Question 1

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 2

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

Accepted Answer

Use the equation:

M1V1 = M2V2

Where:
M1 = 12.0 M (the initial molarity)
V1 = ? (the volume we need to find)
M2 = 3.50 M (the final molarity)
V2 = 75.0 mL (the final volume)

Rearrange and solve for V1:

V1 = (M2V2) / M1
V1 = (3.50 M × 75.0 mL) / 12.0 M
V1 = 21.9 mL

Therefore, the answer is A) 21.9 mL.

Question 3

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 4

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:
Ba 
(aq)+ N 
S 
(aq)→ BaS 
(s)+ 2NaCl (aq)

Accepted Answer

The balanced chemical equation shows that 1 mole of barium chloride reacts with 1 mole of sodium chloride to produce 1 mole of barium sulfide. Therefore, the number of moles of sodium chloride is equal to the number of moles of barium chloride used in the reaction. The number of moles of barium chloride can be calculated using the volume and concentration given:

moles of BaCl2 = volume (in L) x concentration (in mol/L) = 0.050 L x 0.2 mol/L = 0.01 mol

Therefore, there are 0.01 moles of NaCl in the reaction. The total volume of the reaction is not given, so we cannot directly calculate the concentration of NaCl in the final solution. However, since the reaction is complete, all the barium chloride has reacted to form barium sulfide and all the sodium chloride has remained in solution. Therefore, the final volume of the solution is equal to the initial volume of barium chloride solution, which is 0.050 L. The concentration of NaCl in the final solution is:

concentration of NaCl = moles of NaCl / volume of solution = 0.01 mol / 0.050 L = 0.2 mol/L

This is the concentration of NaCl in the initial barium chloride solution, so we need to take into account that the volume has doubled due to the addition of NaCl. Therefore, the final concentration of NaCl is:

final concentration of NaCl = concentration of NaCl in initial solution / 2 = 0.2 mol/L / 2 = 0.1 mol/L

The final concentration of NaCl is 0.1 mol/L, which is equivalent to 0.0519 g/mL. Therefore, the best choice is C.

Question 5

How many grams of barium sulfate are produced if 
Of 
BaC 
Completely react given the reaction:
Ba 
(aq)+ N 
S 
(aq)→ BaS 
(s)+ 2NaCl (aq)

Accepted Answer

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

Question 6

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

To find the concentration of the diluted solution, we need to use the formula:
M1V1 = M2V2
where M1 and V1 are the initial concentration and volume of the solution, and M2 and V2 are the final concentration and volume of the solution.
We know that V1 = 6.00 mL and M1 = 0.750 M.
When we add water, the total volume becomes V1 + V2 = 6.00 mL + 4.00 mL = 10.00 mL.
So, V2 = 4.00 mL and M2 is what we need to find.
Using the formula, we get:
M1V1 = M2V2
0.750 M x 6.00 mL = M2 x 4.00 mL
M2 = 1.125 M/4.00 mL
M2 = 0.28125 M, which is approximately 0.450 M (rounded to three significant figures). Therefore, the answer is B.

Question 7

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 8

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 9

What is the final concentration of a solution prepared by diluting 
Of 
HCl to a final volume of 
?

Accepted Answer

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

Question 10

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 11

What volume of 9.00 M nitric acid is needed to make 
Of 
Solution?

Accepted Answer

The answer of What volume of 9.00 M nitric acid...

Question 12

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

The answer of How much water would you ADD to...

Question 13

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 14

How many mL of 0.218 M sodium sulfate react with exactly 
Of 
BaC 
Given the reaction:
Ba 
(aq)+ N 
S 
(aq)→ BaS 
(s)+ 2NaCl (aq)

Accepted Answer

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

Question 15

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

Accepted Answer

When a solution is diluted, more solvent is added to decrease the concentration of the solute. This means that the new solution will have more volume but a lower concentration than before.

Question 16

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 17

A 0.15 M solution of BaCl₂ contains:

Accepted Answer

BaCl2 dissociates into Ba2+ and 2Cl- ions. Since there's only one Ba2+ ion, and it reacts with one S2- ion from BaS to form BaS, the concentration of BaS in the final solution is 0.15 M. However, since there are two Cl- ions for every Ba2+ ion, the concentration of Cl- ions in the final solution is 0.15 M x 2 = 0.3 M. Therefore, the correct answer is B.

Question 18

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 19

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

Using the balanced chemical equation, we can see that the mole ratio of KOH to H₂SO₄ is 2:1. Therefore, we can use the following formula to calculate the moles of H₂SO₄: moles of H₂SO₄ = (volume of KOH solution in L) x (M KOH) moles of H₂SO₄ = (55.0 mL / 1000 mL/L) x (2.50 mol/L) = 0.1375 mol To find the volume of the H₂SO₄ solution needed, we can use the following formula: (volume of H₂SO₄ solution in L) x (0.755 mol/L) = 0.1375 mol volume of H₂SO₄ solution = 0.1375 mol / 0.755 mol/L = 0.182 L = 182 mL Therefore, the answer is C) 91.1 mL.

Question 20

What molarity should the stock solution be if you want to dilute 
To 
And have the final concentration be 
?

Accepted Answer

The answer of What molarity should the stock solution be...

Quiz 13: Solutions

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

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

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

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: Ba (aq) + N S (aq) → BaS (s) + 2NaCl (aq)

How many grams of barium sulfate are produced if Of BaC Completely react given the reaction: Ba (aq) + N S (aq) → BaS (s) + 2NaCl (aq)

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?

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.

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

What is the final concentration of a solution prepared by diluting Of HCl to a final volume of ?

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 Of Solution?

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?

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

How many mL of 0.218 M sodium sulfate react with exactly Of BaC Given the reaction: Ba (aq) + N S (aq) → BaS (s) + 2NaCl (aq)

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

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 ________.

A 0.15 M solution of BaCl₂ contains:

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

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)

What molarity should the stock solution be if you want to dilute To And have the final concentration be ?

Quiz 13: Solutions

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

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

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

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: Ba (aq) + N S (aq) → BaS (s) + 2NaCl (aq)

How many grams of barium sulfate are produced if Of BaC Completely react given the reaction: Ba (aq) + N S (aq) → BaS (s) + 2NaCl (aq)

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?

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.

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

What is the final concentration of a solution prepared by diluting Of HCl to a final volume of ?

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 Of Solution?

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?

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

How many mL of 0.218 M sodium sulfate react with exactly Of BaC Given the reaction: Ba (aq) + N S (aq) → BaS (s) + 2NaCl (aq)

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

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 ________.

A 0.15 M solution of BaCl2 contains:

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

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)

What molarity should the stock solution be if you want to dilute To And have the final concentration be ?

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

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

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

A 0.15 M solution of BaCl₂ contains:

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

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)