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Q:
Which of the following concerning a barometer or manometer is/are true?
1) Pressure is directly proportional to the height of the liquid used in the device.
2) Pressure is directly proportional to the density of the liquid used in the device.
3) Pressure is independent of the acceleration of gravity.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
Q:
The net ionic equation for the reaction between aqueous ammonia and hydrobromic acid isA) HBr(aq) + NH3(aq) → NH4Br(aq).B) H+(aq) + OH-(aq) → H2O(l).C) HBr(aq) + OH-(aq) → Br-(aq) + H2O(l).D) H+(aq) + NH3(aq) → NH4+(aq).E) H+(aq) + Br-(aq) + NH3(aq) → NH4+(aq) + Br-(aq).
Q:
What is the net ionic equation for the reaction of hydrobromic acid with sodium hydroxide?A) H+(aq) + OH-(aq) → H2O(l)B) H+(aq) + Br-(aq) + Na+(aq) + OH-(aq) → NaBr(aq) + H2O(l)C) H+(aq) + Br-(aq) + Na+(aq) + OH-(aq) → HBr(aq) + NaOH(aq)D) HBr(aq) + Na+(aq) + OH-(aq) → NaBr(aq) + H2O(l)E) HBr(aq) + NaOH(aq) → NaBr(aq) + H2O(l)
Q:
What is the net ionic equation for the neutralization of hydrofluoric acid with sodium hydroxide?A) H+(aq) + NaOH(aq) → H2O(l) + Na+(aq)B) HF(aq) + OH-(aq) → H2O(l) + F-(aq)C) HF(aq) + NaOH(aq) → H2O(l) + NaF(aq)D) H+(aq) + OH-(aq) → H2O(l)E) HF(aq) + OH-(aq) → H2F+(aq) + O2-(aq)
Q:
What is the net ionic equation for the complete neutralization of phosphoric acid with potassium hydroxide?A) H3PO4(aq) + 3OH-(aq) → 3H2O(l) + PO43-(aq)B) H3P(aq) + 3KOH(aq) → 3H2O(l) + K3P(aq)C) H+(aq) + OH-(aq) → H2O(l)D) H3PO4(aq) + 3KOH(aq) → 3H2O(l) + K3PO4(aq)E) 3H+(aq) + 3KOH(aq) → 3H2O(l) + 3K+(aq)
Q:
Which of the following salts cannot be obtained by the neutralization of a strong acid and a strong base?A) NaClB) LiNO3C) NH4BrD) Ba(ClO4)2E) Na2SO4
Q:
What is the net ionic equation for the completeneutralization of the triprotic acid citric acid, H3C6H5O6, by a strong base?A) H3C6H5O6(aq) + 3OH-(aq) → 3H2O(l) + C6H5O63-(aq)B) H3C6H5O6(aq) + 3NaOH(aq) → 3H2O(l) + Na3C6H5O6(aq)C) H+(aq) + OH-(aq) → H2O(l)D) H3C6H5O6(aq) + NaOH(aq) → H2O(l) + NaH2C6H5O6(aq)E) 3H+(aq) + 3OH-(aq) → 3H2O(l)
Q:
Which of the following salts may be obtained by the reaction of a weak acid with a strong base?
A) LiClO4
B) NaCl
C) K2SO3
D) MgCl2
E) NH4F
Q:
What is the net ionic equation for the acid"base reaction that occurs when an excess of a potassium hydroxide solution is added to a solution of H2SeO3?A) H2SeO3(aq) + 2OH-(aq) → 2H2O(l) + SeO32-(aq)B) H+(aq) + OH-(aq) → H2O(l)C) 2H+(aq) + 2OH-(aq) → 2H2O(l)D) 2H+(aq) + SeO32-(aq) + 2K+(aq) + 2OH-(aq) → 2K+(aq) + SeO32-(aq) + 2H2O(l)E) H2SeO3(aq) + 2KOH(aq) → K2SeO3(aq) + 2H2O(l)
Q:
What is the net ionic equation for the acid"base reaction between chlorous acid and sodium hydroxide?A) H+(aq) + ClO2-(aq) + Na+(aq) + OH-(aq) → NaClO2(aq) + H2O(l)B) HClO2(aq) + OH-(aq) → ClO2-(aq) + H2O(l)C) HClO2(aq) + NaOH(aq) → NaClO2(aq) + H2O(l)D) H+(aq) + OH-(aq) → H2O(l)E) H+(aq) + ClO2-(aq) + Na+(aq) + OH-(aq) → Na+(aq) + ClO2-(aq) + H2O(l)
Q:
What is the net ionic equation for the reaction of NH3with HClO4?A) NH3(aq) + H+(aq) → NH4+(aq)B) NH3(aq) + HClO4(aq) → NH4ClO4(aq)C) NH3(aq) + ClO4-(aq) → NH2-(aq) + HClO4(aq)D) H-(aq) + H+(aq) → H2(g)E) H+(aq) + OH-(aq) → H2O(l)
Q:
What is the net ionic equation for the reaction of acetic acid, CH3COOH, with NH3?A) CH3COOH(aq) + NH3(aq) → NH4+(aq) + CH3COO-(aq)B) H+(aq) + OH-(aq) → H2O(l)C) CH3COOH(aq) + NH3(aq) → NH4CH3COO(aq)D) CH3COO-(aq) + H+(aq) + NH3(aq) → NH4CH3COO(aq)E) H+(aq) + NH3(aq) → NH4+(aq)
Q:
What is the net ionic equation for the acid"base reaction that occurs when acetic acid and sodium hydroxide solutions are mixed?A) HC2H3O2(aq) + OH-(aq) → C2H3O2-(aq) + H2O(l)B) H+(aq) + OH-(aq) → H2O(l)C) H3O+(aq) + OH-(aq) → 2H2O(l)D) C2H3O2-(aq) + H+(aq) + Na+(aq) + OH-(aq) → Na+(aq) + C2H3O2-(aq) + H2O(l)E) HC2H3O2(aq) + NaOH-(aq) → NaC2H3O2-(aq) + H2O(l)
Q:
Which of the following is best described as an acid"base reaction?A) HNO3(aq) + NH3(aq) → NH4+(aq) + NO3-(aq)B) P4(s) + 3OH-(aq) + 3H3O(l) → PH3(g) + 3H2PO2-(aq)C) Cu(s) + H2S(g) → CuS(s) + H2(g)D) 2H2(g) + O2(g) → 2H2O(l)E) 2KClO3(aq) → 2KCl(s) + 3O2(g)
Q:
Which of the following is a strong acid in aqueous solution?A) HClOB) H3PO4C) HBrD) HNO2E) H3PO3
Q:
Which of the following is a weak acid in aqueous solution?
A) HClO4
B) HCl
C) H2SO4
D) HNO3
E) H2SO3
Q:
Which of the following is a weak base in aqueous solution?
A) H2CO3
B) Ba(OH)2
C) B(OH)3
D) LiOH
E) N2H4
Q:
Which of the following is a weak base in aqueous solution?
A) HOCl
B) LiOH
C) NH3
D) HBr
E) Ba(OH)2
Q:
Which of the following is a weak acid in aqueous solution?
A) HCl
B) H2SO4
C) H2S
D) HNO3
E) HI
Q:
Which of the following is a weak electrolyte in aqueous solution?
A) Mg(OH)2
B) NH3
C) LiOH
D) RbOH
E) Sr(OH)2
Q:
Which of the following is a weak electrolyte in aqueous solution?
A) HClO4
B) H2SO4
C) H3PO4
D) HNO3
E) HI
Q:
All of the following are weak electrolytes in aqueous solution exceptA) acetic acid.B) tartaric acid.C) nitric acid.D) citric acid.E) nitrous acid.
Q:
Which of the following is a strong electrolyte in aqueous solution?
A) tartaric acid
B) ascorbic acid
C) hypochlorous acid
D) citric acid
E) hydroiodic acid
Q:
Which of the following is a strong base in aqueous solution?
A) LiCl
B) CH3OH
C) LiOH
D) NH3
E) HClO4
Q:
Which of the following is not a strong base in aqueous solution?A) Sr(OH)2B) Ca(OH)2C) KOHD) LiOHE) NH3
Q:
Which of the following is a strong acid in aqueous solution?
A) H3PO3
B) H3PO4
C) H2CO3
D) H2SO3
E) H2SO4
Q:
All the following are strong acids in aqueous solution exceptA) HCl.B) HF.C) HI.D) HBr.E) H2SO4.
Q:
Which of the following is a strong acid in aqueous solution?A) HOCH2CH2OHB) Ba(OH)2C) CH3COOHD) NH3E) HClO4
Q:
Which of the following is a strong base in aqueous solution?
A) HOCH2CH2OH
B) Ba(OH)2
C) H3PO4
D) NH3
E) HI
Q:
Which of the following is a weak base in aqueous solution?
A) HOCH2CH2OH
B) Ba(OH)2
C) CH3COOH
D) NH3
E) HI
Q:
Which of the following is not a strong acid in aqueous solution?A) HBrB) HClO4C) HFD) HIE) HCl
Q:
Which of the following reactions best describes the acid"base properties of acetic acid (HC2H3O2) in aqueous solution?A) HC2H3O2(aq) + H2O(l) → H3O+(aq) + C2H3O2-(aq)B) HC2H3O2(aq) + H2O(l) → C2H5O2+(aq) + OH-(aq)C) HC2H3O2(aq) + H2O(l) C2H5O2+(aq) + OH-(aq)D) HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2-(aq)E) HC2H3O2(aq) + 4H2O(l) 4H3O+(aq) + C2O24-(aq)
Q:
Which of the following reactions best describes the dissolution of gaseous hydrogen chloride (HCl) in water?A) HCl(g) + 2H2O(l) → H3O+(aq) + ClO-(aq) + H2(g)B) 2HCl(g) → H2(g) + Cl2(g)C) HCl(g) + H2O(l) → H3O+(aq) + Cl-(aq)D) HCl(g) + 5H2O(l) → H3O+(aq) + ClO4-(aq) + 4H2(g)E) HCl(g) + H2O(l) → H3O+(aq) + ClO-(aq)
Q:
Which of the following reactions best describes the acid-base properties of ammonia (NH3) in aqueous solution?A) NH3(aq) + 3H2O(l) → N3-(aq) + 3H3O+(aq)B) NH3(aq) → N3-(aq) + 3H+(aq)C) NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)D) NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq)E) NH3(aq) + 3H2O(l) N3-(aq) + 3H3O+(aq)
Q:
Which of the following chemical equations best represents the dissolution of a soluble group 2A metal hydroxide in water?A) M(OH)2(s) → M+(aq) + (OH)2-(aq)B) M(OH)2(s) → M2+(aq) + 2OH-(aq)C) M(OH)2(s) + H2O(l) → MO(aq) + OH-(aq) + H3O+(aq)D) M(OH)2(s) → M(OH)2(aq)E) M(OH)2(s) → MO(aq) + H2O(l)
Q:
Which of the following reactions best describes the dissolution of solid KOH(s) in water?A) KOH(s) + H2O(l) → KO-(aq) + H3O+(aq)B) KOH(s) → KO-(aq) + H+(aq)C) KOH(s) → K+(aq) + OH-(aq)D) KOH(s) → KO+(aq) + H-(aq)E) KOH(s) → KOH(aq)
Q:
Which of the following concerning acid-base reactions is/are correct?
1) Only strong acids and strong bases will undergo an acid-base reaction.
2) All acid-base reactions produce water and an ionic compound (salt) as a product.
3) All reactions that form a gas are also acid-base reactions.
A) 1 only
B) 2 only
C) 3 only
D) 1, 2, and 3
E) none
Q:
Which of the following combinations will result in an acid-base reaction?
1) AgNO3(aq) and HCl(aq)
2) HCl(aq) and Na2CO3(aq)
3) NaOH(aq) and K3PO4(aq)
A) 1 only
B) 2 only
C) 3 only
D) 1, 2, and 3
E) none
Q:
Which of the following may be classified as an acid-base reaction?1) AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)2) 2Mg(s) + O2(g) → 2MgO(s)3) Zn(s) + 2Ag+(aq) → 2Ag(s) + Zn2+(aq)A) 1 onlyB) 2 onlyC) 3 onlyD) 1, 2, and 3E) none
Q:
Which of the following is not an Arrhenius base?A) NH3B) KOHC) Ba(OH)2D) Ca(OH)2E) all are Arrhenius bases
Q:
What products result from mixing aqueous solutions of Cu(C2H3O2)2(aq) and Rb3PO4(aq)?A) Cu2PO4(s) and Rb3(C2H3O2)2(aq)B) Cu3(PO4)2(s) and RbC2H3O2(s)C) CuP(s), CO2(g), H2O(l), RbOH(aq), and PH3(g).D) CuPO4(s) and Rb3(C2H3O2)2(aq)E) Cu3(PO4)2(s), Rb+(aq), and C2H3O2-(aq)
Q:
What products result from mixing aqueous solutions of Ni(NO3)2(aq) and NaNO3(aq)?A) Ni(OH)2(s), Na+(aq), and NO3-(aq)B) Ni(OH)2(s) and NaNO3(s)C) Ni2(OH)2(aq) and NaNO3(aq)D) Ni(OH)2(aq) and NaNO3(s)E) Ni(OH)2(s), N2(g), and H2O(l)
Q:
Which net ionic equation best represents the reaction that occurs when an aqueous solution of barium chloride is mixed with an aqueous solution of lithium sulfate?A) 2H+(aq) + 2Cl-(aq) → 2HCl(g)B) Ba2+(aq) + SO42-(aq) → BaSO4(s)C) Ba2+(aq) + 2Cl-(aq) + 2Li+(aq) + SO42-(aq) → BaSO4(s) + 2LiCl(aq)D) BaCl2(aq) + Li2SO4(aq) → BaSO4(s)+ 2LiCl(aq)E) No net reaction occurs.
Q:
Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct?
A) CuS will precipitate from solution.
B) NaCl will precipitate from solution.
C) No precipitate will form.
D) Both NaCl and CuS will precipitate from solution.
E) No reaction will occur.
Q:
When solutions of barium chloride and lithium sulfate are mixed, the spectator ions in the resulting reaction areA) only SO42-.B) both Li+and Cl-.C) only Cl-D) only Li+.E) only Ba2+.
Q:
When a solution of lithium chloride and a solution of ammonium sulfate are mixed,
A) a new salt is formed.
B) no reaction occurs.
C) a precipitate forms.
D) an acid and a base are formed.
E) a gas is evolved.
Q:
A precipitate will form when a freshly prepared aqueous carbonic acid solution is added to an aqueous solution ofA) potassium carbonate.B) ammonium chloride.C) nitrous acid.D) calcium hydroxide.E) sodium chloride.
Q:
Which of the following are classified as precipitation reactions?1) AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)2) 2Mg(s) + O2(g) → 2MgO(s)3) Zn(s) + 2Ag+(aq) → 2Ag(s) + Zn2+(aq)A) 1 onlyB) 2 onlyC) 3 onlyD) 2 and 3E) 1, 2, and 3
Q:
Which of the following combinations will produce a precipitate?
1) AgNO3(aq) and HCl(aq)
2) HCl(aq) and Na2CO3(aq)
3) NaOH(aq) and K3PO4(aq)
A) 1 only
B) 2 only
C) 3 only
D) 2 and 3
E) 1, 2, and 3
Q:
Which of the following concerning precipitation reactions is/are correct?
1) A precipitation reaction is a type of chemical reaction that forms a gaseous product (such as CO2).
2) A precipitation reaction is possible when two or more aqueous solutions of strong or weak electrolytes are mixed.
3) Only ionic compounds will react to form precipitates in a precipitation reactions.
A) 1 only
B) 2 only
C) 3 only
D) 2 and 3
E) 1, 2, and 3
Q:
A precipitate is expected when an aqueous solution of potassium iodide is added to an aqueous solution of
A) calcium nitrate.
B) barium hydroxide.
C) lead perchlorate.
D) iron(II) chloride.
E) sodium sulfate.
Q:
Which net ionic equation best represents the reaction that occurs when an aqueous solution of lithium nitrate is mixed with an aqueous solution of ammonium bromide?A) Li+(aq) + Br-(aq) →LiBr(s)B) NH4+(aq) + NO3-(aq) → NH4NO3(aq)C) NH4Br(aq) + LiNO3(aq) →LiBr(s) + NH4NO3(aq)D) No net reaction occurs.E) Li+(aq) + NH4Br(aq) →LiBr(s) + NH4+(aq)
Q:
Which equation best represents the net ionic equation for the reaction that occurs when aqueous solutions of potassium phosphate and iron(II) nitrate are mixed?A) 3Fe2+(aq) + 2PO43-(aq) →Fe3(PO4)2(s)B) 2K+(aq) + Fe(NO3)2(aq) →2KNO3(aq) + Fe2+(aq)C) 3Fe2+(aq) + 2PO43-(aq) →Fe3(PO4)2(aq)D) 2K3PO4(aq) + 3Fe2+(aq) → Fe3(PO4)2(s) + (K+)6(aq)E) 2K3PO4(aq) + 3Fe(NO3)2(aq) →Fe3(PO4)2(s) + 6KNO3(aq)
Q:
What precipitate forms when aqueous solutions of calcium bromide and potassium phosphate are mixed?A) (KBr)2(s)B) Ca3(PO4)2(s)C) CaPO4-(s)D) KBr(s)E) CaPO4(s)
Q:
Identify the spectator ion(s) in the following reaction.Zn(OH)2(s) + 2K+(aq) + 2OH-(aq) → 2K+(aq) + Zn(OH)4-(aq)A) K+and Zn(OH)42-B) K+C) Zn(OH)2D) Zn(OH)42-E) K+and OH-
Q:
Identify the spectator ion(s) in the following reaction.Cu(OH)2(s) + 2H+(aq) + 2Cl-(aq) → Cu2+(aq) + 2Cl-(aq) + 2H2O(l)A) Cu2+and Cl-B) Cu2+C) Cu(OH)2D) Cl-E) H+and Cl-
Q:
Which of the following would not be depicted as the individual ions on the reactant side of a complete ionic reaction?
A) LiOH
B) HCl
C) ZnBr2
D) CH3COOH
E) FeI3
Q:
Which of the following would not be depicted as the individual ions on the reactant side of a complete ionic reaction?
A) RbOH
B) HBr
C) Cu(NO3)2
D) CuCO3
E) Ti(NO3)3
Q:
Which of the following concerning molecular and ionic equations is/are correct?
1) Molecular equations cannot be written for reactions involving ionic substances.
2) Charge must be balanced in a properly balanced net ionic reaction.
3) In a balanced complete ionic reaction only the strong electrolytes are shown as the individual aqueous ions.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 2 and 3
Q:
Identify the spectator ions in the following reaction.Ca2+(aq) + 2NO3-(aq) + 2Na+(aq) + CO32-(aq) ->CaCO3(s) + 2Na+(aq) + NO3-(aq)A) NO3-and CO32-B) Ca2+and Na+C) Ca2+and CO32-D) Ca2+and NO3-E) Na+and NO3-
Q:
Which anion will form a precipitate with Ca2+?A) Cl-B) SO42-C) C2H3O2-D) Br-E) none of the above
Q:
Which anion will form a precipitate with Rb+?A) Cl-B) SO42-C) C2H3O2-D) S2-E) none of the above
Q:
A student is given a sample in lab that contains one of the ions listed below. After adding a few drops of AgNO3 solution to a portion of the unknown sample, the student observed a grayish precipitate. After adding a few drops of Mg(NO3)2 solution to another portion of the unknown sample, the student got a black precipitate. Based on these observations, what is the only possible ion in this student's sample?A) Cl-B) F-C) C2H3O2-D) S2-E) SO42-
Q:
Which of the following concerning electrolytes and the solubility rules is/are true?
1) The solubility rules apply only to ionic substances.
2) All soluble ionic compounds are considered strong electrolytes.
3) The solubility rules apply to aqueous and non-aqueous solutions.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
Q:
Which of the following compounds is insoluble in water?
A) NH4I
B) RbI
C) CuCl2
D) AgI
E) LiI
Q:
Which of the following compounds is soluble in water?
A) PbCl2
B) PbBr2
C) CaSO4
D) Ca(NO3)2
E) HgBr2
Q:
Which of the following compounds is insoluble in water?
A) Hg2SO4
B) FeSO4
C) Li2SO4
D) (NH4)2SO4
E) Cr2(SO4)3
Q:
Which of the following compounds is insoluble in water?
A) FeCO3
B) Li2CO3
C) (NH4)2CO3
D) K2CO3
E) Na2CO3
Q:
Which of the following compounds is soluble in water?
A) Ga2O3
B) Na3P
C) ZnS
D) Hg2Cl2
E) CdS
Q:
Which of the following ions is most likely to form an insoluble sulfate?A) Ca2+B) Cl-C) K+D) Li+E) S2-
Q:
Which of the following aqueous solutions would be expected to be the best conductor of an electric current at room temperature?A) 0.10 M CH3COOHB) 0.10 M HClC) 0.10 M Na2SO4D) 0.10 M NaClE) 0.10 M H3PO4
Q:
Which of the following solutes, dissolved in 1000 g of water, would provide the greatest number of particles?
A) 0.030 mol of urea, CO(NH2)2
B) 0.030 mol of ammonium nitrate, NH4NO3
C) 0.030 mol of barium chloride, BaCl2
D) 0.030 mol of acetic acid, CH3COOH
E) 0.030 mol of calcium sulfate, CaSO4
Q:
Which of the following solutions would be expected to be the best conductor of an electric current at room temperature?A) 0.10 M Na2SO4B) 1.0 M CH3COOHC) 0.10 M NaClD) 0.10 M CO(NH2)2E) 0.10 M CH3COOH
Q:
Which of the following is a nonelectrolyte in aqueous solution?
A) NH4F
B) NH4Cl
C) NaHS
D) CH4
E) Na2S
Q:
Which of the following correctly describes one or more of the differences between a strong and weak electrolyte?
A) A strong electrolyte partially ionizes in solution and a weak electrolyte completely ionizes in solution.
B) Strong electrolytes are all classified as soluble ionic substances and weak electrolytes are all classified as soluble molecular substances.
C) Strong electrolytes produce more ions per mole of substance in solution than weak electrolytes.
D) Weak electrolytes inhibit the flow of electricity.
E) Strong electrolytes are weak conductors of electricity.
Q:
Which of the following concerning electrolytes and nonelectrolytes is/are true?
1) Some molecular substances are electrolytes.
2) All electrolytes are ionic substances.
3) Strong electrolytes partially ionize in solution.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 2 and 3
Q:
An impure sample of benzoic acid (C6H5COOH, 122.12 g/mol) is titrated with 0.8067M NaOH. A 5.109-g sample requires 36.97mL of titrant to reach the endpoint. What is the percent by mass of benzoic acid in the sample?C6H5COOH(aq)+NaOH(aq)→NaC6H5COO(aq)+H2O(l)A) 0.02442 %B) 2.982 %C) 100.0 %D) 24.42 %E) 71.29 %
Q:
In a volumetric analysis experiment, an acidic aqueous solution of methanol (CH3OH) is titrated with a solution of potassium dichromate (K2Cr2O7) according to the following balanced chemical equation:2K2Cr2O7(aq) + 8H2SO4(aq) + 3CH3OH(aq) →2Cr2(SO4)3(aq) + 11H2O(l) + 3HCOOH(aq) + 2K2SO4(aq)It required 43.91mL of 0.0435M K2Cr2O7to reach the endpoint. What mass of CH3OH was present initially?A) 0.0918 gB) 2.09 gC) 0.929 gD) 0.0612 gE) 0.0408 g
Q:
In a volumetric analysis experiment, a solution of sodium oxalate (Na2C2O4) in acidic solution is titrated with a solution of potassium permanganate (KMnO4) according to the following balanced chemical equation:2KMnO4(aq) + 8H2SO4(aq) + 5Na2C2O4(aq) →2MnSO4(aq) + 8H2O(l) + 10CO2(g) + 5Na2SO4(aq) + K2SO4(aq)It required 25.0mL of 0.0448M KMnO4to reach the endpoint. What mass of Na2C2O4was present initially?A) 2.40 gB) 0.0600 gC) 15.0 gD) 0.150 gE) 0.375 g
Q:
A 40.00-mL sample of a weak base is titrated with 0.0935M HCl. At the endpoint, it is found that 32.87mL of titrant was used. What was the concentration of the weak base?A) 0.114 MB) 7.11 x10-5MC) 3.07 MD) 0.0935 ME) 0.0768 M