Deck 11: Solutions

Question 1

Which of the diagrams in the figure best represents an aqueous solution of Na₂SO₄?

A)I
B)II
C)III
D)either I or III
E)none of these is correct

Answer 1

II

Question 2

Which of the following equations describes what happens when CH₃OH(l) dissolves in water?

A)CH₃OH(l) $\rightarrow$ C(aq) + 4H(aq) + O(aq)
B)CH₃OH(l) $\rightarrow$ C^2-aq) + 4H⁺(aq) + O^2-(aq)
C)2CH₃OH(l) $\rightarrow$ 2C(aq) + 4H₂(aq) + O₂(aq)
D)CH₃OH(l) $\rightarrow$ CH₃OH(aq)
E)CH₃OH(l) + H₂O(l) $\rightarrow$ CH₅O₂H(l)

Answer 2

CH₃OH(l) $\rightarrow$ CH₃OH(aq)

Question 3

What ions, atoms, or molecules (in addition to the water molecules) are present after HNO₃(l) mixes with water?

A)HNO₃(l)
B)HNO₃(aq)
C)H⁺(aq) + NO₃^-(aq)
D)H(aq) + NO₃(aq)
E)H(aq) + N(aq) + 3O(aq)

Answer 3

H⁺(aq) + NO₃^-(aq)

Question 4

Which of the following substances is a strong electrolyte?

A)CH₃OH
B)C₆H₁₄
C)C₆H₁₂O₆
D)LiCl
E)SO₂

Question 5

Which of the diagrams in the figure best represents an aqueous solution of MgCl₂?

A)I
B)II
C)III
D)either I or III
E)none of these is correct

Question 6

Which of the following should be most soluble in benzene, C₆H₆?

A)H₂O
B)CH₃OH
C)I₂
D)NaCl
E)NaNO₃

Question 7

Which of the following substances is a strong electrolyte?

A)CH₃CH₂OH
B)C₈H₁₈
C)LiOH
D)CO₂
E)PCl₅

Question 8

Which of the following should be most soluble in hexane, C₆H₁₄?

A)NaCl
B)NaNO₃
C)H₂O
D)CH₃OH
E)Br₂

Question 9

Which of the following statements regarding the rule "like dissolves like" is incorrect?

A)Since cooking oil is composed primarily of hydrocarbons, it is soluble in water.
B)Oxygen, O₂, is not very soluble in water.
C)Methanol, CH₃OH, is water-soluble.
D)Cooking oil, a nonpolar substance, is soluble in heptane, C₇H₁₆.
E)Sodium nitrate, NaNO₃, is soluble in water.

Question 10

Which of the following substances is a strong electrolyte?

A)CH₃CH₂OH
B)C₆H₆
C)KOH
D)SO₂
E)PCl₃

Question 11

What ions, atoms, or molecules are present after CH₃CH₂OH(l) mixes with water?

A)CH₃CH₂OH(aq) and H₂O(l)
B)CH₃CH₂O^-(aq), H⁺(aq), and H₂O(l)
C)CH₃CH₂O^-(aq), and H₃O⁺(aq)
D)2C(aq), 6H(aq), and H₂O₂(l)
E)CH₃⁺(aq), CH₂O^-(aq), H⁺(aq), and H₂O(l)

Question 12

Which of the following substances is a nonelectrolyte?

A)NaNO₃
B)LiOH
C)C₆H₁₂O₆
D)LiCN
E)CsCl

Question 13

Which of the following equations describes what happens when HCl(g) dissolves in water?

A)HCl(g) $\rightarrow$ H⁺(aq) + Cl^-(aq)
B)HCl(g) $\rightarrow$ H(aq) + Cl(aq)
C)2HCl(g) $\rightarrow$ H₂(aq) + Cl₂(aq)
D)2HCl(g) $\rightarrow$ H₂(g) + Cl₂(g)
E)HCl(g) + H₂O(l) $\rightarrow$ H₃OCl(l)

Question 14

Which of the following substances is a nonelectrolyte?

A)Na₂SO₄
B)CH₃OH
C)KOH
D)LiNO₃
E)RbCl

Question 15

Which of the following should be most soluble in water?

A)Vitamin C (a very good hydrogen bonder)
B)Vitamin A (a mostly nonpolar molecule)
C)C₆H₆(l)
D)I₂(s)
E)O₂(g)

Question 16

Which of the following substances is a nonelectrolyte?

A)KMnO₄
B)CH₃CH₂OH
C)NaOH
D)K₂SO₄
E)Na₂O

Question 17

Which of the following should be most soluble in water?

A)fat (a nonpolar triglyceride molecule)
B)C₆H₆(l)
C)CH₃NH₂(l)
D)I₂(s)
E)O₂(g)

Question 18

What ions, atoms, or molecules (in addition to the water molecules) are present after Na₂SO₄(s) mixes with water?

A)Na₂SO₄(l)
B)Na₂SO₄ (aq)
C)Na⁺(aq) + NaSO₄^-(aq)
D)Na₂SO₃²⁺(aq) + O^2-(aq)
E)2Na⁺(aq) + SO₄^2-(aq)

Question 19

Which of the following statements regarding the rule "like dissolves like" is incorrect?

A)Since grease is nonpolar, it is not soluble in water.
B)Nitrogen, N₂, is not very soluble in water.
C)Methanol, CH₃OH, is not very water-soluble.
D)Butane, C₄H₁₀, is soluble in cooking oil, a nonpolar substance.
E)Calcium nitrate, Ca(NO₃), is soluble in water.

Question 20

Which of the following statements regarding the rule "like dissolves like" is incorrect?

A)Since cooking oil is composed primarily of hydrocarbons, it is insoluble in water.
B)Iodine, I₂, is very soluble in water.
C)Ethanol, CH₃CH₂OH, is water-soluble.
D)Cooking oil, a nonpolar substance, is soluble in hexane, C₆H₁₄.
E)Potassium nitrate, KNO₃, is soluble in water.

Question 21

Which of the following occurs when an ionic compound dissolves in water to form a solution?

A)Ionic bonds break.
B)Hydrogen bonds are disrupted.
C)H₂O - Ion attractive forces form.
D)Entropy increases.
E)All of these

Question 22

Which of the following statements regarding solubility is incorrect?

A)A polar compound will dissolve an ionic compound due to ion-dipole interactions.
B)A nonpolar solvent will not interact strongly enough with ions to dissolve an ionic compound.
C)Nonpolar liquids will dissolve in one another because the intermolecular forces in the pure liquids are weak, and there is an increase in entropy.
D)Most ionic solids are more soluble in water at higher temperature than at a lower temperature of the solvent.
E)Most gases are more soluble at a higher temperature than at a lower temperature of the solvent.

Question 23

When potassium nitrate is dissolved in water, the resulting solution feels cool to the touch.This means that:

A)the strength of attraction between the solute particles is greater than that of the attraction between the solute and solvent.
B)the strength of attraction between the solute and solvent particles is greater than that of the attraction between the solute particles.
C)the strength of attraction between the solute particles is equal to that of the attraction between the solute and solvent.
D)hydrogen bonds must be broken, which is an exothermic process.
E)there is a decrease in entropy for the solution.

Question 24

Which of the following statements regarding the solution process is incorrect?

A)When a solution is formed from an ionic compound, the anions and cations are evenly distributed throughout the solution.
B)When a polar covalent compound dissolves in water, dipole-dipole interactions take place between the water molecules and the solute molecules.
C)A nonpolar compound such as hexane, C₆H₁₄, forms London dispersion forces with a nonpolar solute, such as I₂ during the solution process.
D)The solution process is always exothermic.
E)When an ionic solute dissolves, the entropy of the solution is greater than the original entropy of the crystalline form of the ionic substance.

Question 25

Which of the following statements regarding the solution process is incorrect?

A)In a sodium chloride solution, the ions interact with the water molecules through ion-dipole forces.
B)Hydration is the process whereby water molecules surround solute particles.
C)A hydrated cation is surrounded by the partially positive end of the water molecules.
D)When an ionic compound dissolves, the ionic bonds break.
E)Some of the hydrogen bonds among the water molecules must break.

Question 26

The solubility of potassium chloride is 34.2 g/100.0 g of water at 20^oC.Which of the following best describes a solution prepared by adding 58.3 g of potassium chloride to 150.0 g of water at this temperature?

A)34.2 g of KCl will dissolve and 24.1 g will remain undissolved.
B)51.3 g of KCl will dissolve and 7.0 g will remain undissolved.
C)24.1 g of KCl will dissolve and 34.2 g will remain undissolved.
D)58.3 g of KCl will dissolve and the solution will be unsaturated.
E)107 g of KCl will dissolve and the solution will be saturated.

Question 27

What mass of sodium nitrate is dissolved in 455 g of a solution that is 15.0% by mass NaNO₃?

A)68.3 g
B)30.3 g
C)4.40 *10² g
D)3.03 * 10³ g
E)15.0 g

Question 28

Which of the following should be most soluble in ethanol, CH₃CH₂OH?

A)CH₃NH₂
B)CCl₄
C)I₂
D)C₆H₆
E)CO₂

Question 29

What is the percent-by-mass concentration of KOH in a solution that is prepared by adding 18.0 g of KOH to 95.0 g of water?

A)18.9%
B)15.9%
C)31.5%
D)5.28%
E)77.0%

Question 30

Which of the following increases the solubility of a gas in solution?

A)increasing gas pressure and increasing temperature
B)increasing gas pressure and decreasing temperature
C)decreasing gas pressure and increasing temperature
D)decreasing gas pressure and decreasing temperature
E)adding more water

Question 31

If the solubility of sodium chloride at 25 $\degree$ C is 36.0 g/100 g water, which of the following best describes what eventually forms after 15.0 grams of sodium chloride is mixed with 50.0 grams of water at 25 $\degree$ C?

A)a saturated solution with some undissolved solid
B)an unsaturated solution with some undissolved solid
C)a saturated solution with no undissolved solid
D)an unsaturated solution with no undissolved solid
E)a supersaturated solution

Question 32

What is the percent-by-mass concentration of KCl in a solution that is prepared by adding 13.0 g of KCl to 85.0 g of water?

A)15.3%
B)17.2%
C)13.3%
D)72.0%
E)65.4%

Question 33

Many cold packs contain ammonium nitrate and water.The dissolving of ammonium nitrate is endothermic.Which of the following best describes the energy and entropy changes that occur for the NH₄NO₃ system when ammonium nitrate and water are mixed to make a solution?

A)There is a net energy increase and an entropy increase.
B)There is a net energy increase and an entropy decrease.
C)There is a net energy decrease and an entropy decrease.
D)There is no a net change in energy or entropy.

Question 34

What mass of sodium hydroxide is dissolved in 295 g of a solution that is 12.0% by mass NaOH?

A)3540 g
B)35.4 g
C)4.07 g
D)40.7 g
E)12.0 g

Question 35

What mass of sodium chloride is dissolved in 365 g of a solution that is 14.0% by mass NaCl?

A)5110 g
B)26.1 g
C)351 g
D)51.1 g
E)14.0 g

Question 36

What is the percent-by-mass concentration of NaCl in a solution that is prepared by adding 14.0 g of NaCl to 75.0 g of water?

A)61.0%
B)15.7%
C)18.7%
D)24.0%
E)5.36%

Question 37

Sodium chloride, NaCl, dissolves in water because

A)there are attractive forces between ions and water molecules.
B)there are no attractive forces between ions and water molecules.
C)the entropy of the solution is greater than the entropy of pure NaCl and pure H₂O.
D)the entropy of the solution is less than the entropy of pure NaCl and pure H₂O.
E)Both A and C

Question 38

If the solubility of a solid substance is 18.2 g/100 g water, which of the following best describes what eventually forms after 10.0 grams of the substance is mixed with 50.0 grams of water?

A)a saturated solution with some undissolved solid
B)an unsaturated solution with some undissolved solid
C)a saturated solution with no undissolved solid
D)an unsaturated solution with no undissolved solid
E)a supersaturated solution

Question 39

Given that the solubility of potassium chlorate in water is 10.0 g/100 g water at 30 $\degree$ C, what mass of potassium chlorate is dissolved in 250 grams of a saturated solution at 30 $\degree$ C?

A)any mass greater than 25.0 g
B)any mass less than 10.0 g
C)any mass less than 25.0 g
D)25.0 g
E)10.0 g

Question 40

Which of the following statements regarding the solubility of oxygen in water is incorrect?

A)Water in contact with air contains a small amount of dissolved oxygen.
B)When water is heated, the first tiny bubbles that you see escaping from the warm water contain O₂.
C)In warm weather, fish must come to the surface more often to get oxygen, since there is less dissolved oxygen in the water than in cooler weather.
D)If a sealed container has both oxygen and water, changing the pressure of the oxygen above the water will have no effect on the solubility of the oxygen in the water.
E)An increase in temperature causes an increase in the kinetic energy of the molecules in a solution, allowing oxygen molecules to escape more readily.

Question 41

A solution contains 15.5 g of NaOH dissolved in sufficient water to give a total mass of 125.0 g.What is the molality of the solution?

A)3.54 m
B)0.124 m
C)0.00310 m
D)3.10 m
E)124 m

Question 42

A 200.0 g sample of river water contains 6.5 mg of lead.How many parts per million of lead are in the sample?

A)6.5 ppm
B)21 ppm
C)3.2 * 10² ppm
D)32 ppm
E)54 ppm

Question 43

What is the molal concentration of ions in a 2.40 m solution of Al(NO₃)₃?

A)2.40 m
B)7.20 m
C)9.60 m
D)0.800 m
E)31.2 m

Question 44

A solution contains 22.0 g of HCl dissolved in sufficient water to give a total mass of 125.0 g.What is the molality of the solution?

A)0.250 m
B)5.86 m
C)2.75 m
D)4.83 m
E)0.176 m

Question 45

A solution of acetic acid, CH₃CO₂H, is prepared by dissolving 40.0 mL of acetic acid in enough water to give a total volume of 250.0 mL.What is the percent-by-volume concentration of acetic acid?

A)19.0%
B)16.0%
C)25.0%
D)40.0%
E)13.8%

Question 46

What volume of 2.00 M HCl contains 0.50 mol HCl?

A)1.0 L
B)0.25 L
C)2.5 L
D)0.50 L
E)1.5 L

Question 47

A solution of acetic acid, CH₃CO₂H, is prepared by dissolving 30.0 mL of acetic acid in enough water to give a total volume of 150.0 mL.What is the percent-by-volume concentration of acetic acid?

A)16.7%
B)15.0%
C)30.0%
D)20.0%
E)25.0%

Question 48

A solution contains 25.5 g of NaCl dissolved in sufficient water to give a total mass of 325.0 g.What is the molality of the solution?

A)0.146 m
B)0.785 m
C)1.34 m
D)1.46 m
E)134 m

Question 49

A 150.0 g sample of ocean water contains 3.5 mg of mercury.How many parts per million of mercury are in the sample?

A)15 ppm
B)23 ppm
C)2.4 F* 10² ppm
D)2.3 *10⁴ ppm
E)43 ppm

Question 50

A solution of ethanol, C₂H₅OH, is prepared by dissolving 25.0 mL of ethanol in enough water to give a total volume of 250.0 mL.What is the percent-by-volume concentration of ethanol?

A)10.0%
B)9.09%
C)90.0%
D)1.00%
E)225%

Question 51

What is the percent-by-mass concentration of hydrogen peroxide, H₂O₂, in an aqueous solution that contains 30.0 g of hydrogen peroxide in 1.00 L of solution.The density of the solution is 1.00 g/mL.

A)30.0%
B)3.00%
C)33.3%
D)31.0%
E)70.0%

Question 52

What volume of 3.00 M NaOH contains 1.75 mol NaOH?

A)1.75 L
B)3.00 L
C)4.75 L
D)0.583 L
E)1.71 L

Question 53

What is the percent-by-mass concentration of antifreeze (ethylene glycol, C₂H₆O₂) in an aqueous solution that contains 420.0 g of ethylene glycol in 1.00 L of solution.The density of the solution is 1.05 g/mL.

A)2.50%
B)42.1%
C)40.0%
D)44.1%
E)60.0%

Question 54

A 200.0 g sample of rainwater contains 4.8 mg of sulfuric acid.How many parts per million of sulfuric acid are in the sample?

A)42 ppm
B)21 ppm
C)2.4 *10² ppm
D)4.8 ppm
E)24 ppm

Question 55

What is the molal concentration of ions in a 1.60 m solution of Fe(NO₃)₃?

A)1.60 m
B)3.20 m
C)4.80 m
D)6.40 m
E)20.8 m

Question 56

What volume of 6.00 M NaOH contains 2.50 mol NaOH?

A)2.50 L
B)6.00 L
C)2.40 L
D)0.417 L
E)15.0 L

Question 57

How many moles of NaOH are contained in 100.0 mL of 3.00 M NaOH?

A)0.300 moles
B)300.0 moles
C)33.3 moles
D)0.00300 moles
E)0.333 moles

Question 58

How many moles of HCl are contained in 75.0 mL of 2.00 M HCl?

A)2.00 moles
B)1.50 *² moles
C)0.150 moles
D)37.5 moles
E)26.7 moles

Question 59

How many moles of NaCl are contained in 50.0 mL of 2.50 M NaCl?

A)2.50 moles
B)0.050 moles
C)5.00 moles
D)2.45 moles
E)0.125 moles

Question 60

What is the percent-by-mass concentration of citric acid, C₆H₈O₇, in an aqueous solution that contains 263.2 g of citric acid in 1.00 L of solution.The density of the solution is 1.10 g/mL.

A)73.7%
B)26.3%
C)23.9%
D)3.80%
E)29.0%

Question 61

Silver nitrate, AgNO₃, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl.What volume of 2.0 M AgNO₃ will be required to react with 50.0 mL of a 0.10 M HCl solution? AgNO₃(aq) + HCl(aq) $\rightarrow$ AgCl(s) + HNO₃(aq)

A)0.25 mL
B)25 mL
C)5.0* 10¹ mL
D)2.5 *10² mL
E)2.5 mL

Question 62

How many moles of potassium iodide, KI, are required to precipitate all of the lead (II) ion from 50.0 mL of a 1.2 M Pb(NO₃)₂ solution? (First, write a balanced equation for the reaction.)

A)0.12 mole
B)0.060 mole
C)0.24 mole
D)0.030 mole
E)0.048 mole

Question 63

How many moles of potassium iodide, KI, are required to precipitate all of the lead (II) ion from 25.0 mL of a 1.6 M Pb(NO₃)₂ solution? (First, write a balanced equation for the reaction.)

A)0.040 mole
B)0.080 mole
C)0.020 mole
D)64 mol
E)0.64 mol

Question 64

When a 25.00 mL sample of NaOH is titrated with 0.4523 M H₂SO₄, 36.69 mL of H₂SO4 solution is required to neutralize the NaOH.What is the molarity of the NaOH?

A)0.3319 M
B)0.6638 M
C)1.328 M
D)0.6164 M
E)0.1988 M

Question 65

Calculate the freezing point of a 1.0 m solution of Ca(NO₃)₂ in water? Remember that Mg(NO₃)₂ is an electrolyte.The normal freezing point of pure water is 0.00 $\degree$ C.K_f (water) = -1.86 $\degree$ C/m

A)1.56 $\degree$ C
B)5.58 $\degree$ C
C)1.86 $\degree$ C
D)-5.58 $\degree$ C
E)-1.86 $\degree$ C

Question 66

Silver nitrate, AgNO₃, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl.What volume of 1.5 M AgNO₃ will be required to react with 30.0 mL of a 0.45 M HCl solution AgNO₃(aq) + HCl(aq) $\rightarrow$ AgCl(s) + HNO₃(aq)

A)45 mL
B)9.0 mL
C)9.0 L
D)1.0 L
E)1.1 *10² mL

Question 67

Calculate the freezing point of a 2.0 m solution of NaCl in water? Remember that NaCl is an electrolyte.The normal freezing point of pure water is 0.00 $\degree$ C.K_f (water) = -1.86 $\degree$ C/m

A)-2.08 $\degree$ C
B)-3.72 $\degree$ C
C)-7.44 $\degree$ C
D)7.44 $\degree$ C
E)3.74 $\degree$ C

Question 68

When a 25.00 mL sample of H₂SO₄ is titrated with 0.3423 M NaOH, 26.67 mL of NaOH solution is required to neutralize the H₂SO₄.What is the molarity of the H₂SO₄?

A)0.3652 M
B)0.3209 M
C)0.1604 M
D)0.1826 M
E)0.1988 M

Question 69

The EPA has determined that the maximum safe level of lead ion in drinking water is 15 ppb.If a sample of tap water has a lead ion concentration of 0.0065 ppm, what is the concentration of the lead ion in ppb, and is the water safe to drink? Assume the density of the solution is 1.00 g/mL.

A)65 ppb, not safe
B)6.5 ppb, safe
C)650 ppb, not safe
D)0.65 ppb, safe
E)6.5 * 10^-6 ppm, safe

Question 70

When a 25.00 mL sample of NaOH is titrated with 0.2523 M H₂SO₄, 26.69 mL of H₂SO₄ solution is required to neutralize the NaOH.What is the molarity of the NaOH?

A)0.1347 M
B)0.4726 M
C)0.5387 M
D)0.2694 M
E)0.2363 M

Question 71

The EPA has determined that the maximum safe level of lead ion in drinking water is 15 ppb.If a sample of tap water has a lead ion concentration of 0.016 ppm, what is the concentration of the lead ion in ppb, and is the water safe to drink? Assume the density of the solution is 1.00 g/mL.

A)160 ppb, not safe
B)16 ppb, not safe
C)1600 ppb, not safe
D)0.16 ppb, safe
E)1.6 * 10^-6 ppm, safe

Question 72

Consider two aqueous glucose solutions of different concentrations, separated by a semi-permeable membrane.Which of the following best describes the process of osmosis at the molecular level?

A)The smaller water molecules move in a net direction from the more dilute side to the more concentrated side.
B)The smaller water molecules move in a net direction from the more concentrated side to the more dilute side.
C)The larger glucose particles move in a net direction from the more dilute side to the more concentrated side.
D)The larger glucose particles move in a net direction from the more concentrated side to the more dilute side.
E)Osmosis will not occur.

Question 73

What volume of 0.1452 M KOH is required to neutralize 25.00 mL of 0.1020 M H₂SO₄? (First, write a balanced equation for the reaction.)

A)17.79 mL
B)17.56 mL
C)8.781 mL
D)35.12 mL
E)71.18 mL

Question 74

What will happen to a blood cell that is placed in pure water?

A)The cell will shrink because there will be a net flow of water to the outside of the cell.
B)The cell will shrink because there will be a net flow of electrolytes to the outside of the cell.
C)The cell will expand because there will be a net flow of water to the inside of the cell.
D)The cell will expand because there will be a net flow of electrolytes to the inside of the cell.
E)Nothing will happen because the cell is impermeable.

Question 75

Calculate the freezing point of a 2.0 m solution of sucrose in water? Sucrose is a nonelectrolyte.The normal freezing point of pure water is 0.00 $\degree$ C.K_f (water) = -1.86 $\degree$ C/m

A)-1.86 $\degree$ C
B)-3.72 $\degree$ C
C)-2.00 $\degree$ C
D)3.72 $\degree$ C
E)1.86 $\degree$ C

Question 76

What volume of 0.1243 M KOH is required to neutralize 25.00 mL of 0.1540 M H₂SO₄? (First, write a balanced equation for the reaction.)

A)10.09 mL
B)30.97 mL
C)61.95 mL
D)20.18 mL
E)40.36 mL

Question 77

What will happen to a blood cell that is placed in an aqueous solution that has a high salt concentration relative to the blood cell concentration?

A)The cell will shrink because there will be a net flow of water to the outside of the cell.
B)The cell will shrink because there will be a net flow of electrolytes to the outside of the cell.
C)The cell will expand because there will be a net flow of water to the inside of the cell.
D)The cell will expand because there will be a net flow of electrolytes to the inside of the cell.
E)Nothing will happen because the cell is impermeable.

Question 78

Calculate the boiling point of a 4.0 m solution of sucrose in water? Sucrose is a nonelectrolyte.The normal boiling point of pure water is 100.0 $\degree$ C.K_b (water) = 0.52 $\degree$ C/m

A)2.1 $\degree$ C
B)97.9 $\degree$ C
C)96.0 $\degree$ C
D)94.0 $\degree$ C
E)102.1 $\degree$ C

Question 79

Calculate the boiling point of a 4.0 m solution of KI in water? Remember that KI is an electrolyte.The normal boiling point of pure water is 100.0 $\degree$ C.K_b (water) = 0.52 $\degree$ C/m

A)101.0 $\degree$ C
B)104.2 $\degree$ C
C)96.0 $\degree$ C
D)102.1 $\degree$ C
E)4.16 $\degree$ C

Question 80

When a 25.00 mL sample of H₂SO₄ is titrated with 0.2453 M NaOH, 32.47 mL of NaOH solution is required to neutralize the H₂SO₄.What is the molarity of the H₂SO₄?

A)0.3186 M
B)0.1889 M
C)0.3777 M
D)3.309 M
E)0.1593 M