Question 1

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?

Accepted Answer

To find parts per million (ppm), you divide the mass of the solute by the total mass of the solution and then multiply by 1,000,000. Here, $ \frac{4.8 \, \text{mg}}{200,000 \, \text{mg}} \times 1,000,000 = 24 \, \text{ppm} $.

Question 2

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?

Accepted Answer

The molality of a solution is calculated using the formula: molality = moles of solute / kilograms of solvent. The molar mass of HCl is approximately 36.46 g/mol. Thus, the moles of HCl = 22.0 g / 36.46 g/mol = 0.603 moles. The mass of the solvent (water) is the total mass minus the mass of HCl, which is 125.0 g - 22.0 g = 103.0 g = 0.103 kg. Therefore, the molality = 0.603 moles / 0.103 kg = 5.86 m.

Question 3

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?

Accepted Answer

The percent-by-volume concentration is calculated by dividing the volume of ethanol by the total volume of the solution and multiplying by 100. (25.0 mL / 250.0 mL) * 100 = 10.0%.

Question 4

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?

Accepted Answer

The answer of A solution of acetic acid, CH₃CO₂H, is...

Question 5

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.

Accepted Answer

The answer of What is the percent-by-mass concentration of antifreeze...

Question 6

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

Accepted Answer

The number of moles of NaCl is calculated using the formula: moles = molarity × volume (in liters). Here, 2.50 M NaCl and 50.0 mL (or 0.050 L) gives 2.50 M × 0.050 L = 0.125 moles.

Question 7

What volume of 3.00 M NaOH contains 1.75 mol NaOH?

Accepted Answer

The equation to use is: moles = concentration x volume. 
Rearranging the equation to solve for volume, we get: volume = moles / concentration. 
Plugging in the values, we get: 
volume = 1.75 mol / 3.00 mol/L
volume = 0.583 L or 583 mL. 
Therefore, the answer is D) 0.583 L.

Question 8

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.

Accepted Answer

To find the percent-by-mass concentration, first calculate the mass of the solution: 1.00 L = 1000 mL, and with a density of 1.10 g/mL, the mass is 1100 g. The percent-by-mass is (mass of solute/mass of solution) x 100 = (263.2 g / 1100 g) x 100 = 23.9%.

Question 9

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

Accepted Answer

The number of moles of NaOH can be calculated using the formula: moles = molarity × volume (in liters). Here, the volume needs to be converted from mL to L: 100.0 mL = 0.100 L. Thus, moles = 3.00 M × 0.100 L = 0.300 moles.

Question 10

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?

Accepted Answer

The answer of A 150.0 g sample of ocean water...

Question 11

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

Accepted Answer

To calculate the number of moles of HCl in 75.0 mL of 2.00 M HCl, we need to use the formula:

moles = concentration (M) x volume (L)

First, we need to convert the volume from milliliters (mL) to liters (L):

75.0 mL = 75.0/1000 L = 0.075 L

Now we can plug in the values:

moles = 2.00 M x 0.075 L = 0.150 moles

Therefore, the answer is C) 0.150 moles.

Question 12

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

Accepted Answer

Al(NO₃)₃ is a strong electrolyte and dissociates completely into its ions in solution. The formula for Al(NO₃)₃ is not given, but we can assume it follows the pattern of other ionic compounds, such as NaCl. In a 2.40 m solution of an ionic compound, there are 2.40 moles of the compound per liter of solution. Each mole of this compound will dissociate into multiple ions, so the molal concentration of ions will be greater than 2.40 m. To find the exact molal concentration of ions, we need to know how many ions are produced by each mole of the compound when it dissociates. Without this information, we cannot calculate the exact molal concentration of ions. However, we can make an estimate. If we assume the formula for Al(NO₃)₃ is similar to NaCl, then each mole of the compound will dissociate into 2 ions (1 Al ion and 1 (NO₃)₃ ion). Therefore, the molal concentration of ions would be 2 x 2.40 m = 4.80 m. However, it is important to note that this is just an estimate and the actual molal concentration of ions could be different depending on the formula of the compound. The closest answer choice to our estimate is C) 9.60 m.

Question 13

What volume of 6.00 M NaOH contains 2.50 mol NaOH?

Accepted Answer

Use the formula: 
moles = concentration (mol/L) x volume (L)
2.50 mol = 6.00 mol/L x volume
Volume = 2.50 mol ÷ 6.00 mol/L = 0.417 L or 417 mL. The answer is (D).

Question 14

A 200.0 g sample of river water contains 6.4 mg of lead. How many parts per million of lead are in the sample?

Accepted Answer

To convert from mg/L to ppm, we need to multiply by 1,000. Therefore, the amount of lead in the sample in ppm is:

(6.4 mg / 200.0 g) * (1,000 ppm / 1 mg) = 32 ppm

Question 15

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

Accepted Answer

Fe(NO3)3 dissociates into 4 ions (1 Fe^3+ and 3 NO3^-), so the total molal concentration of ions is 1.60 m * 4 = 6.40 m.

Question 16

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?

Accepted Answer

The answer of A solution of acetic acid, CH₃CO₂H, is...

Question 17

What volume of 2.00 M HCl contains 0.50 mol HCl?

Accepted Answer

The volume of a solution needed to contain a certain amount of solute can be calculated using the formula: moles of solute = molarity × volume in liters. Rearranging this formula to solve for volume gives: volume = moles of solute / molarity. Plugging in the given values gives: volume = 0.50 mol / 2.00 M = 0.25 L.

Question 18

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?

Accepted Answer

The answer of A solution contains 25.5 g of NaCl...

Question 19

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.

Accepted Answer

The percent-by-mass concentration is calculated using the formula: (mass of solute / mass of solution) * 100%. Given 30.0 g of hydrogen peroxide in 1.00 L (1000 mL) of solution with a density of 1.00 g/mL, the mass of the solution is 1000 g. Thus, the percent-by-mass concentration is (30.0 g / 1000 g) * 100% = 3.00%.

Question 20

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?

Accepted Answer

Molality is calculated as moles of solute per kilogram of solvent. First, calculate the moles of NaOH: $ \frac{15.5 \, \text{g}}{39.997 \, \text{g/mol}} = 0.3875 \, \text{mol} $. The mass of the solvent (water) is $ 125.0 \, \text{g} - 15.5 \, \text{g} = 109.5 \, \text{g} = 0.1095 \, \text{kg} $. Molality = $ \frac{0.3875 \, \text{mol}}{0.1095 \, \text{kg}} = 3.54 \, \text{m} $.

Quiz 11: Solutions

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 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 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 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?

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.

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

What volume of 3.00 M NaOH contains 1.75 mol NaOH?

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.

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

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?

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

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

What volume of 6.00 M NaOH contains 2.50 mol NaOH?

A 200.0 g sample of river water contains 6.4 mg of lead. How many parts per million of lead are in the sample?

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

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?

What volume of 2.00 M HCl contains 0.50 mol HCl?

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?

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 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?

Quiz 11: Solutions

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 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 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 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?

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.

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

What volume of 3.00 M NaOH contains 1.75 mol NaOH?

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.

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

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?

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

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

What volume of 6.00 M NaOH contains 2.50 mol NaOH?

A 200.0 g sample of river water contains 6.4 mg of lead. How many parts per million of lead are in the sample?

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

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?

What volume of 2.00 M HCl contains 0.50 mol HCl?

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?

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 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 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 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?

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.

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.

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

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

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?

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.