Soluble and Insoluble Compounds Chart - Solubility Rules Table - List of Salts & Substances
TLDRThis video script offers an in-depth exploration of solubility rules for chemical compounds, focusing on soluble and insoluble ions and their behavior in aqueous and solid states. It highlights always-soluble ions like group one metals and ammonium, and delves into exceptions for chlorides, sulfates, and hydroxides. The script also provides practical examples and practice problems to test viewers' understanding of solubility, emphasizing the importance of knowing exceptions for accurate predictions in chemistry.
Takeaways
- 📚 Solubility rules are essential for determining if a compound will dissolve in water (aqueous) or remain as a solid (insoluble).
- 🧲 Group one metal cations, including lithium, sodium, potassium, and all alkali metals, are always soluble.
- 🌊 The ammonium ion, nitrate, acetate, chlorate, and perchlorate are also always soluble in water.
- 🚫 Halides are generally soluble except when bonded to silver, lead, and mercury ions.
- 🌀 Sulfates are typically soluble except with calcium, strontium, barium, lead, silver, and mercury cations.
- ❌ Hydroxides are generally insoluble, with exceptions for alkali metals, ammonia, and some group two metals like calcium, strontium, and barium.
- 🚫 Carbonates, phosphates, chromates, and sulfides are usually insoluble, with solubility for group one metals and ammonium.
- 📝 To determine solubility, compare the ions in a compound to the solubility rules and exceptions.
- 🔍 Practice identifying solubility by categorizing compounds as aqueous (aq) if soluble or solid (s) if insoluble.
- 📚 Understanding solubility rules and exceptions can significantly improve performance on chemistry exams.
- 🎓 The video concludes with a reminder of the importance of knowing solubility rules for chemistry success.
Q & A
Which cations from the first column of the periodic table are always soluble?
-The cations from the first column of the periodic table, including lithium (Li+), sodium (Na+), potassium (K+), and others like cesium (Cs+) and rubidium (Rb+), are always soluble.
Besides the group one metal cations, what other ions are always soluble in water?
-Besides the group one metal cations, the ammonium ion (NH4+), the nitrate ion (NO3-), acetate (CH3COO-), chlorate (ClO3-), and perchlorate (ClO4-) ions are also always soluble in water.
What are the general solubility rules for chlorides, bromides, and iodides?
-Chlorides, bromides, and iodides are generally soluble except when bonded to silver (Ag), lead (Pb), and mercury (Hg) cations.
Under what conditions are sulfates considered insoluble?
-Sulfates are generally soluble, but they become insoluble when bonded to calcium (Ca2+), strontium (Sr2+), barium (Ba2+), lead (Pb2+), silver (Ag), or mercury (Hg) cations.
What are the exceptions to the general rule that hydroxides are insoluble?
-The exceptions to the rule that hydroxides are insoluble include alkali metals like sodium (Na) and potassium (K), ammonia (NH3), and group two metals starting with calcium (Ca) and below, which are soluble with hydroxide.
Which compounds are generally insoluble except for when bonded to specific ions?
-Carbonates, phosphates, chromates, and sulfides are generally insoluble except when bonded to group one metals like sodium (Na), lithium (Li), and potassium (K), or the ammonium ion (NH4+).
What does 'aq' stand for in the context of solubility and what does it indicate?
-'Aq' stands for 'aqueous' and indicates that a compound is soluble in water, meaning it is dissolved in water.
What does 's' stand for in the context of solubility and what does it indicate?
-'S' stands for 'solid' and indicates that a compound is insoluble in water, meaning it forms a precipitate and does not dissolve in water.
Why is silver chloride (AgCl) considered insoluble according to the solubility rules?
-Silver chloride (AgCl) is considered insoluble because, although chlorides are generally soluble, silver (Ag) is an exception to this rule, making silver chloride insoluble.
Is barium hydroxide (Ba(OH)2) soluble or insoluble and why?
-Barium hydroxide (Ba(OH)2) is soluble because barium (Ba) is a group two metal, which is an exception to the general rule that hydroxides are insoluble.
How can you determine if a sulfate compound is soluble or insoluble?
-A sulfate compound is soluble unless it is bonded to an ion that is an exception to the general solubility rule, such as calcium (Ca2+), strontium (Sr2+), barium (Ba2+), lead (Pb2+), silver (Ag), or mercury (Hg) cations.
What does it mean for a compound to be considered 'insoluble' in the context of this script?
-In the context of this script, a compound being 'insoluble' means that it does not dissolve in water and will form a solid precipitate when mixed with water.
Can you provide an example of an insoluble carbonate and explain why it is insoluble?
-An example of an insoluble carbonate is calcium carbonate (CaCO3). It is insoluble because carbonates are generally insoluble, and calcium (Ca) is not an exception to this rule.
Why is aluminum phosphate (AlPO4) considered insoluble?
-Aluminum phosphate (AlPO4) is considered insoluble because phosphates are generally insoluble, and aluminum (Al) is not an exception to this rule.
Outlines
🧪 Solubility Rules and Chemistry Basics
This paragraph introduces the topic of soluble and insoluble compounds, focusing on the solubility rules that are key to understanding chemistry. It emphasizes the importance of knowing which compounds or ions are always soluble, such as lithium, sodium, potassium, and ammonium ions, as well as nitrate, acetate, chlorate, and perchlorate. The paragraph also discusses the general solubility of chlorides, bromides, iodides, sulfates, and the exceptions to these rules, such as silver, lead, and mercury ions. It sets the stage for the video by outlining the structure and what viewers can expect to learn, including practice problems and examples.
📚 Applying Solubility Rules with Examples
This paragraph delves into applying the solubility rules with practical examples. It challenges viewers to determine the solubility of various compounds, instructing them to write 'aq' for aqueous (soluble in water) and 's' for solid (insoluble). The paragraph provides a step-by-step analysis of compounds like sodium chloride, silver chloride, potassium hydroxide, and aluminum hydroxide, explaining why each is soluble or insoluble based on the ions involved. It also covers other compounds like barium hydroxide, magnesium iodide, lithium carbonate, and barium sulfate, reinforcing the rules with specific cases.
📝 More Practice Problems and Conclusion
The final paragraph presents additional practice problems for viewers to test their understanding of solubility rules. It includes compounds like barium nitrate, calcium sulfide, ammonium hydroxide, mercury chloride, sodium phosphate, silver acetate, aluminum perchlorate, barium carbonate, ammonium carbonate, and calcium acetate. The paragraph reinforces the idea that knowing the solubility rules and exceptions can significantly aid in solving such problems. It concludes by encouraging viewers to apply this knowledge for their chemistry exams and thanks them for watching the video.
Mindmap
Keywords
💡Solubility
💡Solubility Rules
💡Aqueous
💡Insoluble
💡Group One Metals
💡Ions
💡Exceptions
💡Hydroxides
💡Carbonate
💡Sulfate
💡Practice Problems
Highlights
The video discusses soluble and insoluble compounds, focusing on how to determine if they will be aqueous or solid based on solubility rules.
Ions from the first column of the periodic table, such as lithium, sodium, potassium, cesium, and rubidium, are always soluble.
Ammonium, nitrate, acetate, and chlorate/perchlorate ions are always soluble in water.
Chlorides, bromides, and iodides are generally soluble except when bonded to silver, lead, or mercury ions.
Sulfates are generally soluble except with calcium, strontium, barium, lead, silver, and mercury ions.
Hydroxides are generally insoluble, but exceptions include alkali metals, ammonia, and some group two metals like calcium, strontium, and barium.
Carbonates, phosphates, chromates, and sulfides are mostly insoluble, with exceptions being group one metals and the ammonium ion.
Practice problems are provided to apply knowledge of solubility rules and determine if compounds are soluble (aq) or insoluble (s).
Sodium chloride (NaCl) is soluble due to sodium being a group one metal.
Silver chloride (AgCl) is insoluble because silver is an exception for halides.
Potassium hydroxide (KOH) is soluble as potassium is a group one metal.
Aluminum hydroxide is insoluble because aluminum is not a group one or two metal.
Barium hydroxide is soluble despite hydroxides generally being insoluble, as barium is an exception.
Magnesium iodide (MgI2) is soluble because magnesium is not an exception for iodides.
Lead iodide (PbI2) is insoluble due to lead being an exception for iodides.
Lithium carbonate is soluble because lithium is a group one metal.
Barium sulfate is insoluble, as barium is an exception for sulfates.
Potassium sulfide is soluble due to potassium being a group one metal.
Calcium phosphate is insoluble because calcium is not an exception for phosphates.
Magnesium sulfate is soluble as magnesium is not an exception for sulfates.
Aluminum phosphate is insoluble because aluminum is not an exception for phosphates.
Additional practice problems are provided to further test understanding of solubility rules.
Knowing the exceptions to solubility rules can help solve 60-70% of related chemistry problems.
Transcripts
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