Solubility Rules and Precipitation Reactions

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Questions and Answers

What is the term for an insoluble ionic compound that forms during a chemical reaction in an aqueous solution?

  • Solution
  • Solvent
  • Precipitate (correct)
  • Solute

A solubility table is used to determine if an ionic compound will dissolve in water.

True (A)

What term describes ions that remain dissolved and unchanged during a precipitation reaction?

Spectator ions

A precipitation reaction occurs when two aqueous solutions produce a(n) __________.

<p>precipitate</p> Signup and view all the answers

Match the following ions with their solubility behavior:

<p>Sodium (Na+) = Generally soluble, with no common exceptions Nitrate (NO3-) = Generally soluble, with no common exceptions Carbonate (CO32-) = Generally insoluble, except when combined with Group 1 metals or ammonium Chloride (Cl-) = Generally soluble, except when combined with silver, lead, or mercury(I)</p> Signup and view all the answers

According to solubility rules, which of the following compounds is likely to be insoluble in water?

<p>AgCl (B)</p> Signup and view all the answers

All nitrate compounds are soluble in water, regardless of the cation.

<p>True (A)</p> Signup and view all the answers

What type of chemical reaction is a precipitation reaction primarily classified as?

<p>Double displacement</p> Signup and view all the answers

In a chemical equation for a precipitation reaction, (aq) indicates that the substance is __________ in water, while (s) indicates it is a __________.

<p>dissolved, solid</p> Signup and view all the answers

Match each ionic compound with its expected solubility in water:

<p>AgNO3 = Soluble PbSO4 = Insoluble KOH = Soluble CaCO3 = Insoluble</p> Signup and view all the answers

Which of the following pairs of aqueous solutions, when mixed, will likely form a precipitate?

<p>AgNO3 and KCl (C)</p> Signup and view all the answers

Spectator ions participate directly in the formation of a precipitate.

<p>False (B)</p> Signup and view all the answers

Define a 'full' or 'overall' equation.

<p>full balanced chemical equation</p> Signup and view all the answers

The net ionic equation focuses only on the ions that _________ in the reaction, omitting the __________ ions.

<p>react, spectator</p> Signup and view all the answers

Match each term with its appropriate description in the context of precipitation reactions:

<p>Soluble = Capable of dissolving in water Insoluble = Unable to dissolve in water to a significant extent Spectator Ion = An ion that exists in the same form on both the reactant and product sides of a chemical reaction and does not affect equilibrium Precipitate = A solid that forms out of solution as a result of a chemical reaction</p> Signup and view all the answers

Which of the following is the correct general format for a full balanced equation?

<p>Ionic Compound A (aq) + Ionic Compound B (aq) → Precipitate (s) + Ionic Compound D (aq) (D)</p> Signup and view all the answers

Spectator ions undergo a change in physical state during a precipitation reaction.

<p>False (B)</p> Signup and view all the answers

What does (aq) mean?

<p>dissolved in water</p> Signup and view all the answers

The solubility table/rules are used when the ionic compounds produced will be a __________.

<p>solid</p> Signup and view all the answers

What are the 3 steps on how to write an ionic equation for a precipitation reaction?

<p>Step 1 = Start off by writing the ionic formula of the precipitate on the products Step 2 = Writing the individual cations and anions of the precipitate on the reactants Step 3 = Add coefficients appropriately to the reactants to ensure net zero charge</p> Signup and view all the answers

Given the reaction: $AgNO_3(aq) + NaCl(aq) \rightarrow AgCl(s) + NaNO_3(aq)$, which ion(s) is/are the spectator ion(s)?

<p>$Na^+$ and $NO_3^-$ (D)</p> Signup and view all the answers

All precipitation reactions result in the formation of a toxic gas.

<p>False (B)</p> Signup and view all the answers

When writing a balanced chemical equation for a precipitation reaction, what physical state symbol is used to denote the precipitate?

<p>(s)</p> Signup and view all the answers

In order to determine the spectator ions of an precipitation equation, the product formed alongside the __________ needs to be predicted.

<p>precipitate</p> Signup and view all the answers

Match each of the following example equations to their type, either full/overall equation or ionic equation

<p>$CuSO_4(aq) + 2NaCl(aq) \rightarrow Na_2SO_4(aq) + CuCl_2(s)$ = Full/overall equation $Pb^{2+}(aq) + 2OH^-(aq) \rightarrow Pb(OH)_2(s)$ = Ionic equation</p> Signup and view all the answers

Flashcards

What is a solubility table?

A chart listing ionic compounds and their solubility in water.

Reaction of ionic compounds

When two soluble ionic compounds react, they form two new ionic compound products.

What is a precipitation reaction?

A chemical reaction where soluble reactants yield an insoluble product (precipitate).

What is a double-displacement reaction?

A reaction where the cation and anion of two reactants switch places to form two new products.

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What is a full/overall equation?

An equation showing the complete neutral formulas for each compound in the reaction as if they were molecules.

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What is an ionic equation?

An equation showing only the ions that participate in the reaction, omitting spectator ions.

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What are spectator ions?

Ions that remain dissolved during a precipitation reaction and do not participate in the chemical change.

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Study Notes

  • Solubility tables and precipitation reactions are the topic

Chemical Reactions Between Ionic Compounds

  • When two soluble ionic compounds react, there are two possible outcomes
  • Two new ionic compound products are both soluble
  • Two new ionic compound products, one of which is insoluble (precipitate) and another that is soluble

Solubility Table

  • A solubility table predicts the solubility of an ionic compound
  • Solubility of different ions:
  • Sodium, Potassium, Ammonium, Nitrate, Perchlorate, and Ethanoate are generally soluble with no exceptions
  • Chloride, Bromide, and Iodide are soluble, except when combined with Silver (Ag+) or Lead (Pb2+)
  • Sulfate is soluble, except when combined with Calcium (Ca2+), Barium (Ba2+), Strontium (Sr2+), Silver (Ag+), or Lead (Pb2+)
  • Carbonate, Phosphate, Hydroxide, and Sulfide are generally insoluble
  • The exceptions are when they are combined with Group 1 metal ions or Ammonium

Precipitation Reactions

  • A precipitation reaction occurs when two aqueous solutions produce a precipitate
  • Precipitation reactions are a double-displacement reaction, where ion pairs are exchanged
  • Predicting the solid formation can be done using the solubility table/rules

Writing Balanced Chemical Equations

  • There are two ways of writing balanced chemical equations for precipitation reactions -Full/overall equation, and Ionic equation
  • Full balanced equations have the general formula:
  • Ionic Compound A (aq) + Ionic Compound B (aq) → Precipitate (s) + Ionic Compound D (aq)

Spectator Ions

  • In a precipitation reaction, some ions remain dissolved in solution
  • These ions haven't undergone a change in physical state, and are referred to as spectator ions
  • Spectator ions are identified by predicting the product formed alongside the precipitate

Ionic Equations

  • An ionic equation omits the spectator ions
  • When writing an ionic equation for a precipitation reaction:
  • Start by writing the ionic formula of the precipitate on the products
  • Writing the individual cations and anions of the precipitate on the reactants, add coefficients appropriately to the reactants to ensure net zero charge

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