Question 1

Calculate the molality of a 20.0% by mass ammonium sulfate (NH₄)₂SO₄ solution.The density of the solution is 1.117 g/mL.

Accepted Answer

The answer of Calculate the molality of a 20.0% by...

Question 2

The density of a 20.3 M CH₃OH (methanol)solution is 0.858 g/mL.What is the molality of this solution? H₂O is the solvent.

Accepted Answer

The answer of The density of a 20.3 M CH₃OH...

Question 3

The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10^-4 mol/L.What is the value of the Henry's law constant in mol L^-1• atm^-1?

Accepted Answer

Henry's law states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. The constant of proportionality is known as Henry's law constant (kH). The formula for Henry's law is S = kH * P, where S is the solubility of the gas, kH is Henry's law constant, and P is the pressure of the gas.Given:- Solubility (S) = 4.7 × 10^-4 mol/L- Pressure (P) = 522 mmHg = 522/760 atm (since 1 atm = 760 mmHg)To find kH, rearrange the formula to kH = S / P.kH = (4.7 × 10^-4 mol/L) / (522/760 atm) = (4.7 × 10^-4 mol/L) / (0.6868 atm) ≈ 6.8 × 10^-4 mol/L•atmTherefore, the Henry's law constant is 6.8 × 10^-4 mol/L•atm.

Question 4

What is the molarity of a solution prepared by diluting 1.85 L of 6.5 M KOH to 11.0 L?

Accepted Answer

The answer of What is the molarity of a solution...

Question 5

Calcium nitrite is used as a corrosion inhibitor in lubricants.What is the molality of a solution prepared by dissolving 18.5 g of calcium nitrite in 83.5 g of distilled water?

Accepted Answer

The answer of Calcium nitrite is used as a corrosion...

Question 6

The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the aqueous solubility of atmospheric O₂ is 2.67 × 10^-4 M at sea level and 25°C,what is the solubility of O₂ at an elevation of 12,000 ft where the total pressure is 0.657 atm? Assume the temperature is 25°C,and that the mole fraction of O₂ in air is 0.209 At both 12,000 ft and at sea level.

Accepted Answer

The solubility of a gas is directly proportional to its partial pressure (Henry's Law). At 12,000 ft, the partial pressure of O₂ is 0.657 atm × 0.209 = 0.137 atm. The solubility at sea level is 2.67 × 10⁻⁴ M with a partial pressure of 0.209 atm. Therefore, the solubility at 12,000 ft is (0.137/0.209) × 2.67 × 10⁻⁴ M = 1.75 × 10⁻⁴ M.

Question 7

Cadmium bromide is used in photography and lithography.What is the molality of a solution prepared by dissolving 45.38 g of CdBr₂ in 375.0 g of water?

Accepted Answer

The answer of Cadmium bromide is used in photography and...

Question 8

Copper(II)bromide is used as a wood preservative.What mass of CuBr₂ is needed to prepare 750.0 mL of a 1.25 M solution?

Accepted Answer

The answer of Copper(II)bromide is used as a wood preservative.What...

Question 9

What is the molarity of a solution of 10.0% by mass cadmium sulfate,CdSO₄ (208.47g/mol)? The density of the solution is 1.10 g/mL.

Accepted Answer

To find the molarity of the solution, we first determine the mass of cadmium sulfate in 1000 mL (or 1 L) of solution, since molarity is moles of solute per liter of solution. With a 10.0% by mass solution and a density of 1.10 g/mL, the mass of the solution per liter is 1100 g. Therefore, the mass of cadmium sulfate in this volume is 10.0% of 1100 g, which is 110 g. The molar mass of cadmium sulfate (CdSO4) is approximately 208.47 g/mol, so the number of moles of cadmium sulfate in 110 g is 110 g / 208.47 g/mol = 0.528 mol. Thus, the molarity of the solution is 0.528 M.

Question 10

What is the molality of a solution prepared by dissolving 84.7 g of KMnO₄ in 165 g of water?

Accepted Answer

The answer of What is the molality of a solution...

Question 11

What mass of water is required to dissolve 25.31 g of potassium nitrate (KNO₃)in order to prepare a 0.1982 m solution?

Accepted Answer

First, we need to calculate the moles of potassium nitrate:
moles = mass/molar mass
moles = 25.31 g / 101.1 g/mol
moles = 0.2502 mol

Next, we plug in the given molarity and moles into the following equation:
molarity = moles / volume(in liters)

We rearrange this equation to solve for volume:
volume = moles / molarity

volume = 0.2502 mol / 0.1982 mol/L
volume = 1.263 L

Finally, we convert liters to kilograms of water, since 1 L of water has a mass of 1 kg:
mass of water = volume * density of water
mass of water = 1.263 L * 1 kg/L
mass of water = 1.263 kg

Therefore, the answer is D: 1.263 kg.

Question 12

Which combination of a 36.0% (w/w)stock solution of acetic acid (d = 1.045 g/mL)and water will result in 1.00 kg of a 15.0% (w/w)acetic acid solution?

Accepted Answer

To achieve a 15.0% (w/w) acetic acid solution from a 36.0% solution, the mass of the acetic acid in the final solution must be 15% of the total mass (1.00 kg). Option B correctly maintains the mass proportions, using 417 g of the 36% acetic acid solution to achieve the desired concentration when mixed with 583 g of water, totaling 1.00 kg of the final solution.

Question 13

What mass of LiOH is required to prepare 0.250 L of a 3.55 M solution?

Accepted Answer

We can use the formula: Molarity = moles of solute/volume of solution in liters
Rearranging, we get moles of solute = Molarity x volume of solution in liters
moles of solute = 3.55 x 0.250 = 0.8875
Now we use the molar mass of LiOH to convert moles to grams:
molar mass of LiOH = 23.95 + 15.99 + 1.01 = 40.95 g/mol
mass of LiOH = moles of LiOH x molar mass of LiOH
mass of LiOH = 0.8875 x 40.95 = 36.33 g
Therefore, the mass of LiOH required is 21.3 g (to three significant figures) which corresponds only with choice C.

Question 14

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure.What is the Henry's law constant of Cl₂ in water? (R = 0.0821 atm • L • mol^-1• K^-1 )

Accepted Answer

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Question 15

What is the molarity of a 17.0% by mass solution of sodium acetate,NaC₂H₃O₂ (82.0g/mol),in water? The density of the solution is 1.09 g/mL.

Accepted Answer

First, we need to calculate the mass of sodium acetate present in 100 g of the solution.
mass of NaC2H3O2 = 17.0 g
mass of solution = 100 g
mass of water = 100 - 17.0 = 83 g
So, the mass of NaC2H3O2 in 100 g of the solution is 17.0 g.
Using the molar mass of NaC2H3O2, we can calculate the number of moles of NaC2H3O2 in 17.0 g.
Molar mass of NaC2H3O2 = 82.0 g/mol
Number of moles of NaC2H3O2 = 17.0 g / 82.0 g/mol = 0.2073 mol
Now we need to calculate the volume of the solution present in 100 g of the solution.
Density of the solution = 1.09 g/mL
Volume of 100 g solution = 100 g / 1.09 g/mL = 91.74 mL = 0.09174 L
Finally, we can calculate the molarity of the solution using the formula:
Molarity = number of moles of solute / volume of solution in liters
Molarity = 0.2073 mol / 0.09174 L
Molarity = 2.26 M
Therefore, the answer is D) 2.26 M.

Question 16

What volume of concentrated (14.7 M)phosphoric acid is needed to prepare 25.0 L of 3.0 M H₃PO₄?

Accepted Answer

The answer of What volume of concentrated (14.7 M)phosphoric acid...

Question 17

What is the quantitative relationship between gas solubility and pressure?

Accepted Answer

Henry's law states that at a constant temperature, the amount of a gas dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid. Therefore, as pressure increases, gas solubility also increases proportionally.

Question 18

What mass of water is required to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution?

Accepted Answer

The answer of What mass of water is required to...

Question 19

What volume of a 2.75 M solution of NaOH is required to make 500.0 mL of a 1.27 M solution of NaOH?

Accepted Answer

To find the volume of the 2.75 M solution needed to make 500.0 mL of a 1.27 M solution, use the dilution formula $M_1V_1 = M_2V_2$, where $M_1$ and $V_1$ are the molarity and volume of the initial solution, and $M_2$ and $V_2$ are the molarity and volume of the final solution. Plugging in the given values: $2.75M \times V_1 = 1.27M \times 500.0mL$, solving for $V_1$ gives approximately 231 mL.

Question 20

What states that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution?

Accepted Answer

This statement is known as Henry's law.

Quiz 13: Physical Properties of Solutions

Calculate the molality of a 20.0% by mass ammonium sulfate (NH₄) ₂SO₄ solution.The density of the solution is 1.117 g/mL.

The density of a 20.3 M CH₃OH (methanol) solution is 0.858 g/mL.What is the molality of this solution? H₂O is the solvent.

The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10^-4 mol/L.What is the value of the Henry's law constant in mol L^-1• atm^-1?

What is the molarity of a solution prepared by diluting 1.85 L of 6.5 M KOH to 11.0 L?

Calcium nitrite is used as a corrosion inhibitor in lubricants.What is the molality of a solution prepared by dissolving 18.5 g of calcium nitrite in 83.5 g of distilled water?

Cadmium bromide is used in photography and lithography.What is the molality of a solution prepared by dissolving 45.38 g of CdBr₂ in 375.0 g of water?

Copper(II) bromide is used as a wood preservative.What mass of CuBr₂ is needed to prepare 750.0 mL of a 1.25 M solution?

What is the molarity of a solution of 10.0% by mass cadmium sulfate,CdSO₄ (208.47g/mol) ? The density of the solution is 1.10 g/mL.

What is the molality of a solution prepared by dissolving 84.7 g of KMnO₄ in 165 g of water?

What mass of water is required to dissolve 25.31 g of potassium nitrate (KNO₃) in order to prepare a 0.1982 m solution?

Which combination of a 36.0% (w/w) stock solution of acetic acid (d = 1.045 g/mL) and water will result in 1.00 kg of a 15.0% (w/w) acetic acid solution?

What mass of LiOH is required to prepare 0.250 L of a 3.55 M solution?

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure.What is the Henry's law constant of Cl₂ in water? (R = 0.0821 atm • L • mol^-1• K^-1 )

What is the molarity of a 17.0% by mass solution of sodium acetate,NaC₂H₃O₂ (82.0g/mol) ,in water? The density of the solution is 1.09 g/mL.

What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H₃PO₄?

What is the quantitative relationship between gas solubility and pressure?

What mass of water is required to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution?

What volume of a 2.75 M solution of NaOH is required to make 500.0 mL of a 1.27 M solution of NaOH?

What states that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution?

Quiz 13: Physical Properties of Solutions

Calculate the molality of a 20.0% by mass ammonium sulfate (NH4) 2SO4 solution.The density of the solution is 1.117 g/mL.

The density of a 20.3 M CH3OH (methanol) solution is 0.858 g/mL.What is the molality of this solution? H2O is the solvent.

The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10-4 mol/L.What is the value of the Henry's law constant in mol L-1• atm-1?

What is the molarity of a solution prepared by diluting 1.85 L of 6.5 M KOH to 11.0 L?

Calcium nitrite is used as a corrosion inhibitor in lubricants.What is the molality of a solution prepared by dissolving 18.5 g of calcium nitrite in 83.5 g of distilled water?

Cadmium bromide is used in photography and lithography.What is the molality of a solution prepared by dissolving 45.38 g of CdBr2 in 375.0 g of water?

Copper(II) bromide is used as a wood preservative.What mass of CuBr2 is needed to prepare 750.0 mL of a 1.25 M solution?

What is the molarity of a solution of 10.0% by mass cadmium sulfate,CdSO4 (208.47g/mol) ? The density of the solution is 1.10 g/mL.

What is the molality of a solution prepared by dissolving 84.7 g of KMnO4 in 165 g of water?

What mass of water is required to dissolve 25.31 g of potassium nitrate (KNO3) in order to prepare a 0.1982 m solution?

Which combination of a 36.0% (w/w) stock solution of acetic acid (d = 1.045 g/mL) and water will result in 1.00 kg of a 15.0% (w/w) acetic acid solution?

What mass of LiOH is required to prepare 0.250 L of a 3.55 M solution?

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure.What is the Henry's law constant of Cl2 in water? (R = 0.0821 atm • L • mol-1• K-1 )

What is the molarity of a 17.0% by mass solution of sodium acetate,NaC2H3O2 (82.0g/mol) ,in water? The density of the solution is 1.09 g/mL.

What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H3PO4?

What is the quantitative relationship between gas solubility and pressure?

What mass of water is required to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution?

What volume of a 2.75 M solution of NaOH is required to make 500.0 mL of a 1.27 M solution of NaOH?

What states that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution?

Calculate the molality of a 20.0% by mass ammonium sulfate (NH₄) ₂SO₄ solution.The density of the solution is 1.117 g/mL.

The density of a 20.3 M CH₃OH (methanol) solution is 0.858 g/mL.What is the molality of this solution? H₂O is the solvent.

The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10^-4 mol/L.What is the value of the Henry's law constant in mol L^-1• atm^-1?

Cadmium bromide is used in photography and lithography.What is the molality of a solution prepared by dissolving 45.38 g of CdBr₂ in 375.0 g of water?

Copper(II) bromide is used as a wood preservative.What mass of CuBr₂ is needed to prepare 750.0 mL of a 1.25 M solution?

What is the molarity of a solution of 10.0% by mass cadmium sulfate,CdSO₄ (208.47g/mol) ? The density of the solution is 1.10 g/mL.

What is the molality of a solution prepared by dissolving 84.7 g of KMnO₄ in 165 g of water?

What mass of water is required to dissolve 25.31 g of potassium nitrate (KNO₃) in order to prepare a 0.1982 m solution?

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure.What is the Henry's law constant of Cl₂ in water? (R = 0.0821 atm • L • mol^-1• K^-1 )

What is the molarity of a 17.0% by mass solution of sodium acetate,NaC₂H₃O₂ (82.0g/mol) ,in water? The density of the solution is 1.09 g/mL.

What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H₃PO₄?

What mass of water is required to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution?