Unit 5 lesson 2
Select all the compounds that are correctly paired with their solubility in water at 25°C.
CaSO4, insoluble (NH4)2S, soluble
Which of the following ions always form soluble ionic compounds? Select all that apply.
Group 1A cations NO3- NH4+
Which of the following compounds are soluble in water? Select all that apply.
NH4Cl Na3PO4 Pb(NO3)2
Which of the following options describe the steps required to write the ionic and net ionic equations for a precipitation reaction? Select all that apply.
The ionic equation should contain all species present in the reaction mixture. Spectator ions are identified and canceled in the net ionic equation.
An ionic equation shows species ____ in solution. This equation is the ____ accurate representation of the chemical change occurring.
as they actually exist; most
When writing the ionic equation for a reaction ____. (Select all that apply.)
soluble ionic compounds are shown dissociated into ions molecular substances are included
A precipitation reaction occurs when two or more water-_____ salts react in solution to produce a(n) _____ precipitate.
soluble; insoluble
If a fair amount of solute visibly dissolves when added to water, the solute is qualitatively described as being in water. A solute that does not visibly dissolve is considered
soluble; insoluble
Ions that are present in a reaction, but not involved in the actual chemical change, are called ions. These ions will appear unchanged on both sides of a total ionic equation.
spectator
Place the steps required to determine whether or not a precipitate forms when two solutions are mixed in the correct order. Start with the first step at the top of the list.
1.) note the ions present in the reactants2.) consider possible cation-anion combinations3.) use the solubility rules to determine whether or not either of the combinations gives an insoluble salt
Which of the following statements correctly describe a molecular equation? Select all that apply.
A molecular equation will not include any charges on any of the species. This equation represents all reactants and products as if they were intact and undissociated.
Which of the following statements correctly describe a net ionic equation? Select all that apply. Multiple select question.
A net ionic equation shows only the species that have undergone a change in the reaction, and any products that form. A net ionic equation shows only the chemical change that is taking place in a reaction.
Which of the following correctly defines a precipitate?
A solid product that separates from a solution
Which of the following gives the correct net ionic equation for the process represented below? AgNO3(aq) + KCl(aq) → KNO3(aq) + AgCl(s) Multiple choice question.
Ag+(aq) + Cl-(aq) → AgCl(s)
Which of the following options describe how to write the ionic and net ionic equations for a precipitation reaction? Select all that apply.
Any insoluble ionic combinations will be included in the net ionic equation. Start by identifying the ions present in solution. Ions that appear on both sides in the ionic equation will not appear in the net ionic equation.
Which of the following gives the correct net ionic equation for the process represented below? Ba(ClO4)2(aq) + Li2SO4(aq) → BaSO4(s) + 2LiClO4(aq) Multiple choice question.
Ba2+(aq) + SO42-(aq) → BaSO4(s)
Identify ALL the spectator ions in the reaction represented by the following molecular equation: 3Ca(CH3COO)2(aq) + 2K3PO4(aq) → Ca3(PO4)2(s) + 6KCH3COO(aq)
CH3COO-- K+
Which of the following ions typically form water-insoluble salts, except when partnered with a Group 1A cation or NH4+?
CO32- OH- PO43-
Select the correct net ionic equation for the ionic equation given below. Ca(s) + 2H+ (aq) + 2Cl-(aq) → Ca2+(aq) + H2(g) + 2Cl-(aq)
Ca(s) + 2H+(aq) → Ca2+(aq) + H2(g)
Which of the following species should be included in the net ionic equation for the precipitation reaction given? (States of matter have not been included; use the solubility rules to determine which compound(s) form(s) precipitates, if any.) ZnSO4 + CaCl2 → CaSO4 + ZnCl2
Ca2+ CaSO4 SO42-
Which species will appear in the net ionic equation for the reaction shown, given the balanced molecular equation below? Ca(NO3)2(aq) + K2CO3(aq) → CaCO3(s) + 2KNO3(aq)
CaCO3(s) Ca2+(aq) CO32-(aq)
Which of the following options influence the solubility of a solute in a solvent? Select all that apply.
Chemical nature of the solute Quantity of solvent Temperature
Identify ALL the spectator ions in the following ionic equation: 2Na+(aq) + SO42--(aq) + Ba2+(aq) + 2Cl--(aq) → BaSO4(s) + 2Na+(aq) + 2Cl--(aq)
Cl- Na+
Which of the following correctly defines spectator ions?
Ions that do not participate in the reaction although they are present
Match each species in the reaction represented by the molecular equation shown below correctly to the role it plays in the reaction. MgSO4(aq) + BaCl2(aq) → MgCl2(aq) + BaSO4(s)
MgCl2 - soluble ionic species BaSO4 - solid product Ba2+ and SO42- - reactant ions Mg2+ and Cl- - spectator ions
Match each ion to the correct description of its solubility when combined with an ion of opposite charge.
Na+ - soluble in all combinations SO42- - soluble except with Ca2+, Sr2+, Ba2+, Ag+, and Pb2+ CO32- - insoluble except with Group 1A cations or NH4+ Cl- - soluble except with Ag+, Pb2+, Cu+, and Hg22+
When solutions of Na2CO3 and BaCl2 are mixed ____. (Select all that apply.)
Na+ is a spectator ion BaCO3 precipitates from solution
Aqueous solutions of NH4Br and Pb(NO3)2 are mixed. Which of the following species will appear in the net ionic equation? Select all that apply.
Pb2+ Br-- PbBr2
Match each species in the reaction represented by the molecular equation shown below correctly to the role it plays in the reaction. Pb(ClO4)2(aq) + 2KCl(aq) → PbCl2(s) + 2KClO4(aq)
Pb2+ and Cl- - ions that combine to form a precipitate; will appear in the net ionic equation PbCl2 - solid product; will appear in the net ionic equation K+ and ClO4- - reactant ions; will not appear in the net ionic equation KClO4 - soluble salt; will not appear in the net ionic equation
Select the correct net ionic equation if the ionic equation is given below. 2K+(aq) + 2Cl-(aq) + Pb2+(aq) + 2CH3COO--(aq) → 2K+(aq) + PbCl2(s) + 2CH3COO-(aq) Multiple choice question.
Pb2+(aq) + 2Cl-(aq) → PbCl2(s)
Which of the following is the correct formula for the precipitate that forms when aqueous solutions of Pb(NO3)2 and KCl are mixed
PbCl2
Which of the following is the correct formula for the precipitate that forms when aqueous solutions of Pb(NO3)2 and KCl are mixed?
PbCl2
Which of the following options correctly describe the steps required to decide whether or not a precipitate forms when two aqueous solutions are mixed? Select all that apply.
The first step is to identify the ions present in each solution. The products of the reaction are identified from the possible cation-anion combinations. Any product that is insoluble in water will be a precipitate.
Which of the following options correctly describe a precipitation reaction? Select all that apply.
This type of reaction often occurs in aqueous solution. This type of reaction forms one or more insoluble products. This type of reaction usually involves ionic compounds.
Correctly order the steps required to write the ionic and net ionic equations for a given precipitation reaction. Place the first step at the top of the list.
Write a balanced molecular equation... Write the ionic equation... Identify and cancel... The net ionic...
A reaction in which one or more precipitates form when the aqueous solutions of two ionic compounds are mixed is called a(n) displacement reaction, since both pairs of ions exchange partners. Another name for this type of reaction is a(n) reaction.
double; metathesis
A(n) equation shows all soluble ionic substances dissociated into ions. Both the and electrical must be balanced in this type of equation.
ionic, atoms, charges
A precipitate may form when solutions containing ionic compounds are mixed. To identify a precipitate, first consider the _____ present in solution and determine the possible new combinations. Using the solubility rules, determine if one or more of these combinations gives a(n) ____ salt. Such a salt will precipitate from solution.
ions; insoluble
A precipitate may form when solutions containing ionic compounds are mixed. To identify a precipitate, first consider the _____ present in solution and determine the possible new combinations. Using the solubility rules, determine if one or more of these combinations gives a(n) ____ salt. Such a salt will precipitate from solution. Multiple choice question.
ions; insoluble
A precipitate ____. (Select all that apply.)
is a solid that forms from a reaction in solution is often a water-insoluble ionic compound is designated by the symbol (s)
A chemical equation that shows all reactants and products as intact, undissociated compounds is called a(n) equation. The name is misleading because not all compounds are composed of .
molecular molecules
The equation that shows all species as if they were intact and undissociated in solution is called a(n) ____ equation. This equation is the ____ accurate representation of the chemical change occurring.
molecular; least
A(n) ____ equation shows the overall chemical change involved in a given reaction. Spectator ions are ____ in this equation. Multiple choice question.
net ionic; omitted
A solid that forms in a reaction and separates from solution is called a(n) ______.
precipitate
An insoluble product (i.e., a solid) that forms from a reaction in solution is called a(n).
precipitate
A reaction in which two or more soluble ionic compounds react to form an insoluble product is called a(n) _____ reaction.
precipitation
Spectator ions ____. (Select all that apply.)
remain unchanged in a chemical reaction are included in the ionic equation for the reaction are omitted in a net ionic equation
