Questions and Answers
What does ion concentration refer to?
What is the concentration of K+ in 0.15 M of K2S?
0.3 M
What can be said about the concentration of the Ca2+ ion when CaCl2 is dissolved in water?
It will be equal to 0.5 M if 0.5 M CaCl2 is used.
How many grams of Na3PO4 are needed to produce 700 mL of a solution that has a concentration of Na+ ions of 0.800 M?
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What is an electrolyte?
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Classify the following solute reactions: X(s)→X(aq) and CD(aq)⇌C+(aq)+D−(aq).
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Which of the following compounds is a strong electrolyte?
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Which samples will conduct electricity?
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Which solid is a weak electrolyte when dissolved in water?
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If one of the tested solids is barium chloride (BaCl2), which solids could be BaCl2?
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Rank the following substances based on conductivity from most conductive to least: barium chloride, potassium bromide, butanoic acid, sugar.
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Which combinations could yield a black precipitate?
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What is the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate?
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Which of the following choices is insoluble: AX, AY, AZ, BX, BY, BZ?
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Classify these compounds as soluble or insoluble.
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Study Notes
Ion Concentration
- Represents molar concentration of ions in a solution.
- May differ from the molar concentration of the compound.
- For soluble salts, molarity of an ion = molarity of compound × ion subscript.
- Example: 1 M of AlCl3 yields 1 M Al3+ and 3 M Cl−.
K+ Concentration in K2S
- The concentration of K+ in a 0.15 M K2S solution is 0.30 M.
Ca2+ Ion Concentration in CaCl2
- The concentration of Ca2+ from dissolved CaCl2 can be inferred with respect to molarity.
Na3PO4 Solution Preparation
- To prepare 700 mL of 0.800 M Na+ solution from Na3PO4, 30.6 g of Na3PO4 is required.
Electrolytes
- Substances that dissociate in solution to produce ions and conduct electricity are called electrolytes.
- Strong electrolytes fully dissociate into ions; weak electrolytes partially dissociate.
- Non-electrolytes remain as molecules in solution.
Electrode Classification
- Strong electrolytes: YZ, PQ.
- Weak electrolytes: X, R.
- Non-electrolyte: CD.
Classification of Common Solutes
- Strong electrolytes: Hydrochloric acid (HCl), Calcium hydroxide (Ca(OH)2), Aluminum chloride (AlCl3).
- Weak electrolytes: Acetic acid (H3CCOOH), Ammonia (NH3).
- Non-electrolytes: Sucrose (C12H22O11), Butanol (C4H9OH).
Conductivity Tests
- Only NaCl solution from a sugar solution and solid NaCl will conduct electricity.
Identifying Weak Electrolytes
- Among solids A, B, C, and D, solid B is identified as a weak electrolyte due to its dim light emission.
Barium Chloride Identification
- Solids A and D could represent BaCl2 based on their bright light emission.
Conductivity Ranking
- Conductivity ranking for 0.20 M solutions:
- Most to least conductive: Barium chloride, Potassium bromide, Butanoic acid, Sugar.
Precipitation Reactions
- General solubility rules include:
- Group I compounds, nitrates, and chlorates are soluble.
- Carbonates, hydroxides, phosphates, and sulfides are typically insoluble.
Black Precipitate Formation
- Combinations yielding a black precipitate include:
- Li2S(aq) + Pb(NO3)2(aq)
- K2S(aq) + Sn(NO3)4(aq)
Net Ionic Equation for NaCl and AgNO3
- The net ionic equation is: Ag+(aq) + Cl−(aq) → AgCl(s).
Insoluble Choices from Reaction Data
- In the given reactions, AZ is identified as insoluble.
Qualitative Analysis
- Entails assessing the solubility of compounds under specific conditions.
Solubility Classification
- Soluble compounds: Strontium hydroxide, Sodium sulfate, Calcium hydroxide, Potassium sulfate, Nickel(II) sulfate, Potassium hydroxide, Iron(II) sulfate.
- Insoluble compounds: Strontium sulfate, Copper(II) hydroxide, Magnesium sulfide.
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