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100% EVERYDAY.
Name: ____________________________________
General Chemistry
Period: ________
UNIT 10: Solutions and Gases
Date: ___________________
KIPP NYC College Prep
Lecture 2: Table F Solubility Guidelines
By the end of today, you will have an answer to:
How do we determine if a substance is soluble?
Do Now:
Consider the dissolving of 100 g of LiCl in 5.00 L of
water.
1. Which substance is the solute: _______________
solvent: _________________
2. Determine the gram-formula mass of LiCl.
3. Determine the number of moles of LiCl in 100 g.
4. Determine the Molarity of the solution in 5.00 L.
5. Describe why increasing the temperature could increase the solubility of LiCl in water.
Water is polar (has positive H and negative O). This allows it to dissolve some ionic compounds, like NaCl.
However, some ionic compounds are insoluble.
--How do you think the strength of the ionic bonds in these compounds compares to soluble ionic compounds?
1. Based on Figure 1 and the two solutions in front of you, which substance is soluble MgS or KI?
Figure 1
What is the evidence?
--What two ions make MgS? ______________________
--What two ions make KI? ________________________
--Which has stronger ionic bonds? _______________
2. Based on Figure 2, describe what happens to the ions in an ionic compound that dissolve in water.
Figure 2
--What two ions make KCl? ___________________
--How are the K+ and Cl- ions dissolved in water?
Work hard. Be nice.
100% EVERYDAY.
Review Key Terms: If a solid substance is soluble it dissolves in the solvent. If it is insoluble it forms a
precipitate and does not dissolve. A precipitate is the solid in an undissolved mixture.
Solid Added to Solvent
Dissolves or does not dissolve?
Formation of Precipitate?
Soluble
Insoluble
Table F determines solubility of Ionic Compounds.
So how do we use Table F? Listen and annotate
Question: Is NH4Cl soluble in H2O?
--Step 1: What are the two ions? ________________________ --Step 2: find ONE ion on ONE side of the Table!
--Step 3: Determine if soluble or insoluble.
--Step 4: Examine exceptions.
Answer:
______________________________________
Example 2:
Is AgCl soluble in H2O?
Example 3:
Is CaCO3 soluble in H2O?
--Two ions: _______________________________
--Soluble or insoluble? _______________________
--Two ions: _______________________________
--Soluble or insoluble __________________________
In-class Practice:
Directions: State whether the ionic compound will be soluble (precipitate does not form) or insoluble
(precipitate forms)
Ionic
Compound
LiF
HNO3
NaOH
Ca(OH)2
AgBr
Fe3(PO4)2
Soluble (S)/ Insoluble (I)
Ionic
Compound
PbCl2
H2SO4
AgI
CaS
(NH4)2S
KClO4
Soluble (S)/ Insoluble (I)
Work hard. Be nice.
100% EVERYDAY.
Name: ____________________________________
General Chemistry
WORK 10.2 Determining Solubility Using Table F
Period: ________
Date: ___________________
KIPP NYC College Prep
10 points
Important Information First:
1. Why are many ionic compounds soluble in water? Explains in-terms of charge.
____________________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________________
2. Explain what happens to ions in an ionic compound that are soluble vs. those that are insoluble.
____________________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________________
Consider NaClO3.
3. What types of bond()s are found in this compound? _____________________________ and ________________________
4. Using Table F, explain the process of determining how you know that NaClO3 is soluble in water.
____________________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________________
Consider AgCl.
5. What types of bond(s) are found in this compound? ___________________________________________________________
6. Using Table F, explain the process of determining how you know that AgCl is insoluble in water.
____________________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________________
Regents Practice:
1. Which ion, when combined with chloride ions,
Cl-, forms an insoluble substance in water?
(1) Fe2+
(2) Mg2+
(3) Pb2+
(4) Zn2+
2. According to Table F, which of these salts is
least soluble in water?
(1) LiCl
(2) RbCl
(3) FeCl2
(4) PbCl2
3.
Which type of bonding is found in all molecular
substances?
(1) covalent bonding
(2) hydrogen bonding
(3) ionic bonding
(4) metallic bonding
4. Which compound is insoluble in water?
(1) BaSO4
(2) CaCrO4
(3) KClO3
(4) Na2S
5. Which substance contains bonds that
involved the transfer of electrons from one
atom to another?
(1) CO2
(2) NH3
(3) KBr
(4) Cl2
6. According to Reference Table F, which of
these compounds is the least soluble in
water?
(1) K2CO3
(2) KC2H3O2
(3) Ca3(PO4)2
(4) Ca(NO3)2
Work hard. Be nice.
7. Based on Reference Table F, describe the solubility of magnesium hydroxide in water.
8. Based on Reference Table F, describe the solubility of zinc sulfide in water.
9. Identify one ion from Table F that can combine with Pb2+(aq) to produce an insoluble compound.
The dissolving of solid lithium bromide in water is represented by the balanced equation below.
10. Based on Table F, identify one ion that reacts with Br− ions in an aqueous solution to form an insoluble
compound.
11. You’re walk along the beach and stop to reach down and grasp a handful of warm sand
and water. Your friend reaches down and does the same but instead continues to bring
the handful of water to their mouth– but you stop him/her. They argue that it is fresh
water and perfect for drinking on a hot day, but you know better. Explain why the clear
water is still not pure water. Use the terms soluble/ insoluble and mixture/pure
substance.