe(OH)
2
c) Fe
2
(PO
4
)
3
d) FeO
12. The reaction between aqueous solutions of iron(III) chloride and sodium hydroxide will produce sodium chloride and an ionic compound not soluble in water.
9
FeCl
3
(aq) + 3 NaOH (aq) → 3 NaCl (aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) Fe
2
(CO
3
)
3
b) Fe(OH)
3
c) FePO
4
d) Fe
2
O
3
Name: ___________________________
Post Lab Questions
Circle it with pen or pencil, or highlight in yellow for the following multiple-choice questions. Check solubility rules in Table 9.7 on page 4 or Google search on the Internet.
13. The reaction between aqueous solutions of iron(III) chloride and sodium phosphate will produce sodium chloride and an ionic compound not soluble in water.
FeCl
3
(aq) + Na
3
PO
4
(aq) → 3 NaCl (aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) Fe
2
(CO
3
)
3
b) Fe(OH)
3
c) FePO
4
d) Fe
2
O
3
14. The reaction between aqueous solutions of iron(III) chloride and sodium carbonate will produce sodium chloride and an ionic compound not soluble in water.
2 FeCl
3
(aq) + 3 Na
2
CO
3
(aq) → 6 NaCl (aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) Fe
2
(CO
3
)
3
b) Fe(OH)
3
c) FePO
4
d) Fe
2
O
3
15. The reaction between aqueous solutions of silver nitrate and sodium hydroxide will produce sodium nitrate and an ionic compound not soluble in water.
2 AgNO
3
(aq) + 2 NaOH (aq) → 2 NaNO
3
(aq) + H
2
O (l) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) Ag
2
CO
3
b) Ag
3
PO
4
c) AgCl
d) Ag
2
O
16. The reaction between aqueous solutions of silver nitrate and hydrogen chloride gas dissolved in water (hydrochloric acid) will produce nitric acid and an ionic compound not soluble in water.
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AgNO
3
(aq) + HCl (aq) → HNO
3
(aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) Ag
2
CO
3
b) Ag
3
PO
4
c) AgCl
d) Ag
2
O
Name: ___________________________
Post Lab Questions
Circle it with pen or pencil, or highlight in yellow for the following multiple-choice questions. Check solubility rules in Table 9.7 on page 4 or Google search on the Internet.
17. The reaction between aqueous solutions of silver nitrate and sodium phosphate will produce sodium nitrate and an ionic compound not soluble in water.
3 AgNO
3
(aq) + Na
3
PO
4
(aq) → 3 NaNO
3
(aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) Ag
2
CO
3
b) Ag
3
PO
4
c) AgCl
d) Ag
2
O
18. The reaction between aqueous solutions of silver nitrate and sodium carbonate will produce
sodium nitrate and an ionic compound not soluble in water.
2 AgNO
3
(aq) + Na
2
CO
3
(aq) → 2 NaNO
3
(aq) + Solid
Which one of the following ionic compounds is the solid that precipitates out of water since
it is an ionic compound not soluble in water? a) Ag
2
CO
3
b) Ag
3
PO
4
c) AgCl
d) Ag
2
O
11
Name: ___________________________
Prelab Questions
Circle with pen or pencil, or highlighting in yellow for your answers in the following multiple-
choice questions.
1. Which one of the following statements best defines precipitate formation?
a) Formation of gas bubbles in a chemical reaction
b) Formation of an insoluble ionic compound in a chemical reaction
c) Formation of a liquid in a chemical reaction
2 Which one of the following statements defines spectator ions?
a) Ions that take an active part in a chemical reaction
b) Ions that do not take an active part in a chemical reaction
3. How can you tell if a gas forms during a reaction?
a) Gas bubbles appear
b) Smell of a gas
c) Both of these
4. For precipitation reaction of iron(II) carbonate by mixing iron(II) sulfate with sodium carbonate can be typed out as:
FeSO
4
(aq) + Na
2
CO
3
(aq) → FeCO
3
(s) + Na
2
SO
4
(aq)
Which one of the following is this representation of the precipitation reaction of iron(II) carbonate? a) Condensed b) Complete ionic
c) Net ionic
5. For precipitation reaction of iron(II) carbonate by mixing iron(II) sulfate with sodium carbonate can be typed out as:
12
Fe
2+
(aq) + SO
4
2−
(aq) + 2 Na
+
(aq) + CO
3
2−
(aq) → FeCO
3
(s) + 2 Na
+
(aq) + SO
4
2−
(aq)
Which one of the following is this representation of the precipitation reaction of iron(II) carbonate?
a) Condensed form
b) Complete ionic form
c) Net ionic form
Name: ___________________________
Prelab Questions Continued
Circle with pen or pencil, or highlighting in yellow for your answers in the following multiple-
choice questions.
6. For precipitation reaction of iron(II) carbonate by mixing iron(II) sulfate with sodium carbonate can be typed out as:
Fe
2+
(aq) + CO
3
2−
(aq) → FeCO
3
(s) Which one of the following is this representation of the precipitation reaction of iron(II) carbonate?
a) Condensed form
b) Complete ionic form
c) Net ionic form
7. For precipitation reaction of iron(II) carbonate by mixing iron(II) sulfate with sodium carbonate can be typed out as:
FeSO
4
(aq) + Na
2
CO
3
(aq) → FeCO
3
(s) + Na
2
SO
4
(aq)
Which of the following are two spectator ions?
a) Na
+
b) SO
4
2−
c) Both of these are spectator ions.
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Name
Chem
Section
Data Sheet
determination
23°C
23°C
25°C
temperature of filtered KHT
solution, °C
0.04m
concentration of NaOH solution,
mol L-
0.04 m
0.04m
KHT solution
14.9
49-5
final buret reading, mL
initial buret reading, mL
49.9
volume of KHT
used, mL
NaOH solution
28
final buret reading, mL
10
49.8
१.१
49.7
initial buret reading, mL
50
40mL
volume of NaOH
used, mL
number of moles of NaOH used
0014
0014
number of moles of HT titrated
.04
[HT] in KHT solution, mol L-
1.42
1.142
1.142
[K*] in KHT solution, mol L-1
solubility of KHT, mol L-1
average solubility of KHT,
mol L-
Ksp
average Ksp
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Constants | Periodic Table
These questions refer to determing unknown
concentrations of acids and/or bases.
Part A
In a titration experiment, a solution of rubidium hydroxide (RBOH) of unknown concentration was titrated with a solution of nitric acid
(HNO3) of known concentration. 15.00 mL of the unknown rubidium hydroxide (RbOH) solution required 23.21 mL of 0.1429 mol L-1 nitric
acid (HNO3) solution. What is the concentration of the rubidium hydroxide (RbOH) solution?
OH
9.235x10-2 mol L-1
0.2211 mol L-1
0.2322 mol L-
0.1429 mol L-1
0.2587 mol L
|-1
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9. A solution of 40ml containing 15 grams of sodium hydroxide is analyzed.
a. What is the concentration of the solution?
O 4.7M
10 M
3.7 M
9.4 M
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41. What volume of 0.110 M H2SO4 is required to exactly neutralize 10.0 mL of 0.085 M NaOH?
а.
0.19 mL
b. 7.7 mL
c. 0.39 mL
d. 3.9 mL
е.
1.9 mL
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II
TEXT ANSWER
Question 18
Calculate the molarity of a sodium hydroxide solution if
50.0 mL of this solution was completely neutralized by 46.6
mL of 0.750 M sulfuric acid.
Balanced equation:
H,SO, +2N2OH→ Na,SO4+2H,0
->
Show your work. Use the following formula:
2x mL H2SO4 × [H2SO4]
[N2OH]=
mL NAOH
Normal
BIUS
A A
Vx
X2 x2
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Consider the titration of 25.00 mL of Sprite with 0.050 M NaOH. Using the following
data, determine the citric acid concentration in Sprite (g/L). Take the molar mass of
citric acid to be 192.124 g/mol. Give your answer to one decimal place.
initial volume (mL)
final volume (mL)
Buret reading (mL)
1.75
14.32
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What is the coefficient for water in the following reaction that is balanced in base? Please enter only a numeric value in the box.
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14
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A student is analyzing an unknown chloride mixture to discover the percentage of chloride in the sample. The following three sets of titration data were collected using a 0.05205 M silver nitrate solution. Find the percent chloride value for each sample, the average percent chloride value, and the parts per thousand value for the three samples.
Sample #1: 0.1100 g sample required 18.25 mL of silver nitrate
Sample #2: 0.1050 g sample required 17.30 mL of silver nitrate
Sample #3: 0.1199 g sample required 20.42 mL of silver nitrate
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Macmillan Learning
Experiment 1: Suppose a student repeats the experiment, but adds 25 g of sodium bicarbonate to the 6 M HC
instead of adding 1 M NaOH. What observations indicate that a reaction took place?
Bubbles formed in the solution after the sodium bicarbonate was added to the HCl in the Erlenmeyer flas
The solution changed color after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
A reaction did not happen when the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
The temperature decreased after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
A precipitate (solid) formed after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
The temperature increased after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
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14.
What volume of 0.10 M NAOH is required to neutralize 45.0 ml of 0.8M hydroiodic acid, HI?
А.
36 mL
в. О 178 mL
5.6 mL
D.
360 mL
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6. According to label on a bottle of concentrated hydrochloric acid, the contents are
37% of HCI by mass has a density of 1.18g/ml. Calculate the molarity of acid.
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- 2arrow_forwardDuring a titration experiment, you notice that no matter how much base you add to the sample of acid, the color of the solution does not change. In fact, you have added three times the amount of base you expected to add! What is the next thing you should do to troubleshoot this problem? a. Try the titration with another base. Maybe this one doesn't react with your acid. b. Put everything into the waste container and start over. c. Redo your calculation to make sure you are expecting the correct amount of base. d. Add a few drops of indicator to your flask. Perhaps you forgot to add them.arrow_forwardThe following volumes of 0.000300 M SCN- are diluted to 15.00 mL. Determine the concentration of SCN- in each sample after dilution. These values will be used during the experiment. Sample 0.000300 M SCN- (mL) [SCN-] (M) 1 1.50 2 3.50 3 7.00 4 10.00arrow_forward
- Can someone pls help thxarrow_forwardVolumetric Analysis Liza carefully pipets 25.0 mL of 0.525 M NaOH into a test tube. She places the test tube into a small beaker to keep it from spilling and then pipets 75.0 mL of 0.355 M HCl into another test tube. When Liza reaches to put this test tube of acid into the beaker along with test tube of base, she accidentally knocks the test tubes together hard enough to break them and their respective contents combine in the bottom of the beaker. Is the solution formed from the contents of the two test tubes acidic or basic? What is the pH of the resulting solution?arrow_forwardRemaining Time: 41 minutes, 51 seconds. * Question Completion Status: A Moving to another question will save this response. Question 19 What concentration of 29.03 mL of H2SO4 can be prepared from 13.53 mL of 0.45 M H2SO4? 8.5 M 0.21 M 0.34 M 9.6 M A Moving to another question will save this response.arrow_forward
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