chap 4

Which element is oxidized in this reaction? Fe2O3+3CO→2Fe+3CO2 Enter the chemical symbol of the element.

C

Which one of the following compounds is a nonelectrolyte?

C2H5OH

What is the net ionic equation of the reaction of MgCl2 with NaOH?

Mg2+(aq)+2OH−(aq)→Mg(OH)2(s)

Which element is reduced in this reaction? 2KMnO4+3Na2SO3+H2O→2MnO2+3Na2SO4+2KOH

Mn

What is the oxidation state of each individual carbon atom in C2O42−?

+3

What is the oxidation number of Cr in the Cr2O7 2− ion?

+6

What is the oxidizing agent of the following redox reaction? H2O + HNO2 + 3 H2SO3 → NH3 + 3 H2SO4

HNO2

What is the net ionic equation of the reaction of MgSO4 with Pb(NO3)2?

Pb2+(aq)+SO42−(aq)→PbSO4(s)

The name of HClO4 is _____.

perchloric acid

A 0.100 M solution of K2SO4 would contain the same total ion concentration as which of the following solutions?

0.0750 MNa3PO4

What is the oxidation state of an individual sulfur atom in SO32−? Express the oxidation state numerically (e.g., +1).

+4

In a neutral compound, the sum of the oxidation states is zero. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In H2O, for example, each hydrogen atom has an oxidation state of +1 and each oxygen atom has an oxidation state of −2 for a total of 2(+1)+(−2)=0. What is the oxidation state of an individual sulfur atom in BaSO4? Express the oxidation state numerically (e.g., +1).

+6

What is the oxidation state of an individual nitrogen atom in NH2OH?

-1

What is the concentration of K+ ions in a 0.025 M K2CO3 solution assuming complete dissociation? Express the concentration in molarity.

0.050

What are the coefficients of the six species in the balanced equation above? Remember to include coefficients for H2O(l) and H+(aq) in the appropriate blanks.

1,3,6,1,3,3

Given the partial equation ? MnO4−+ ? Fe2+ → ? Mn2++ ? Fe3+ what must the coefficients be so that the electrons are balanced?

1,5,1,5

What are the coefficients of the six species in the balanced equation above? Remember to include coefficients for H2O(l) and OH−(aq) in the blanks where appropriate.

2,3,1,2,3,2

What is the correct net ionic equation, including all coefficients, charges, and phases, for the following set of reactants? Assume that the contribution of protons from H2SO4 is near 100 %. Ba(OH)2(aq)+H2SO4(aq)→

2H+(aq)+2OH−(aq)+Ba2+(aq)+SO42−(aq)→2H2O(l)+BaSO4(s)

Given the equation MnO4−+5Fe2+→Mn2++5Fe3+ how many H2O molecules should be added to the right side of the equation to balance the oxygen atoms?

4

What is the total molar concentration of ions in a 0.90 M Al2 (SO4)3 solution?

4.5 M

Given the equation MnO4−+5Fe2+→Mn2++5Fe3++4H2O how many H+ ions should be added to the left side to balance the hydrogen atoms?

8

Look again at the table in Part B, repeated below. Solid Concentration (M) Strength of light emitted A 0.20 Bright B 0.20 Dim C 0.20 None D 0.20 Bright The student is told that one of the four solids tested is actually calcium bromide ,CaBr2. Which of the solids could be CaBr2?

A,D

magine that A and B are cations and X, Y, and Z are anions, and that the following reactions occur: AX(aq)+BY(aq)→no precipitate AX(aq)+BZ(aq)→precipitate Which of the following choices is insoluble?

AZ

Classify these compounds as acid, base, salt, or other. Drag the appropriate items to their respective bins.

Acid: HCOOH, HNO3 Base: NaOH, NH3 Salt: NaBr, KCl Other: CO2, CH3CH3

According to the activity series, which one of the following metals cannot replace the Cu2+ ion in solution?

Ag

enter the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate.

Ag+(aq)+Cl−(aq)→AgCl(s)

A student tests four solids for their ability to complete an electrical circuit when dissolved in water by observing their ability to close a circuit containing a light bulb and obtains the following results: Solid Concentration (M) Strength of light emitted A 0.20 Bright B 0.20 Dim C 0.20 None D 0.20 Bright Which of the solids is a weak electrolyte when dissolved in water?

B

What is(are) the precipitate(s) that form when K2SO4, BaCl2, and AgNO3 solutions are mixed?

BaSO4 and AgCl

The electrical conductivities of the following 0.100 M solutions were measured in an apparatus that contained a light bulb as the indicator of conductivity. Rank the solutions in order of decreasing intensity (brightest to dimmest) of the light bulb. Rank from brightest to dimmest bulb. To rank items as equivalent, overlap them.

Brightest to dimmest : Al(NO3)3, KI, HF, CH3OH

When the following reaction occurs: H3PO4(aq)+Ca(OH)2(aq)→ what is the formula for the salt formed?

Ca3(PO4)2

Which of the following would you least expect to find in CaCl2(aq)?

CaCl2 molecules

The student is now told that the four solids, in no particular order, are calcium bromide (CaBr2), sugar (C6H12O6), butanoic acid (C3H7COOH), and sodium bromide (NaBr). Assuming that conductivity is correlated to the number of ions in solution, rank the four substances based on how well a 0.20 M solution in water will conduct electricity. Rank from most conductive to least conductive. To rank items as equivalent, overlap them.

Calcium bromide, sodium bromide, butanoic acid, sugar

Here is a more complex redox reaction involving the dichromate ion in acidic solution: 3NO2− + 8H+ + Cr2O72− → 3NO3− +2Cr3+ + 4H2O Classify each reactant as the reducing agent, oxidizing agent, or neither. Drag the appropriate items to their respective bins.

Cr2O7^2- is the oxidizing agent NO2^- is the reducing agent H^+ is neither

Which substance is the oxidizing agent in this reaction? Fe2O3+3CO→2Fe+3CO2

Fe2O3 is the oxidizing agent.

What is the net ionic equation for the following reaction? HNO2 (aq) + KOH(aq) → H2O(l) + KNO2 (aq)

HNO2 (aq) + OH−(aq) → H2O(l) + NO2 −(aq)

Classify the following reactions. HNO3(aq)+NH3(aq)→NH4NO3(aq) 2Cu(s)+O2(g)→2CuO(s) NaCl(aq)+AgNO3(aq)→NaNO3(aq)+AgCl(s) 2LiOH(aq)+H2SO4(aq)→Li2SO4(aq)+2H2O(l) CaCl2(aq)+K2CO3(aq)→2KCl(aq)+CaCO3(s)

HNO3(aq)+NH3(aq)→NH4NO3(aq) neutralization 2Cu(s)+O2(g)→2CuO(s) redox NaCl(aq)+AgNO3(aq)→NaNO3(aq)+AgCl(s) precipitation 2LiOH(aq)+H2SO4(aq)→Li2SO4(aq)+2H2O(l) neutralization CaCl2(aq)+K2CO3(aq)→2KCl(aq)+CaCO3(s) precipitation

Insoluble sulfide compounds are generally black in color. Which of the following combinations could yield a black precipitate?

Li2S(aq)+Pb(NO3)2(aq), K2S(aq)+Sn(NO3)4(aq)

Which substance is the reducing agent in this reaction? 2KMnO4+3Na2SO3+H2O→2MnO2+3Na2SO4+2KOH

Na2SO3

Watch the animation, then check off the samples that will conduct electricity.

NaCl solution

Consider the diagram. (Figure 1) The yellow spheres represent the cation and the red spheres the anion Which of the following combinations of reactants could the diagram represent?

Pb2+(aq)+2I−(aq)→

When the following two solutions are mixed: K2CO3(aq)+Fe(NO3)3(aq) the mixture contains the ions listed below. Sort these species into spectator ions and ions that react.

Spectator ions K+, NO3 IONs, Fe3+, (CO3)2-

Classify each of these soluble solutes as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. Solutes Formula Hydrochloric acid HCl Sodium hydroxide NaOH Hydrofluoric acid HF Methyl amine CH3NH2 Aluminum chloride AlCl3 Methanol CH3OH Glucose C6H12O6 Drag the appropriate items to their respective bins.

Strong : hydrochloric acid, sodium hydroxide, aluminum chloride Weak: hydrofluoric acid, metyll amine non electrolyte: glucose, methanol

Substance X is a molecular compound and is not an acid nor a base. Based just on this information, what can you determine about substance X?

X is not an electrolyte.

Which of the following reactions could be used to produce hydrogen gas?

Zn(s)+HCl(aq)→

Suppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound or compounds that precipitate? Enter the name of the precipitate.

barium carbonate

Each of the following reactions shows a solute dissolved in water. Classify each solute as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. A(l)→A(aq) BC(aq)⇌B+(aq)+C−(aq) DE(aq)→D+(aq)+E−(aq) XY(s)→X+(aq)+Y−(aq) Z(s)→Z(aq) Drag the appropriate items to their respective bins.

in order Non electrolyte Weak electrolyte Strong electrolyte Strong electrolyte Non electrolyte

For the given reactions, classify the reactants as the reducing agent, oxidizing agent, or neither. N2 + 3H2 → 2NH3 2S + 3O2 → 2SO3

oxidizing agent N2, O2 Reducing agent S, H2

Classify the following reactions: HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l) Ba(OH)2(aq)+ZnCl2(aq)→BaCl2(aq)+Zn(OH)2(s) 2AgNO3(aq)+Mg(s)→Mg(NO3)2(aq)+2Ag(s) Drag the appropriate items to their respective bins.

precipitation B Acid base A oxidation reduction C

Which of the following situations is most favorable for solubility?

strong attraction of solute particles to solvent particles