Question 1

What is the concentration of sodium chloride in the final solution if   of   BaC  completely reacts and the total volume of the reaction is  , given the reaction:

Accepted Answer

Step 1: Identify the limiting reactant: BaCl2

Step 2: Use stoichiometry to determine the number of moles of NaCl produced:

1 mole of BaCl2 produces 2 moles of NaCl

Therefore, 0.215 mole of BaCl2 produces 2*0.215 = 0.43 moles of NaCl

Step 3: Calculate the concentration of NaCl:

C = n/V

C = 0.43 moles / 8.28 L

C = 0.0519 M

Therefore, the concentration of NaCl in the final solution is 0.0519 M.

The answer is C.

Question 2

Which one of the following aqueous solutions would have the higher concentration of K⁺ (aq)ions? (Assume total solubility in water.)

Accepted Answer

The compound that leads to the formation of K⁺(aq) ions is K2S1U1, and D is the only option that contains K2S1U1. Therefore, it has the higher concentration of K⁺(aq) ions.

Question 3

How many milliliters of 0.755 M H₂SO₄ solution is needed to react with 55.0 mL of 2.50 M KOH solution? Given: 2 KOH (aq)+ H₂SO₄ (aq)→ 2 H₂O (l)+ K₂SO₄ (aq)

Accepted Answer

To solve this problem, we need to use stoichiometry and the equation given to us. First, let's balance the equation: 2 KOH (aq) + H₂SO₄ (aq) → 2 H₂O (l) + K₂SO₄ (aq) We can see that the ratio of KOH and H₂SO₄ is 2:1, which means that for every 2 moles of KOH, we need 1 mole of H₂SO₄ to react. We can use the equation: moles = concentration (M) x volume (L) to find the number of moles of KOH we have: moles of KOH = concentration (2.50 M) x volume (55.0 mL / 1000 mL/L) = 0.1375 mol Since the ratio of KOH to H₂SO₄ is 2:1, we need half the number of moles of H₂SO₄: moles of H₂SO₄ = 0.1375 mol / 2 = 0.06875 mol Finally, we can use the equation: volume (L) = moles / concentration (M) to find the volume of 0.755 M H₂SO₄ we need: volume of H₂SO₄ = 0.06875 mol / 0.755 M = 0.0911 L = 91.1 mL Therefore, the best choice is C.

Question 4

Which solution below contains the highest total quantity of dissolved sodium ions?

Accepted Answer

The answer of Which solution below contains the highest total...

Question 5

In comparing a 0.25 molality aqueous NaCl solution to a 0.25 molality aqueous CaCl₂ solution:

Accepted Answer

The CaCl2 solution has a higher boiling point and a lower freezing point due to the van't Hoff factor. CaCl2 dissociates into three ions (Ca^2+ and 2 Cl^-), while NaCl dissociates into two ions (Na^+ and Cl^-), leading to a greater colligative effect for CaCl2.

Question 6

What volume of 9.00 M nitric acid is needed to make 6.50L of 1.25M solution?

Accepted Answer

M1V1 = M2V29.00 M * V1 = 1.25 M * 6.50 LV1 = 0.903 L = 903 mL

Question 7

After you have completed the task of diluting a solution,which statement below must be TRUE?

Accepted Answer

Dilution involves adding solvent to a solution to decrease its concentration. This means that the new solution will have more volume (due to the addition of solvent) but a lower concentration (due to the dilution). Therefore, choice A is the correct answer.

Question 8

What mass (in grams)of fructose (C₆H₁₂O₆)is contained in 125 mL of a 0.500 M fructose solution?

Accepted Answer

To find the mass of fructose in grams, first calculate the molar mass of fructose (C6H12O6). The molar mass is approximately 180.16 g/mol. Then, use the concentration and volume to find moles of fructose: 0.500 moles/L * 0.125 L = 0.0625 moles. Finally, multiply the moles by the molar mass to get the mass in grams: 0.0625 moles * 180.16 g/mol = 11.26 g, which rounds to 11.3 g.

Question 9

What are the ion concentrations in a 0.12 M solution of AlCl₃?

Accepted Answer

AlCl3 dissociates into one Al^3+ ion and three Cl^- ions for every formula unit that dissolves. Therefore, a 0.12 M solution of AlCl3 will have 0.12 M Al^3+ ions and 0.36 M Cl^- ions (0.12 M * 3).

Question 10

How much water would you ADD to 175 mL of 6.00 M hydrochloric acid to prepare a 2.00 M solution of this acid?

Accepted Answer

To dilute the solution, use the formula M1V1 = M2V2. Here, M1 = 6.00 M, V1 = 175 mL, M2 = 2.00 M. Solving for V2 gives V2 = 525 mL. The amount of water to add is V2 - V1 = 525 mL - 175 mL = 350 mL.

Question 11

What molarity should the stock solution be if you want to dilute 25.0mL to 2.00L and have the final concentration be 0.103M ?

Accepted Answer

First, use the dilution equation: 
M1V1 = M2V2 
where M1 is the initial concentration (unknown), V1 is the initial volume (25.0 mL = 0.025 L), M2 is the final concentration (0.103 M), and V2 is the final volume (2.00 L). 
Rearranging the equation to solve for M1: 
M1 = (M2V2)/V1 
M1 = (0.103 M)(2.00 L)/(0.025 L) 
M1 = 8.24 M 
Therefore, the stock solution should be 8.24 M in order to dilute 25.0 mL to 2.00 L and have the final concentration be 0.103 M.

Question 12

If you add 4.00 mL of pure water to 6.00 mL of 0.750 M NaCl solution,what is the concentration of sodium chloride in the diluted solution?

Accepted Answer

Before dilution:
moles of NaCl = (6.00 mL) x (0.750 mol/L) = 4.5 mmol
After dilution:
total volume = 4.00 mL + 6.00 mL = 10.00 mL
moles of NaCl = 4.5 mmol
concentration = moles / volume = 4.5 mmol / 10.00 mL = 0.450 M

Question 13

How many grams of barium sulfate are produced if 25.34mL of 0.113M BaCl₂ completely react given the reaction: BaCl₂(aq)+ Na₂SO₄ (aq)→ BaSO₄ (s)+ 2NaCl (aq)

Accepted Answer

The answer of How many grams of barium sulfate are...

Question 14

How many mL of 0.218 M sodium sulfate react with exactly   of   BaC  given the reaction:

Accepted Answer

The answer of How many mL of 0.218 M sodium...

Question 15

A 0.15 M solution of BaCl₂ contains:

Accepted Answer

BaCl2 dissociates into one Ba2+ ion and two Cl- ions. Ba2+ reacts with S2- ions to form BaS solid, leaving half the Cl- ions remaining in solution. Therefore, the solution contains 0.15 M Ba2+ ions and 0.30 M Cl- ions. BaS dissociates into one Ba2+ ion and one S2- ion, so the solution also contains 0.15 M S2- ions. Therefore, choice B is correct, as it contains 0.15 M BaS and 0.30 M Cl-.

Question 16

How many liters of a 2.18 M solution can be made from   S?

Accepted Answer

The answer of How many liters of a 2.18 M...

Question 17

What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a final volume of 1.20L ?

Accepted Answer

The answer of What is the final concentration of a...

Question 18

Oftentimes solubility of a compound limits the concentration of the solution that can be prepared.Use the solubility data given with each compound shown below to determine which compound would allow the preparation of a 10.0 Molar solution.

Accepted Answer

The answer of Oftentimes solubility of a compound limits the...

Question 19

A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final volume of 3.00 liters.The molarity of the final solution is ________.

Accepted Answer

The answer of A 90.0 g sample of NaOH is...

Question 20

What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?

Accepted Answer

Use the dilution formula:

M1V1 = M2V2

Where:

M1 = 12.0 M (initial concentration)
V1 = unknown (volume of 12.0 M HCl to be used)
M2 = 3.50 M (final concentration)
V2 = 75.0 mL (final volume)

Solving for V1:

V1 = (M2 x V2) / M1

V1 = (3.50 M x 75.0 mL) / 12.0 M

V1 = 21.9 mL

Therefore, the answer is A) 21.9 mL

Quiz 13: Solutions

What is the concentration of sodium chloride in the final solution if of BaC completely reacts and the total volume of the reaction is , given the reaction:

Which one of the following aqueous solutions would have the higher concentration of K⁺ (aq) ions? (Assume total solubility in water.)

How many milliliters of 0.755 M H₂SO₄ solution is needed to react with 55.0 mL of 2.50 M KOH solution? Given: 2 KOH (aq) + H₂SO₄ (aq) → 2 H₂O (l) + K₂SO₄ (aq)

Which solution below contains the highest total quantity of dissolved sodium ions?

In comparing a 0.25 molality aqueous NaCl solution to a 0.25 molality aqueous CaCl₂ solution:

What volume of 9.00 M nitric acid is needed to make 6.50L of 1.25M solution?

After you have completed the task of diluting a solution,which statement below must be TRUE?

What mass (in grams) of fructose (C₆H₁₂O₆) is contained in 125 mL of a 0.500 M fructose solution?

What are the ion concentrations in a 0.12 M solution of AlCl₃?

How much water would you ADD to 175 mL of 6.00 M hydrochloric acid to prepare a 2.00 M solution of this acid?

What molarity should the stock solution be if you want to dilute 25.0mL to 2.00L and have the final concentration be 0.103M ?

If you add 4.00 mL of pure water to 6.00 mL of 0.750 M NaCl solution,what is the concentration of sodium chloride in the diluted solution?

How many grams of barium sulfate are produced if 25.34mL of 0.113M BaCl₂ completely react given the reaction: BaCl₂(aq) + Na₂SO₄ (aq) → BaSO₄ (s) + 2NaCl (aq)

How many mL of 0.218 M sodium sulfate react with exactly of BaC given the reaction:

A 0.15 M solution of BaCl₂ contains:

How many liters of a 2.18 M solution can be made from S?

What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a final volume of 1.20L ?

Oftentimes solubility of a compound limits the concentration of the solution that can be prepared.Use the solubility data given with each compound shown below to determine which compound would allow the preparation of a 10.0 Molar solution.

A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final volume of 3.00 liters.The molarity of the final solution is ________.

What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?

Quiz 13: Solutions

What is the concentration of sodium chloride in the final solution if of BaC completely reacts and the total volume of the reaction is , given the reaction:

Which one of the following aqueous solutions would have the higher concentration of K+ (aq) ions? (Assume total solubility in water.)

How many milliliters of 0.755 M H2SO4 solution is needed to react with 55.0 mL of 2.50 M KOH solution? Given: 2 KOH (aq) + H2SO4 (aq) → 2 H2O (l) + K2SO4 (aq)

Which solution below contains the highest total quantity of dissolved sodium ions?

In comparing a 0.25 molality aqueous NaCl solution to a 0.25 molality aqueous CaCl2 solution:

What volume of 9.00 M nitric acid is needed to make 6.50L of 1.25M solution?

After you have completed the task of diluting a solution,which statement below must be TRUE?

What mass (in grams) of fructose (C6H12O6) is contained in 125 mL of a 0.500 M fructose solution?

What are the ion concentrations in a 0.12 M solution of AlCl3?

How much water would you ADD to 175 mL of 6.00 M hydrochloric acid to prepare a 2.00 M solution of this acid?

What molarity should the stock solution be if you want to dilute 25.0mL to 2.00L and have the final concentration be 0.103M ?

If you add 4.00 mL of pure water to 6.00 mL of 0.750 M NaCl solution,what is the concentration of sodium chloride in the diluted solution?

How many grams of barium sulfate are produced if 25.34mL of 0.113M BaCl2 completely react given the reaction: BaCl2(aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaCl (aq)

How many mL of 0.218 M sodium sulfate react with exactly of BaC given the reaction:

A 0.15 M solution of BaCl2 contains:

How many liters of a 2.18 M solution can be made from S?

What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a final volume of 1.20L ?

Oftentimes solubility of a compound limits the concentration of the solution that can be prepared.Use the solubility data given with each compound shown below to determine which compound would allow the preparation of a 10.0 Molar solution.

A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final volume of 3.00 liters.The molarity of the final solution is ________.

What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?

Which one of the following aqueous solutions would have the higher concentration of K⁺ (aq) ions? (Assume total solubility in water.)

How many milliliters of 0.755 M H₂SO₄ solution is needed to react with 55.0 mL of 2.50 M KOH solution? Given: 2 KOH (aq) + H₂SO₄ (aq) → 2 H₂O (l) + K₂SO₄ (aq)

In comparing a 0.25 molality aqueous NaCl solution to a 0.25 molality aqueous CaCl₂ solution:

What mass (in grams) of fructose (C₆H₁₂O₆) is contained in 125 mL of a 0.500 M fructose solution?

What are the ion concentrations in a 0.12 M solution of AlCl₃?

How many grams of barium sulfate are produced if 25.34mL of 0.113M BaCl₂ completely react given the reaction: BaCl₂(aq) + Na₂SO₄ (aq) → BaSO₄ (s) + 2NaCl (aq)

A 0.15 M solution of BaCl₂ contains: