13.25 By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g ofwater at 40 °C will lead to a saturated solution: (a) NaNO(b) KCl, (c) K2Cr2O7, (d) Pb(NO3)2.10 1 SECTION 13.3 Factors AffectinHenry's lawGo FigureGo FigureHow does the solubility of KCI at 80 °C compare with thatof NaCl at the same temperature?molarity), Pnality constantBetween which two gases would you ethis graph?s on the soluteter at 25 CandCH10090n25°Cwateris2.0NANO3partial pressure°Calso doubles70CaCl2CO60bonated beverPb(NO3)2nl atm. When50КСІ1.0e the solution40sfrom the solNaCl30KСIO,Не2010Ce2(SO4)320100Temperature0010 20 30 40 50 60 70 80 90 100AFigure 13.16 Solubilities of four gaseof temperature. The solubilities are in msolution, for a constant total pressure oTemperature (°C)A Figure 13.15 Solubilities of some ionic compounds in water asa function of temperature.Temperature EffectsThe solubility of most solid solutes in water increases as the solution temperature increases,as Figure 13.15 shows. There are exceptions to this rule, however, as seen for Ce2(SO4)3,whose solubility curve slopes downward with increasing temperature.In contrast to solid solutes, the solubility of gases in water decreases with increasing tem-perature (Figure 13.16). If a glass of cold tap water is warmed, you can see bubbles on theinside of the glass because some of the dissolved air comes out of solution.Similarly, as carbonated beverages are allowed to warm, the solubility of CO2decreases, and CO2 (g) escapes from the solution.of solution whenution is reducedes in13.4Solubility (g of salt in 100 g H2O)KNO3% R 8 RK2Cr2O7Solubility (mM)

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Asked Nov 18, 2019
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13.25 By referring to Figure 13.15, determine whether the addi
tion of 40.0 g of each of the following ionic solids to 100 g of
water at 40 °C will lead to a saturated solution: (a) NaNO
(b) KCl, (c) K2Cr2O7, (d) Pb(NO3)2.
10 1
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13.25 By referring to Figure 13.15, determine whether the addi tion of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution: (a) NaNO (b) KCl, (c) K2Cr2O7, (d) Pb(NO3)2. 10 1

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SECTION 13.3 Factors Affectin
Henry's law
Go Figure
Go Figure
How does the solubility of KCI at 80 °C compare with that
of NaCl at the same temperature?
molarity), P
nality constant
Between which two gases would you e
this graph?
s on the solute
ter at 25 Cand
CH
100
90
n25°Cwateris
2.0
NANO3
partial pressure
°Calso doubles
70
CaCl2
CO
60
bonated bever
Pb(NO3)2
nl atm. When
50
КСІ
1.0
e the solution
40
sfrom the sol
NaCl
30
KСIO,
Не
20
10
Ce2(SO4)3
20
10
0
Temperature
0
0
10 20 30 40 50 60 70 80 90 100
AFigure 13.16 Solubilities of four gase
of temperature. The solubilities are in m
solution, for a constant total pressure o
Temperature (°C)
A Figure 13.15 Solubilities of some ionic compounds in water as
a function of temperature.
Temperature Effects
The solubility of most solid solutes in water increases as the solution temperature increases,
as Figure 13.15 shows. There are exceptions to this rule, however, as seen for Ce2(SO4)3,
whose solubility curve slopes downward with increasing temperature.
In contrast to solid solutes, the solubility of gases in water decreases with increasing tem-
perature (Figure 13.16). If a glass of cold tap water is warmed, you can see bubbles on the
inside of the glass because some of the dissolved air comes out of solution.
Similarly, as carbonated beverages are allowed to warm, the solubility of CO2
decreases, and CO2 (g) escapes from the solution.
of solution when
ution is reduced
es in
13.4
Solubility (g of salt in 100 g H2O)
KNO3
% R 8 R
K2Cr2O7
Solubility (mM)
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Image Transcriptionclose

SECTION 13.3 Factors Affectin Henry's law Go Figure Go Figure How does the solubility of KCI at 80 °C compare with that of NaCl at the same temperature? molarity), P nality constant Between which two gases would you e this graph? s on the solute ter at 25 Cand CH 100 90 n25°Cwateris 2.0 NANO3 partial pressure °Calso doubles 70 CaCl2 CO 60 bonated bever Pb(NO3)2 nl atm. When 50 КСІ 1.0 e the solution 40 sfrom the sol NaCl 30 KСIO, Не 20 10 Ce2(SO4)3 20 10 0 Temperature 0 0 10 20 30 40 50 60 70 80 90 100 AFigure 13.16 Solubilities of four gase of temperature. The solubilities are in m solution, for a constant total pressure o Temperature (°C) A Figure 13.15 Solubilities of some ionic compounds in water as a function of temperature. Temperature Effects The solubility of most solid solutes in water increases as the solution temperature increases, as Figure 13.15 shows. There are exceptions to this rule, however, as seen for Ce2(SO4)3, whose solubility curve slopes downward with increasing temperature. In contrast to solid solutes, the solubility of gases in water decreases with increasing tem- perature (Figure 13.16). If a glass of cold tap water is warmed, you can see bubbles on the inside of the glass because some of the dissolved air comes out of solution. Similarly, as carbonated beverages are allowed to warm, the solubility of CO2 decreases, and CO2 (g) escapes from the solution. of solution when ution is reduced es in 13.4 Solubility (g of salt in 100 g H2O) KNO3 % R 8 R K2Cr2O7 Solubility (mM)

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Expert Answer

Step 1

a)

NaNO3’s solubility in the figure 13.15 is more than 100g per 100g of water at 400C and for the given solution of NaNO3 is 40g per 100g of water at the same temperature. So, the given solution forms an unsaturated solution.

Step 2

b)

KCl’s solubility in the figure 13.15 is less than 40g at 400C. But for the given solution of KCl is 40g per 100g of water at the same temperature. So, the given solution forms a saturated solution.

Step 3

c)

K2Cr2O7’s solubility in the figure 13.15 is less than 22g at 400C and for the given solution of K2Cr2O7is 40g per 100g of water...

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