Chapter 4

What volume, in L, of a 0.00945-M solution of potassium hydroxide would be required to titrate 50.00 mL of a sample of acid rain with a H2SO4concentration of 0.000123 M.H2SO4(aq) + 2KOH(aq) --> K2SO4(aq) + 2H2O(l) MV= moles 0.000123M H2SO4 x 0.050L=6.15 x 10-6 mol H2SO4 mol-mol 6.15 x 10-6 mol H2SO4 x KOH/2H2SO4= 1.12 x 10-6 mol KOH Mol x L/mol 1.12 x 10-6 mol KOH x L/0.00945= ???????

0.00130 L KOH

What is the concentration of NaCl, in M, in a solution if titration of 15.00 mL of the solution with 0.150 M AgNO3 requires 12.25 mL of the AgNO3 solution to reach the end point?AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3 MV=mol 12.25ml x L/1000ml=0.01225L (0.150 M)( 0.01225 L)= 0.001838 mol AgNO3 mol-mol 0.001838 mol AgNO3 x NaCl/AgNO3= 0.001838 mol NaCl mol-M 15.00mL L/1000mL=0.010mL 0.001838 mol NaCl/0.01500mL= ???????

0.1225M NaCl

Urea, CO(NH2)2, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass, in Kilograms, of urea, CO(NH2)2[MM=62.07g/mol], that can be manufactured from 1.00kg of CO2.CO2(g) + 2NH3(g) --> CO(NH2)2(s) + H2O(l) 1.00 kg CO2 x 1000g/kg x mol /44.01g x CO(NH2)2/CO2 x 62.07g/mol x 1kg/1000g= ?????

1.41 kg CO(NH2)2

Gallium chloride is formed by the reaction of 2.25 L of a 1.50 M solution of HCl according to the following equation: 2Ga + 6HCl --> 2GaCl3 + 3H2Determine the mass of gallium chloride, in grams, produced. MV=mol (1.50 M)( 2.25 L)= 3.38 mol HCl mol-mol 3.38 mol HCl x 2GaCl3/6HCl= 1.13mol GaCl3 mol-g 1.13 mol GaCl3 x 176.10g/mol= 198g GaCl3 Or (1.50 M)( 2.25 L) x 2GaCl3/6HCl x 176.10g/mol= ????

198 g Ga

Calculate the mass of magnesium carbonate ( MgCO3), in grams, required to produce 110.0 g of carbon dioxide using the following equation: MgCO3 --> MgO + CO2 This is a three step problem g-mol 110.0gCO2 x mol/44.01g= 2.500mol O2 mol-mol 2.500mol CO2 x MgCO3/CO2= 2.500mol MgCO3 mol-g 2.500mol MgCO3x 84.31g/mol= 211g NaNO3 Or 110gCO2 x mol/44.01g x MgCO3/CO2 x 84.31g/mol= ?????

211 g MgCO3

Balance the following equation:Al(s) + H2SO4(aq) --> Al2(SO4)3(aq) + H2(g)

2Al(s) + 3H2SO4(aq) --> Al2(SO4)3(aq) + 3H2(g)

Balance the following equation:K(s) + H2O(l) --> KOH(aq) + H2(g

2K(s) + 2H2O(l) --> 2KOH(aq) + H2(g)

Match balanced equation described by the following .Solid potassium chlorate, KClO3, decomposes to form solid potassium chloride and diatomic oxygen gas.

2KClO3(s) --> 2KCl(s) + 3O2(g)

Match balanced equation described by the following .When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.

2NaCl(s) + H2SO4(ag) -->2HCl(g) + Na2SO4(aq)

Balance the following equation:Pb(s) + H2O(l) + O2(g) -->Pb(OH)2(s)

2Pb(s) + 2H2O(l) + O2(g) -->2Pb(OH)2(s)

What volume, in mL, of 0.600 M HCl is required to react completely with 2.50 g of sodium hydrogen carbonate?NaHCO3(aq) + HCl(aq) --> NaCl(aq) + CO2(g) + H2O(l) # 29 is a three step problem, with Liter/mL conversions added in, which can be combined into on long problem(see below). I find it easier to do titrations in multiple steps due to the variations in the volume conversions before and after the first and third steps. g-mol 2.50 g NaHCO3 x mol/84.01g= 0.0298mol NaHCO3 mol-mol 0.0298mol NaHCO3 x HCl/NaHCO3 = 0.0298mol HCl mol-L 0.0298mol HCl x L/0.600mol= 0.0496 L HCl 0.0496 L KI 1000mL/L=49.6mL I have notated where the molarity M=mol/L in red. g-mol 2.50 g NaHCO3 x mol/84.01g x HCl/NaHCO3 x L/0.600mol= 0.0496 L HCl 0.0496 L KI 1000mL/L= ??????????

49.6 mL HCl

Balance the following equationAl(s) + O2(g) --> Al2O3(s)

4Al(s) + 3O2(g) --> 2Al2O3(s)

What mass of silver oxide, Ag2O [MM=131.74g/mol],in grams, is required to produce 35.0 g of silver sulfadiazine, AgC10H9N4SO2(MM=357.14g/mol), from the reaction of silver oxide and sulfadiazine?2C10H10N4SO2 + Ag2O --> 2AgC10H9N4SO2 + H2O 35.0 g AgC10H9N4SO2 x mol /357.14g x Ag2O/2AgC10H9N4SO2x 131.74g/mol= ??????

6.46 g Ag2O

What volume, in mL, of a 0.100 M KI solution contains enough KI to react exactly with 15.25 mL of a 0.200 M solution of Cu(NO3)2?2Cu(NO3)2 + 4KI --> 2CuI + I2 + 4KNO3 This is a three step problem MV=mol 15.25ml x L/1000ml=0.01525L (0.200 M)( 0.01525 L)= 0.003050 mol Cu(NO3)2 mol-mol 0.003050 mol Cu(NO3)2 x 4KI/2Cu(NO3)2= 0.006100mol KI mol-L 0.006100mol KI x L/0.100mol= 0.0305 L KI 0.0305 L KI 1000mL/L= ??????

61.00 mL KI Solution

Calculate the mass of sodium nitrate( NaNO3), in grams, required to produce 128 g of oxygen, using the following equation: 2NaNO3 --> 2NaNO2 + O2 This is a three step problem g-mol 128gO2 x mol/32.00g= 4.00mol O2 mol-mol 4.00mol O2 x 2NaNO3/O2= 8.00mol NaNO3 mol-g 8.00mol NaNO3 x 85g/mol= 608g NaNO3 Or 128gO2 x mol/32.00g x 2NaNO3/O2 x 85.00g/mol= ??????

680 g NaNO3

Citric acid, C6H8O7, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction isC12H22O11 + H2O + 3O2 --> 2C6H8O7 + 4H2OUsing a metric ton(1000kg) of sucrose the expected yield is 1122Kg. On average if only 1036kg is produced, what is the % yield for this reaction?

92.3% yield

Balance the following equation:CH4(g) + O2(g) --> CO2(g) +H2O(l)

CH4(g) + 2O2(g) --> CO2(g) + 2H2O(l)

Determine the oxidation states of the elements in the compound listed.ClO4- total 7+ 8- =- Individual 7+ 2- Cl O4

Cl=7+, O=2-

Identify the atom that is oxidized/reduced and its oxidizing/reducing agent, in the following equation:Co(s) + 8HNO3(aq) --> 3Co(NO3)2(aq) + 2NO(g) + H2O(l)

Co is oxidized and Co(s) is the reducing agent Co0(s) + 8H1+N5+O2-3(aq) --> 3Co+2(N5+O2-3)2(aq) + 2N2+O2-(g) + H1+2O(l) Co0(s) --> Co2+ Oxidized 0 ->2+ Reducing agent=Co N5+-->N2+ Reduced 5+-->2+ Oxidizing agent=HNO3

Match balanced equation described by the following .Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.

H3PO4(aq) + KOH(aq) --> KH2PO4(aq) + H2O(l)

Determine the oxidation states of the elements in the compound listed.HNO3 total 1+ 5+ 6- =0 Individual 1+ 5+ 2- H N O3

H=1+, N=5+, O=2-

Determine the oxidation states of the elements in the compound listed.H2SO4 total 2+ 6+ 8- =0 Individual 1+ 6+ 2- H2 S O4

H=1+, S=6+, O=2-

What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following equation? 6Li + N2 --> 2Li3N

Li

Identify the atom that is oxidized/reduced and its oxidizing/reducing agent, in the following equation: PCl3(l) + Cl2(g) --> PCl5(s)

P is oxidized and PCl3(l) is the reducing agent P3+Cl31-(l) + Cl20(g) --> P5+Cl1-5(s) P3+(l) --> P5+(s) Oxidized 3+ ->5+ Reducing agent=PCl3 Cl20(g) -->Cl1-5(s) Reduced 0-->1- Oxidizing agent=Cl2(g)

Balance the following equation:P4(s) + Cl2(g) --> PCl5(l)

P4(s) + 10Cl2(g) --> 4PCl5(l)

Identify the atom that is oxidized/reduced and its oxidizing/reducing agent, in the following equation: Zn(s) + H2SO4(aq) --> ZnSO4(aq) + H2(g)

Zn is oxidized and Zn(s) is the reducing agent Zn0(s) + H1+2S6+O2-4(aq) --> Zn2+S6+O2-4(aq) + H02(g) Zn0(s) --> Zn2+ Oxidized 0 ->3+ Reducing agent=Zn H1+-->H02(g) Reduced 1+-->0 Oxidizing agent=H2(g)

Indicate the type of reaction represented:Al(OH)3(aq) + 3HCl(aq) --> AlBr3(aq) + H2O(l)

acid-base (neutralization)

Indicate the type of reaction represented:O2(g) + 2C(s) --> 2CO(g)

oxidation-reduction (combustion)

Indicate the type of reaction represented:2KClO3(s) --> 2KCl(s) + 3O2(g)

oxidation-reduction;

Indicate the type of reaction represented:Pb(NO3)2(aq) + H2SO4(aq) --> PbSO4(s) + 2 HNO3(aq)

precipitation