Deck 4: Aqueous Reactions and Solution Stoichiometry

Question 1

Which of the following is soluble in water at 25°C?

A) Fe(NO₃)₂
B) FeS
C) Fe(OH)₂
D) Fe₃(PO₄)₂
E) FeCO₃

Answer 1

Fe(NO₃)₂

Question 2

An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g) of KOH was in the original sample?

A) 1.6
B) 0.21
C) 7.2
D) 0.17
E) 0.42

Answer 2

0.21

Question 3

What mass (g) of potassium chloride is contained in 430 mL of a potassium chloride solution that has a chloride ion concentration of 0.193 M?

A) 12.37
B) 6.19
C) 0.0830
D) 0.0643
E) 0.386

Answer 3

6.19

Question 4

Zinc is more active than cobalt and iron but less active than aluminum. Cobalt is more active than nickel but less active than iron. Which of the following correctly lists the elements in order of increasing activity?

A) Ni < Co < Fe < Zn < Al
B) Zn < Al < Co < Ni < Fe
C) Ni < Fe < Co < Zn < Al
D) Fe < Ni < Co < Al < Zn
E) Co < Ni < Fe < Zn < Al

Question 5

Which combination will produce a precipitate?

A) NaOH (aq) and HCl (aq)
B) AgNO₃ (aq) and Ca(C₂H₃O₂)₂ (aq)
C) NaC₂H₃O₂ (aq) and HCl (aq)
D) KOH (aq) and Mg(NO₃)₂ (aq)
E) NaOH (aq) and HCl (aq).

Question 6

The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is .

A) 2H⁺ (aq) + SO₄^2- (aq) + 2Na⁺ (aq) + 2OH^- (aq) - 2H₂O (l) + 2Na⁺ (aq) + SO₄^2- (aq)
B) 2H⁺ (aq) + 2OH^- (aq) - 2H₂O( l)
C) SO₄^2- (aq) + 2Na⁺ (aq) - 2Na⁺ (aq) + SO₄^2- (aq)
D) H⁺ (aq) + HSO₄^- (aq) + 2OH^- (aq) - 2H₂O (l) + SO₄^2- (aq)
E) H⁺ (aq) + HSO₄^- (aq) + 2Na⁺ (aq) + 2OH^- (aq) - 2H₂O (l) + 2Na⁺ (aq) + SO₄^2- (aq)

Question 7

When aqueous solutions of are mixed, a precipitate forms.

A) NaI and KBr
B) KOH and Ba(NO₃)₂
C) K₂SO₄ and CrCl₃
D) Li₂CO₃ and CsI
E) NiBr₂ and AgNO₃

Question 8

Which solution contains the largest number of moles of chloride ions?

A) 4.00 mL of 1.000M NaCl
B) 25.00 mL of 0.400M KCl
C) 10.0 mL of 0.500M BaCl₂
D) 30.00 mL of 0.100M CaCl₂
E) 7.50 mL of 0.500M FeCl₃

Question 9

What are the respective concentrations (M) of Fe³⁺ and I^- afforded by dissolving 0.200 mol FeI₃ in water and diluting to 725 mL?

A) 0.276 and 0.276
B) 0.276 and 0.828
C) 0.145 and 0.0483
D) 0.828 and 0.276
E) 0.145 and 0.435

Question 10

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200. mL to make a 1.50 M solution of sodium hydroxide?

A) 0.800
B) 800
C) 45
D) 50.0
E) 0.05

Question 11

The point in a titration at which the indicator changes is called the .

A) endpoint
B) equivalence point
C) indicator point
D) standard point
E) volumetric point

Question 12

A 36.3 mL aliquot of 0.0529 M H₂SO₄ (aq) is to be titrated with 0.0411 M NaOH (aq). What volume (mL) of base will it take to reach the equivalence point?

A) 1.92
B) 3.84
C) 93.6
D) 187
E) 46.8

Question 13

Of the reactions below, only is not spontaneous.

A) Mg (s) + 2HCl (aq) - MgCl₂ (aq) + H₂ (g)
B) 2Ni (s) + H₂SO₄ (aq) -Ni₂SO₄ (aq) + H₂ (g)
C) 2Ag (s) + 2HNO₃ (aq) - 2AgNO₃ (aq) + H₂ (g)
D) Zn (s) + 2HI (aq) - ZnI₂ (aq) + H₂ (g)
E) 2Al (s) + 6HBr (aq) - 2AlBr₃ (aq) + 3H₂ (g)

Question 14

In which reaction does the oxidation number of hydrogen change?

A) CaO (s) + H₂O (l) -Ca(OH)₂ (s)
B) HCl (aq) + NaOH (aq) -NaCl (aq) + H₂O (l)
C) 2 Na (s) + 2 H₂O (l) -2 NaOH (aq) + H₂ (g)
D) 2 HClO₄ (aq) + CaCO₃ (s) -Ca(ClO₄)₂ (aq) + H₂O (l) + CO₂ (g)
E) SO₂(g) + H₂O (l) -H₂SO₃ (aq)

Question 15

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:

Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How Many grams of solid NaCl must be added to 25.0 mL of 0.366 M AgNO₃ solution to completely precipitate the silver?

A) 1.57 × 10^{- 4}
B) 9.15 × 10^{- 3}
C) 6.39 × 10³
D) 0.157
E) 0.535

Question 16

What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?

A) 14.3
B) 0.24
C) 0.076
D) 6.55
E) 13.1

Question 17

Pure acetic acid (HC₂H₃O₂) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in sufficient water to give500.0 mL of solution. The density of glacial acetic acid at 25°C is 1.049 g/mL.

A) 21.0
B) 0.350
C) 0.0210
D) 1.26 × 10³
E) 3.50 × 10^{- 4}

Question 18

Which of the following is an oxidation- reduction reaction?

A) Cu (s) + 2AgNO₃ (aq) - 2Ag (s) + Cu(NO₃)₂ (aq)
B) Ba(C₂H₃O₂)₂ (aq) + Na₂SO₄ (aq) - BaSO₄ (s) + 2NaC₂H₃O₂ (aq)
C) HCl (aq) + NaOH (aq) -H₂O (l) + NaCl (aq)
D) AgNO₃ (aq) + HCl (aq) - AgCl (s) + HNO₃ (aq)
E) H₂CO₃ (aq) + Ca(NO₃)₂ (aq) - 2HNO₃ (aq) + CaCO₃ (s)

Question 19

The balanced molecular equation for complete neutralization of H₂SO₄ by KOH in aqueous solution is _ .

A) H₂SO₄ (aq) + 2KOH (aq) - 2H₂O (l) + K₂SO₄ (aq)
B) 2H⁺ (aq) + 2KOH (aq) - 2H₂O (l) + 2K⁺ (aq)
C) H₂SO₄ (aq) + 2OH^- (aq) - 2H₂O (l) + SO₄^2- (aq)
D) 2H⁺ (aq) + 2OH^- (aq) - 2H₂O (l)
E) H₂SO₄ (aq) + 2KOH (aq) - 2H₂O (l) + K₂SO₄ (s)

Question 20

What volume (L) of 0.250 M HNO₃ is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water?

A) 1.75
B) 0.070
C) 1.75 × 10^{- 3}
D) 50.0
E) 0.44

Question 21

The reaction between strontium hydroxide and chloric acid produces .

A) two molecular compounds
B) two strong electrolytes
C) a molecular compound and a weak electrolyte
D) a molecular compound and a strong electrolyte
E) two weak electrolytes

Question 22

A compound was found to be soluble in water. It was also found that addition of acid to an aqueous solution of this compound resulted in the formation of carbon dioxide. Which one of the following cations would form a precipitate when added to an aqueous solution of this compound?

A) NH₄⁺
B) Rb⁺
C) K+
D) Na⁺
E) Cr³⁺

Question 23

Aqueous solutions of a compound did not form precipitates with Cl^- , Br^- , I^- , SO₄^2- , CO₃^2- , P O₄^3- , OH^- , or S^2- . This highly water- soluble compound produced the foul- smelling gas H₂S when the solution was acidified. This compound is .

A) AgNO₃
B) Pb(NO₃)₂
C) Li₂CO₃
D) (NH₄)₂S
E) KBr

Question 24

Based on the activity series, which one of the reactions below will occur?

A) 3Hg (l) + 2Cr(NO₃)₃ (aq) - 3Hg(NO₃)₂ + 2Cr (s)
B) Zn (s) + MnI₂ (aq) - ZnI₂ (aq) + Mn (s)
C) SnCl₂ (aq) + Cu (s) - Sn (s) + CuCl₂ (aq)
D) 3FeBr₂ (aq) + 2Au (s) - 3Fe (s) + 2AuBr₃ (aq)
E) 2AgNO₃ (aq) + Pb (s) - 2Ag (s) + Pb(NO₃)₂ (aq)

Question 25

Which solution has the same number of moles of solute A as 50.00 mL of 0.100M solution of NaOH?

A) 25.00 mL of 0.175M solution of A
B) 100.00 mL of 0.0500M solution of A
C) 30.00 mL of 0.145M solution of A
D) 20.00 mL of 0.200M solution of A
E) 50.00 mL of 0.125M solution of A

Question 26

The net ionic equation for formation of an aqueous solution of Al(NO₃)₃ via mixing solid Al(OH)₃ and aqueous nitric acid is .

A) Al(OH)₃ (s) + 3NO₃^- (aq) - 3OH^- (aq) + Al(NO₃)₃ (s)
B) Al(OH)₃ (s) + 3HNO₃ (aq) - 3H₂O (l) + Al(NO₃)₃ (aq)
C) Al(OH)₃ (s) + 3H⁺ (aq) - 3H₂O (l) + Al³⁺ (aq)
D) Al(OH)₃ (s) + 3HNO₃ (aq) - 3H₂O (l) + Al³⁺ (aq) + NO₃^- (aq)
E) Al(OH)₃ (s) + 3NO₃^- (aq) - 3OH^- (aq) + Al(NO₃)₃ (aq)

Question 27

Which one of the following is a diprotic acid?

A) phosphoric acid
B) nitric acid
C) sulfuric acid
D) chloric acid
E) hydrofluroric acid

Question 28

Which combination will produce a precipitate?

A) AgNO₃ (aq) and Ca(C₂H₃O₂)₂ (aq)
B) NaOH (aq) and HCl (aq)
C) NH₄OH (aq) and HCl (aq)
D) NaCl (aq) and HC₂H₃O₂ (aq)
E) NaOH (aq) and Fe(NO₃)₂ (aq)

Question 29

Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca₃(PO₄)₂?

A) This solution contains 0.800 mol of oxygen atoms.
B) This solution contains 6.67 × 10^{- 2} mol of Ca²⁺.
C) There are 6.02 × 10²² phosphorus atoms in 500.0 mL of this solution.
D) This solution contains 0.200 mol of Ca₃(PO₄)₂.
E) 1.00 L of this solution is required to furnish 0.300 mol of Ca²+ ions.

Question 30

Which compound has the atom with the highest oxidation number?

A) Al(NO₂)₃
B) MgSO₃
C) CaS
D) Na₃N
E) NH₄Cl

Question 31

What volume (mL) of 7.48 × 10^{- 2} M phosphoric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?

A) 375
B) 750
C) 75.0
D) 125
E) 188

Question 32

A 0.100 M solution of will contain the highest concentration of potassium ions.

A) potassium phosphate
B) potassium iodide
C) potassium hypochlorite
D) potassium hydrogen carbonate
E) potassium oxide

Question 33

Which one of the following compounds is insoluble in water?

A) K₂SO₄
B) ZnS
C) AgNO₃
D) Na₂CO₃
E) Fe(NO₃)₃

Question 34

Calculate the number of grams of solute in 500.0 mL of 0.189 M KOH.

A) 5.30 × 10³
B) 5.30
C) 1.68 × 10^{- 3}
D) 1.68
E) 148

Question 35

Of the species below, only is NOT an electrolyte.

A) Rb₂SO₄
B) NaCl
C) KOH
D) HCl
E) Ar

Question 36

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

A) 20.0 mL of 0.0500 M nitric acid
B) 15.0 mL of 0.0500 M hydrobromic acid
C) 5.0 mL of 0.0100 M sulfuric acid
D) 10.0 mL of 0.0500 M perchloric acid
E) 10.0 mL of 0.0500 M phosphoric acid

Question 37

Which one of the following is a weak acid?

A) HF
B) HClO₄
C) HI
D) HCl
E) HNO₃

Question 38

What mass (g) of CaF₂ is formed when 47.8 mL of 0.334 M NaF is treated with an excess of aqueous calcium nitrate?

A) 2.49
B) 0.472
C) 1.25
D) 0.623
E) 0.943

Question 39

The net ionic equation for formation of an aqueous solution of NiI₂ accompanied by evolution of C O₂ gas via mixing solid NiCO₃ and aqueous hydriodic acid is .

A) NiCO₃ (s) + 2HI (aq) -H₂O (l) + CO₂ (g) + Ni²⁺ (aq) + 2I^- (aq)
B) NiCO₃ (s) + 2HI (aq) - 2H₂O (l) + CO₂ (g) + NiI₂ (aq)
C) NiCO₃ (s) + 2H⁺ (aq) -H₂O (l) + CO₂ (g) + Ni²⁺ (aq)
D) NiCO₃ (s) + I^- (aq) - 2H₂O (l) + CO₂ (g) + Ni²⁺ (aq) + HI (aq)
E) 2NiCO₃ (s) + HI (aq) - 2H₂O (l) + CO₂ (g) + 2Ni²⁺ (aq)

Question 40

A 13.8 mL aliquot of 0.176 M H₃PO₄ (aq) is to be titrated with 0.110 M NaOH (aq). What volume (mL) of base will it take to reach the equivalence point?

A) 20.9
B) 7.29
C) 199
D) 66.2
E) 22.1

Question 41

Which of the following reactions will not occur as written?

A) Mg (s) + Ca(OH)₂ (aq) - Ca (s) + Mg(OH)₂ (aq)
B) Co (s) + 2AgCl (aq) - 2Ag (s) + CoCl₂ (aq)
C) Sn (s) + 2AgNO₃ (aq) - 2Ag (s) + Sn(NO₃)₂ (aq)
D) Co (s) + 2HI (aq) -H₂ (g) + CoI₂ (aq)
E) Zn (s) + Pb(NO₃)₂ (aq) - Pb (s) + Zn(NO₃)₂ (aq)

Question 42

What mass (g) of barium iodide is contained in 250 mL of a barium iodide solution that has an iodide ion concentration of 0.193 M?

A) 9.44
B) 18.9
C) 0.024
D) 37.7
E) 0.048

Question 43

is an oxidation reaction.

A) Ice melting in a soft drink
B) The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate
C) Neutralization of HCl by NaOH
D) Rusting of iron
E) Table salt dissolving in water for cooking vegetables

Question 44

The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is

A) HNO₃ (aq) + Sr(OH)₂ (aq) - Sr(NO₃)₂ (aq) + H₂ (g)
B) 2HNO₃ (aq) + Sr(OH)₂ (aq) - 2H₂O (l) + Sr(NO₃)₂ (aq)
C) HNO₃ (aq) + SrOH (aq) -H₂O (l) + SrNO₃ (aq)
D) 2HNO₃ (aq) + Sr(OH)₂ (aq) - Sr(NO₃)₂ (aq) + 2H₂ (g)
E) HNO₃ (aq) + Sr(OH)₂ (aq) -H₂O (l) + Sr(NO₃)₂ (aq)

Question 45

What volume (mL) of 7.48 × 10^{- 2} M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?

A) 188
B) 375
C) 125
D) 8.60
E) 750

Question 46

A stock solution of HNO₃ is prepared and found to contain 13.5 M of HNO₃. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is M.

A) 1.48
B) 0.270
C) 675
D) 0.675
E) 270

Question 47

Oxidation and mean essentially the same thing.

A) reduction
B) activity
C) decomposition
D) corrosion
E) metathesis

Question 48

The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is .

A) Zn (s) + 2HBr (aq) - ZnBr₂ (aq) + 2H⁺ (aq)
B) Zn (s) + 2H⁺ (aq) -Zn²⁺ (aq) + H₂ (g)
C) 2Zn (s) + H⁺ (aq) - 2Zn²⁺ (aq) + H₂ (g)
D) Zn (s) + 2Br^- (aq) - ZnBr₂ (aq)
E) Zn (s) + 2HBr (aq) - ZnBr₂ (s) + 2H⁺ (aq)

Question 49

A 0.200 M K₂SO₄ solution is produced by .

A) dissolving 20.2 g of K₂SO₄ in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL
B) diluting 20.0 mL of 5.00 M K₂SO₄ solution to 500.0 mL
C) dissolving 43.6 g of K₂SO₄ in water and diluting to a total volume of 250.0 mL
D) dilution of 1.00 mL of 250 M K₂SO₃ to 1.00 L
E) dilution of 250.0 mL of 1.00 M K₂SO₄ to 1.00 L

Question 50

In which reaction does the oxidation number of oxygen increase?

A) 2 SO₂ (g) + O₂ (g) -2 SO₃ (g)
B) HCl (aq) + NaOH (aq) -NaCl (aq) + H₂O (l)
C) Ba(NO₃)₂ (aq) + K₂SO₄ (aq) -BaSO₄ (s) + 2 KNO₃ (aq)
D) 2 H₂O (l) -2 H₂ (g) + O₂ (g)
E) MgO (s) + H₂O (l) -Mg(OH)₂ (s)

Question 51

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H₂SO₄ solution is required to neutralize a 25.0- mL sample of the NaOH solution?

A) 0.400
B) 0.315
C) 125
D) 0.629
E) 0.801

Question 52

How many milliliters of 0.132 M HClO₄ solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

A) 0.0120
B) 0.0335
C) 83.7
D) 29.9
E) 0.521

Question 53

A tenfold dilution of a sample solution can be obtained by taking .

A) 10 parts sample and 1 part solvent
B) 99 parts sample and 1 part solvent
C) 9 parts sample and 1 part solvent
D) 1 part sample and 10 parts solvent
E) 1 part sample and 9 parts solvent

Question 54

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide:

Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.700 mol of Pb(NO₃)₂ (aq) to completely precipitate the lead?

A) 0.197
B) 0.394
C) 394
D) 197
E) 2.54 × 10^{- 3}

Question 55

Which one of the following solutions will have the greatest concentration of hydroxide ions?

A) 0.100 M ammonia
B) 0.100 M hydrochloric acid
C) 0.100 M beryllium hydroxide
D) 0.100 M rubidium hydroxide
E) 0.100 M magnesium hydroxide

Question 56

Sodium does not occur in nature as Na (s) because .

A) it is easily reduced to Na^-
B) it reacts with water with great difficulty
C) it is easily oxidized to Na⁺
D) it is easily replaced by silver in its ores
E) it undergoes a disproportionation reaction to Na^- and Na⁺

Question 57

Which one of the following is a correct expression for molarity?

A) mol solute/mL solvent
B) µmol solute/L solution
C) mol solute/kg solvent
D) mmol solute/mL solution
E) mol solute/L solvent

Question 58

A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?

A) 8.57
B) 0.183
C) 3.50
D) 0.0500
E) 0.117

Question 59

One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

A) zinc
B) copper
C) none of these
D) cobalt
E) lead

Question 60

In which species does sulfur have the highest oxidation number?

A) S₈ (elemental form of sulfur)
B) H₂SO₃
C) K₂SO₄
D) SO₂
E) H₂S

Question 61

Oxidation is the _ and reduction is the .

A) gain of electrons, loss of electrons
B) gain of oxygen, loss of electrons
C) loss of oxygen, gain of electrons
D) gain of oxygen, loss of mass
E) loss of electrons, gain of electrons

Question 62

How many grams of CH₃OH must be added to water to prepare 150mL of a solution that is 2.0 M CH₃OH?

Question 63

The solvent in an aqueous solution is .

Question 64

You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true?

A) A smaller volume of the less concentrated solution contains the same number of moles of the acid compared to the more concentrated solution.
B) The product of concentration and volume of the less concentrated solution equals the product of concentration and volume of the more concentrated solution.
C) It would take more base solution (per milliliter of the unknown solution) to neutralize the more concentrated solution.
D) There is no chemical method designed to tell the two solutions apart.
E) If the same volume of each sample was taken, then more base solution would be required to neutralize the one with lower concentration.

Question 65

Aqueous potassium chloride will react with which one of the following in an exchange (metathesis) reaction?

A) lead nitrate
B) barium nitrate
C) sodium bromide
D) sodium chloride
E) calcium nitrate

Question 66

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200 mL to make a 0.88 M solution of sodium hydroxide?

A) 26.4
B) 176
C) 29.3
D) 50.0
E) 2.64

Question 67

When gold dissolves in aqua regia, into what form is the gold converted?

Question 68

Of the choices below, which would be the best for the lining of a tank intended for use in storage of hydrochloric acid?

A) tin
B) copper
C) iron
D) zinc
E) nickel

Question 69

How many moles of Co²⁺ are present in 0.150 L of a 0.200 M solution of CoI₂?

Question 70

With which of the following will ammonium ion form an insoluble salt?

A) chloride
B) carbonate
C) sulfate
D) sulfate and carbonate
E) none of the above

Question 71

How many milliliters of a stock solution of 11.1 M HNO₃ would be needed to prepare 0.500 L of 0.500 M HNO₃?

A) 22.5
B) 44.4
C) 2.78
D) 0.0444
E) 0.0225

Question 72

What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO₃ is treated with an excess of aqueous hydrobromic acid?

A) 188
B) 34.5
C) 1.44
D) 1.23
E) 53.6

Question 73

Oxidation cannot occur without .

A) reduction
B) oxygen
C) air
D) water
E) acid

Question 74

Which one of the following substances is produced during the reaction of an acid with a metal hydroxide?

A) O₂
B) H₂
C) H₂O
D) NaOH
E) CO₂

Question 75

Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a .

A) tenfold dilution
B) neutralization
C) titration
D) twofold dilution
E) crystallization

Question 76

A solution is prepared by adding 1.60 g of solid NaCl to 50.0 mL of 0.100 M CaCl₂. What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

A) 0.547
B) 0.132
C) 0.232
D) 0.747
E) 0.647

Question 77

The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is

A) KOH (aq) + HC₂H₃O₂ (aq) -H₂KC₂H₃O (aq) + O₂ (g)
B) KOH (aq) + HC₂H₃O₂ (aq) - OH^- (l) + HC₂H₃O₂⁺ (aq) + K (s)
C) KOH (aq) + HC₂H₃O₂ (aq) -H₂C₂H₃O₃ (aq) + K (s)
D) KOH (aq) + HC₂H₃O₂ (aq) - KC₂H₃O₃ (aq) + H₂ (g)
E) KOH (aq) + HC₂H₃O₂ (aq) -H₂O (l) + KC₂H₃O₂ ( aq)

Question 78

What is aqua regia?

Question 79

How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?

Question 80

Calculate the concentration (M) of sodium ions in a solution made by diluting 40.0 mL of a
0.474 M solution of sodium sulfide to a total volume of 300 mL.