Question 1

What is the approximate Na⁺ ion concentration in a 0.75 M Na₂CO₃ solution?

Accepted Answer

In a Na2CO3 solution, each formula unit dissociates into 2 Na+ ions and 1 CO3^2- ion. Therefore, a 0.75 M Na2CO3 solution will produce 2 x 0.75 M = 1.50 M Na+ ions.

Question 2

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

Accepted Answer

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

Question 3

Which of the following aqueous solutions has the lowest freezing point?

Accepted Answer

The freezing point depression is determined by the van't Hoff factor (i) and molality (m). Na₂SO₄ dissociates into 3 ions (2 Na⁺ and 1 SO₄²⁻), giving it the highest effective concentration of particles, resulting in the lowest freezing point.

Question 4

An aqueous dextrose solution having a density of 1.04 g/cm³ freezes at -1.15°C. Find the osmotic pressure of this solution at 25°C.K_f of water is 1.86 °C/m; molecular mass of dextrose = 180.16 g/mol.

Accepted Answer

The freezing point depression is used to find the molality of the solution. ΔTf = i * Kf * m, where ΔTf = 1.15°C, i = 1 (since dextrose is a non-electrolyte), and Kf = 1.86°C/m. Solving for m gives m = 0.618 mol/kg. Using the density, convert molality to molarity: M = m * density = 0.618 mol/kg * 1.04 kg/L = 0.643 mol/L. The osmotic pressure (π) is given by π = MRT, where R = 0.0821 L·atm/mol·K and T = 298 K. π = 0.643 mol/L * 0.0821 L·atm/mol·K * 298 K = 14.1 atm.

Question 5

What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

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Question 6

Consider a 0.90 M Al(NO₃)₃ solution. This solution has a nitrate ion concentration of

Accepted Answer

Al(NO3)3 dissociates into one Al^3+ ion and three NO3^- ions. Therefore, the concentration of nitrate ions is 3 times the concentration of Al(NO3)3, which is 0.90 M x 3 = 2.7 M.

Question 7

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

Accepted Answer

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Question 8

The concentration of nitrogen in water at 25°C was determined to be 7.2 *10^-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 *10^-4 mol/L·atm?

Accepted Answer

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Question 9

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

Accepted Answer

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Question 10

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Accepted Answer

The answer of How many grams of propanol (C₃H₇OH, 60.10...

Question 11

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

The answer of What is the percent by mass of...

Question 12

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO₃, 100.11 g/mol)and has a density of 1.0650 g/mL?

Accepted Answer

The answer of What is the molarity and molality of...

Question 13

A solution is prepared by adding 40.3 g of Mg(NO₃)₂ to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

Accepted Answer

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Question 14

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol).Calculate the mole fraction and molality of benzene in this solution.

Accepted Answer

The answer of A solution is prepared by adding 6.24...

Question 15

What is the osmotic pressure of a solution prepared from 13.7 g of the electrolyte HCl and enough water to make 0.500 L of solution at 18°C?

Accepted Answer

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Question 16

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

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Question 17

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO₃)₂; 0.100 m ethanol; 0.090 m NaCl.

Accepted Answer

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Question 18

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution freezes.[Given: for water K_f = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

Accepted Answer

The answer of An aqueous fructose solution having a density...

Question 19

The osmotic pressure of a 0.010 M MgSO₄ solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO₄ solution.

Accepted Answer

The answer of The osmotic pressure of a 0.010 M...

Question 20

What is the concentration of O₂(g)in water at 25°C exposed to a partial pressure of oxygen of 325 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10^-3 mol/L·atm.

Accepted Answer

The answer of What is the concentration of O₂(g)in water...

Quiz 12: Physical Properties of Solutions

What is the approximate Na⁺ ion concentration in a 0.75 M Na₂CO₃ solution?

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

Which of the following aqueous solutions has the lowest freezing point?

An aqueous dextrose solution having a density of 1.04 g/cm³ freezes at -1.15°C. Find the osmotic pressure of this solution at 25°C.K_f of water is 1.86 °C/m; molecular mass of dextrose = 180.16 g/mol.

What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Consider a 0.90 M Al(NO₃) ₃ solution. This solution has a nitrate ion concentration of

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

The concentration of nitrogen in water at 25°C was determined to be 7.2 10^-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 10^-4 mol/L·atm?

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO₃, 100.11 g/mol)and has a density of 1.0650 g/mL?

A solution is prepared by adding 40.3 g of Mg(NO₃)₂ to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol).Calculate the mole fraction and molality of benzene in this solution.

What is the osmotic pressure of a solution prepared from 13.7 g of the electrolyte HCl and enough water to make 0.500 L of solution at 18°C?

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO₃) ₂; 0.100 m ethanol; 0.090 m NaCl.

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution freezes.[Given: for water K_f = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

The osmotic pressure of a 0.010 M MgSO₄ solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO₄ solution.

What is the concentration of O₂(g)in water at 25°C exposed to a partial pressure of oxygen of 325 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10^-3 mol/L·atm.

Quiz 12: Physical Properties of Solutions

What is the approximate Na+ ion concentration in a 0.75 M Na2CO3 solution?

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C2H2O4)and has a density of 1.0244 g/mL?

Which of the following aqueous solutions has the lowest freezing point?

An aqueous dextrose solution having a density of 1.04 g/cm3 freezes at -1.15°C. Find the osmotic pressure of this solution at 25°C.Kf of water is 1.86 °C/m; molecular mass of dextrose = 180.16 g/mol.

What is the molality of a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Consider a 0.90 M Al(NO3) 3 solution. This solution has a nitrate ion concentration of

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 102 g of H2O. [Kf of water is 1.86°C/m.]

The concentration of nitrogen in water at 25°C was determined to be 7.2 *10-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 *10-4 mol/L·atm?

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

How many grams of propanol (C3H7OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO3, 100.11 g/mol)and has a density of 1.0650 g/mL?

A solution is prepared by adding 40.3 g of Mg(NO3)2 to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

A solution is prepared by adding 6.24 g of benzene (C6H6, 78.11 g/mol)to 80.74 g of cyclohexane (C6H12, 84.16 g/mol).Calculate the mole fraction and molality of benzene in this solution.

What is the osmotic pressure of a solution prepared from 13.7 g of the electrolyte HCl and enough water to make 0.500 L of solution at 18°C?

What is the mole fraction of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO3) 2; 0.100 m ethanol; 0.090 m NaCl.

An aqueous fructose solution having a density of 1.049 g/cm3 is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution freezes.[Given: for water Kf = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

The osmotic pressure of a 0.010 M MgSO4 solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO4 solution.

What is the concentration of O2(g)in water at 25°C exposed to a partial pressure of oxygen of 325 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10-3 mol/L·atm.

What is the approximate Na⁺ ion concentration in a 0.75 M Na₂CO₃ solution?

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

An aqueous dextrose solution having a density of 1.04 g/cm³ freezes at -1.15°C. Find the osmotic pressure of this solution at 25°C.K_f of water is 1.86 °C/m; molecular mass of dextrose = 180.16 g/mol.

What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Consider a 0.90 M Al(NO₃) ₃ solution. This solution has a nitrate ion concentration of

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

The concentration of nitrogen in water at 25°C was determined to be 7.2 10^-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 10^-4 mol/L·atm?

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO₃, 100.11 g/mol)and has a density of 1.0650 g/mL?

A solution is prepared by adding 40.3 g of Mg(NO₃)₂ to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol).Calculate the mole fraction and molality of benzene in this solution.

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO₃) ₂; 0.100 m ethanol; 0.090 m NaCl.

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution freezes.[Given: for water K_f = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

The osmotic pressure of a 0.010 M MgSO₄ solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO₄ solution.

What is the concentration of O₂(g)in water at 25°C exposed to a partial pressure of oxygen of 325 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10^-3 mol/L·atm.