Questions and Answers
Of the species below, only ________ is not an electrolyte.
The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is ________.
Aqueous potassium chloride will react with which one of the following in an exchange (metathesis) reaction?
This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified. This compound is ________.
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The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2 gas is ________.
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The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is ________.
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Which of the following is insoluble in water at 25 °C?
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When aqueous solutions of ________ are mixed, a precipitate forms.
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Which one of the following compounds is insoluble in water?
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Which one of the following compounds is insoluble in water?
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Which combination will produce a precipitate?
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Which combination will produce a precipitate?
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Which combination will produce a precipitate?
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With which of the following will the ammonium ion form an insoluble salt?
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The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________.
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The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is ________.
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The reaction between strontium hydroxide and chloric acid produces ________.
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Which one of the following is a diprotic acid?
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Which one of the following is a triprotic acid?
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Which one of the following is a weak acid?
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Which of the following are weak acids?
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A compound was found to be soluble in water. It was also found that addition of acid to an aqueous solution of this compound resulted in the formation of carbon dioxide. Which one of the following cations would form a precipitate when added to an aqueous solution of this compound?
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The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is ________.
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The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________.
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Study Notes
Electrolytes and Reactions
- Ar is identified as the only non-electrolyte among given options.
- Complete neutralization of sulfuric acid (H2SO4) by potassium hydroxide (KOH) results in potassium sulfate (K2SO4) and water, represented by the equation H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq).
- Potassium chloride in an aqueous solution reacts with lead nitrate in a metathesis reaction, forming a precipitate.
Solubility and Precipitation Reactions
- (NH4)2S is a highly soluble compound producing H2S gas upon acidification.
- Formation of insoluble compounds occurs when mixing certain aqueous solutions.
- NiI2 formation involves the net ionic equation: NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq).
Acids, Bases, and Ionic Strength
- Aluminum hydroxide reacts with nitric acid to yield aluminum nitrate and water, concluding with the equation Al(OH)3 (s) + 3H+ (aq) → 3H2O (l) + Al3+ (aq).
- Mg3(PO4)2 is an insoluble salt in water at 25 °C.
- The formation of precipitates is expected when mixing NaOH (aq) and Mg(NO3)2 (aq).
Acid-Base Neutralization
- Strong acids tend to neutralize bases releasing water.
- Diprotic (e.g., sulfuric acid) and triprotic acids (e.g., phosphoric acid) can donate multiple protons.
- HF is categorized as a weak acid, while HCl is a strong acid.
Oxidation and Reduction
- Oxidation involves loss of electrons, while reduction involves gain of electrons.
- Certain reactions involving metals and acids undergo oxidation-reduction processes, like Zn (s) in hydrobromic acid yielding hydrogen gas.
- Spontaneous reactions proceed naturally under standard conditions; however, some are non-spontaneous.
Molarity and Concentration Calculations
- Molarity is defined as moles of solute per liter of solution.
- Dilution calculations involve mixing solutions to achieve desired concentrations.
- The number of moles of ions in solutions can be computed based on volume and molarity.
Titration and Neutralization
- Endpoint in titration occurs at the moment an indicator signals the completion of the reaction.
- The volume of titrant required can vary greatly depending on the concentration of both the acid and base involved in the reaction.
Key Chemical Concepts
- Oxidation states indicate changes during reactions; oxygen may increase or decrease its oxidation number depending on reactants.
- Activity series assists in determining whether certain metal reactions are feasible based on their reactivity.
- Hydrochloric acid does not appear in its elemental form due to its high reactivity with water to form hydronium ions.
Practical Applications
- Careful solution preparation is essential for experimental accuracy in lab scenarios, especially in titration and neutralization processes.
- Identifying the nature of reactions involving weak and strong acids can guide choices in laboratory methods and environmental chemistry applications.
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Description
Test your knowledge with this multiple choice quiz based on Chapter 4 of your chemistry textbook. Covered topics include electrolytes, neutralization reactions, and their balanced equations. Perfect for students looking to reinforce their understanding of these concepts.
