Chapter 5 HW

Imagine that you were to conduct an experiment by placing an aluminum wire into a solution of nickel chloride:2 Al(s) + 3NiCl2(aq) What are the products of this reaction?

2AlCl3(aq) + 3 Ni(s)

(IN VIDEO) What will be the decomposition products for KClO3?

KCl(s) + O2(g) To Balance: 2KClO3(s) ---> 2KCl(s) + 3O2(g) (NOTE: This is a decomposition Reaction.)

Using what you have learned about the three forms of writing chemical equations, classify each of the presented equations as either a molecular equation, a complete ionic equation, or a net ionic equation. Drag the appropriate equations to their respective bins.

MOLECULAR EQUATION: Ba(NO3)2(aq)+K2SO4(aq)→BaSO4(s)+2KNO3(aq) CuSO4(aq)+2KOH(aq)→Cu(OH)2(s)+K2SO4(aq) COMPLETE IONIC EQUATION: Ag+(aq)+NO3−(aq)+I−(aq)+Na+(aq) →AgI(s)+NO3−(aq)+Na+(aq) Cu2+(aq)+SO42−(aq)+2K+(aq)+2OH−(aq)→Cu(OH)2(s)+2K+(aq)+ SO42−(aq) NET IONIC EQUATION: Ca2+(aq)+SO42−(aq)→CaSO4(s) Ba2+(aq)+SO42−(aq)→BaSO4(s)

(IN VIDEO) What will be the product when we react Mg(s) with O2(g) from the air?

MgO(s) (NOTE: This is a Combination Reaction: 2Mg (s) + O2 (g) --> 2MgO(s) )

The complete ionic equation you determined in Part C is shown above for your convenience. The net ionic equation only depicts the chemical species that participate in the reaction, and that is the formation of a solid between one type of cation and one type of anion in this precipitation reaction. Recall that any of the ions that do not participate in the reaction are spectator ions, and spectator ions are excluded from the net ionic equation. Write the net ionic equation for this precipitation reaction. Express your answer as a chemical equation including phases. Type an underscore (_) or a carat (^) to add subscripts and superscripts more quickly.

Zn2+(aq)+2OH−(aq)→Zn(OH)2(s) (NOTE: make sure to use subscript and superscripts and change the arrow on the format)

Identify the precipitate(s) of the reaction that occurs when a silver nitrate solution is mixed with a sodium chloride solution.

silver chloride (NOTE: AgNO3 + NaCl --> AgCl(s) + NaNO3 The AgCl(s) is the precipitation reaction)

A solution of hydrochloric acid is mixed with an equal volume solution of barium hydroxide. When pH paper is inserted into the resulting solution, the pH was determined to be 7.0. If the initial concentration of the hydrochloric acid solution was 0.5 MM, what is the concentration of the barium hydroxide solution?

0.25 M

What is the balanced chemical reaction between CH3OH and O2 to form CO2 and H2O?

2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) (NOTE: This is a Combustion Reaction.)

2NaOH(aq)+Zn(NO3)2(aq) → Zn(OH)2(s)+2NaNO3(aq) The molecular equation you determined in Part B is shown above for your convenience. Examine each of the chemical species involved to determine the ions that would be present in solution. Be sure to consider both the coefficients and subscripts of the molecular equation, and then write this precipitation reaction in the form of a balanced complete ionic equation. Express your answer as a chemical equation including phases. Type an underscore (_) or a carat (^) to add subscripts and superscripts more quickly.

2 Na+ (aq) + 2 OH- (aq) + Zn2+ (aq) + 2 NO3- (aq) -> Zn(OH)2 (s) + 2 Na+ (aq) + 2 NO3- (aq) (NOTE: make sure to use subscript and superscripts and change the arrow on the format)

A 1.0 MM solution of hydrochloric acid is mixed with an equal volume of sodium hydroxide solution. The resulting solution turns pH paper blue, meaning the solution is basic. Which of the following concentrations would be consistent with the experimental results for sodium hydroxide?

2.0 M

Identify the oxidizing agent and the reducing agent in each reaction below. Drag each label to the appropriate target.

2Al(s) is Reducing agent 3Cl2(g) is Oxidizing agent O2(g) is Oxidizing agent 2Mg(s) is Reducing agent

When aluminum, Al, metal is dipped in an aqueous solution of hydrochloric acid, HCl, hydrogen gas, H2H2, is produced with the formation of an aluminum chloride, AlCl3AlCl3, solution. Write the balanced chemical equation showing the phases of reactants and products. Express your answer as a chemical equation including phases.

2Al(s)+6HCl(aq)→2AlCl3(aq)+3H2(g) (NOTE: Write exactly like the above with subscripts)

Chromium metal is added to a solution of nickel(II) sulfate. What is the balanced chemical reaction?

2Cr(s) + 3NiSO4(aq) → Cr2(SO4)3 + 3Ni(s)

Aqueous sodium hydroxide was mixed with aqueous zinc(II) nitrate, and a crystallized zinc(II) hydroxide product was formed. A crystalized product is a solid. The other product, sodium nitrate, remains dissolved in solution. Consider the other product and its phase, and then write the balanced molecular equation for this precipitation reaction. Express your answer as a chemical equation including phases. Type an underscore (_) or a carat (^) to add subscripts and superscripts more quickly.

2NaOH(aq)+Zn(NO3)2(aq)→Zn(OH)2(s)+2NaNO3(aq) (NOTE: don't forget to use subscript)

Which of the following general reactions appropriately models a combination reaction?

A + B ---> C (NOTE: Because Combination reactions include elements combining to make a compound or compounds forming to form a new compound.)

Balance the chemical equation by indicating the number of each species in the appropriate blanks. For this exercise, indicate coefficients of 1 explicitly. Match the numbers in the left column to the appropriate blanks in the chemical equations on the right. Make certain the chemical equation is complete before submitting your answer.

ANSWER: 3Fe+4H2O→1Fe3O4+4H2

If you carry out the reaction between table salt (NaCl) and lead(II) iodide (PbI2PbI2 ) in 100.0 mL100.0 mL of water, the salt lead(II) iodide will behave similarly to the salts given in the tab named Slightly Soluble Salts. Enter the formula for the precipitate, without the phase, that will be formed. If no precipitate is formed, simply type "noreaction" in the answer box. Express your answer as a chemical formula.

ANSWER: PbCl2 (use subscript for the 2 on Cl) (NOTE: whole chemical formula: 2NaCl + PbI2 = PbCl2 + 2NaI)

Which of the following reactions would be classified as oxidation-reduction? Check all that apply.

ANSWERS: 2Na(s)+Cl2(g)→2NaCl(s) Na(s)+CuCl(aq)→NaCl(aq)+Cu(s)

Listed are examples of several types of chemical equations. Note that a combination reaction and a synthesis reaction are the same type of reaction. Each reaction is only partially balanced. Complete the task of balancing each chemical equation. Drag the appropriate labels to their respective targets.

Combustion: 3,3 Decomposition: 2,2 Single Replacement: 2,2 Double Replacement: 3,2 Combination: 2

We can also use the activity series to predict reactions between a metal and an acid. What are the products of the reaction Fe(s) + H2SO4(aq)?

FeSO4(aq) + H2(g)

Classify these elements by whether they get oxidized or reduced in the reactions shown here: Drag each item to the appropriate bin 2Ca(s)+O2(g) → 2CaO(s) F2(g)+2Li(s) → 2LiF(s)

Gets Oxidized: Calcium and Lithium Gets Reduced: Oxygen and Fluorine

Go to the Slightly Soluble Salts tab. Choose a salt from the dropdown menu to the right. Mouse over the salt shaker and move your mouse up and down while clicking the left mouse button to add the salt to the container of water. You can also add and remove water from the container by moving the sliders on the faucets to the left of the container back and forth. Notice that there is a table indicating the number of dissolved and bound (solid) ions to the right under the dropdown menu. Using the data in this table, enter the chemical formula of mercury(II) bromide. Express your answer as a chemical formula.

HgBr2 (NOTE: make sure the 2 on BR is a subscript)

Making sure the default volume of water is 1.00×10−16 L when using the Slightly Soluble Salts tab, add each of the possible salts to the water. Observe how much salt dissolves before the solution becomes saturated. Arrange the following salts according to their solubility in water.

Most Soluble to Least Soluble: Silver arsenate, copper(I) iodide, silver bromide, thallium(I) sulfide.

Which reaction is a decomposition reaction?

NH4NO3(s) → N2O(g) + H2O(g) (NOTE: Decomposition reactions are when complex molecules breakdown into more simpler components, molecules or elements.)

Silver metal is added to a solution of lead(II) nitrate. What is the balanced chemical reaction?

No reaction occurs.

The following equation is not balanced: CaSO4+AlCl3→CaCl2+Al2(SO4)3 Notice that "SO4" appears in two different places in this chemical equation. SO 2−4− is a polyatomic ion called sulfate . What number should be placed in front of CaSO4 to give the same total number of sulfate ions on each side of the equation? ?CaSO4+AlCl3→CaCl2+Al2(SO4)3

PART A: Express your answer numerically as an integer. ANSWER: 3 PART B: Now that we have put a coefficient of 3 in front of CaSO4, what coefficient should go in front of CaCl2CaCl2 to balance calcium (CaCa )? 3CaSO4+AlCl3→?CaCl2+Al2(SO4)3 PART B: Express your answer numerically as an integer. ANSWER: 3 (note: By placing a coefficient of 3 in front of calcium chloride, we have indicated 3 calcium atoms on the right to match the 3 calcium ions on the left: 3CaSO4+AlCl3→3CaCl2+Al2(SO4)3 ) PART C: Now that we have put a coefficient of 3 in front of CaSO4C and a coefficient of 3 in front of CaCl2, what coefficient should go in front of AlCl3AlCl3 to balance both the Cl atoms and the Al atoms? 3CaSO4+?AlCl3→3CaCl2+Al2(SO4)3 Express your answer numerically as an integer. ANSWER: 2 (NOTE: There are now 6 chlorine atoms and 2 aluminum atoms on each side of the equation. The final balanced equation looks like this: 3CaSO4+2AlCl3→3CaCl2+Al2(SO4)3)

Which of the following equations are balanced?

Part A: HCl+KOH→H2O+KCl ANSWER: balanced Part B: CH4+Cl2→CH2Cl2+HCl ANSWER: not balanced Part C: H2O+MgO→Mg(OH)2 ANSWER: balanced Part D: CO2+4H2→CH4+2H2O ANSWER: balanced

Identify the precipitation reactions. Drag the appropriate items to their respective bins.

Precipitation reactions: -Ba(NO3)2 + K2SO4 --> BaSO4+2KNO3 -2KCl+Pb(NO3)2 --> PbCl2+2KNO3 -Hg2(C2H3O2)2+2NBr--> Hg2Br2+2NaC2H3O2 Non-precipitation reactions: -H2O2+NaIo --> NaI+H2O+O2 -C+O2--> CO2 -HCl+LiOH--> LiCl+H2O -HBr+LiOH--> LiBr+H2O

Determine if each compound shown is soluble or insoluble. Drag the appropriate items to their respective bins.

SOULBLE:MnCl2, Cu(NO3)2, LiNO3, RbCl, LiBr, BaCl2 INSOLUBLE: Hg2I2, Mn(OH)2, BaSO4

Which one of the following is a diprotic acid?

sulfuric acid

A neutralization reaction between an acid and a metal hydroxide produces

water and a salt