Question 1

How many grams of NaCl are required to prepare 500. mL of an aqueous 0.500 M NaCl solution?
MM(NaCl) = 58.44 g/mol

Accepted Answer

We can use the formula:
Molarity (M) = moles of solute (n) / volume of solution in liters (V)

Rearranging the formula, we get:
moles of solute (n) = Molarity (M) x volume of solution in liters (V)

Substituting the given values, we get:
n = 0.500 mol/L x 0.500 L = 0.25 mol

Now, we can use the molar mass of NaCl to convert the moles of NaCl to grams:
mass = moles x molar mass
mass = 0.25 mol x 58.44 g/mol = 14.61 g

Therefore, the answer is B (14.6 g NaCl).

Question 2

How many moles of H₂SO₄ are present in 211 mL of a 4.36 molar solution?

Accepted Answer

To calculate the number of moles of a solute present in a solution, we use the formula: moles of solute = molarity x volume (in liters) We are given the molarity of the solution as 4.36 M and the volume as 211 mL. We need to convert the volume to liters by dividing by 1000: 211 mL ÷ 1000 = 0.211 L Now, we can plug in the values: moles of H₂SO₄ = 4.36 M x 0.211 L = 0.920 mol Therefore, the correct answer is C.

Question 3

How many grams of NH₃ are present in 2.50 L of 3.00 M NH₃ solution? Molar Mass(NH₃) = 17.03 g/mol

Accepted Answer

The answer of How many grams of NH₃ are present...

Question 4

How many grams of HCl are present in 2.50 L of 3.00 M HCl solution?
Molar Mass(HCl) = 36.46 g/mol

Accepted Answer

To find the grams of HCl in the solution, use the formula: mass = molarity × volume × molar mass. Here, mass = 3.00 M × 2.50 L × 36.46 g/mol = 273 g HCl.

Question 5

How many milliliters of 1.50 M KOH solution are needed to provide 0.125 moles of KOH?

Accepted Answer

We can use the formula: moles = concentration x volume (in liters)
0.125 moles = 1.50 M x volume (in liters)
Volume (in liters) = 0.125 moles / 1.50 M
Volume (in liters) = 0.0833 L
Volume (in milliliters) = 83.3 mL

Question 6

What volume in milliliters of a 0.200 M NaCl solution is required to provide 1.00 grams of NaCl?
Molar Mass(NaCl) = 58.44 g/mol

Accepted Answer

The answer of What volume in milliliters of a 0.200...

Question 7

How many moles of KNO₃ are present in 45.6 mL of a 3.11 molar solution?

Accepted Answer

We can use the formula:
moles = molarity x volume (in liters)
First, we need to convert the volume from milliliters to liters:
45.6 mL = 0.0456 L
Now we can substitute the values into the formula:
moles = 3.11 mol/L x 0.0456 L
moles = 0.141816 mol
To the correct number of significant figures, the answer is 0.142 mol. Therefore, the best choice is A) 0.142 mol.

Question 8

How many grams of NaF are needed to make 250 mL of a 0.22 molar solution?

Accepted Answer

To find the grams of NaF needed, use the formula: grams = molarity (M) × volume (L) × molar mass (g/mol). The molar mass of NaF is approximately 42 g/mol. For a 0.22 M solution in 0.250 L, the calculation is: 0.22 mol/L × 0.250 L × 42 g/mol = 2.31 g, which rounds to 2.3 g.

Question 9

How many grams of KCl is required to prepared 500 mL of a 2.50 M aqueous solution of KCl?
Molar Mass(KCl) = 74.55 g/mol

Accepted Answer

To prepare a 2.50 M solution of KCl in 500 mL (or 0.5 L), you need to calculate the amount of KCl using the formula: moles = molarity × volume (in liters). For a 2.50 M solution, this is 2.50 moles/L × 0.5 L = 1.25 moles of KCl. The mass of KCl required is then calculated by multiplying the moles by the molar mass of KCl (74.55 g/mol), resulting in 1.25 moles × 74.55 g/mol = 93.2 g of KCl.

Question 10

How many grams of H₂SO₄ are present in 75.0 mL of 12.0 M H₂SO₄? Molar Mass (H₂SO₄) = 98.09 g/mol

Accepted Answer

We can use the formula: moles = concentration x volume First, we need to calculate the number of moles of H₂SO₄ in 75.0 mL of 12.0 M solution: moles = 12.0 mol/L x 0.0750 L = 0.9 mol Next, we can use the molar mass of H₂SO₄ to convert moles to grams: grams = moles x molar mass grams = 0.9 mol x 98.09 g/mol = 88.3 g Therefore, there are 88.3 g of H₂SO₄ present in 75.0 mL of 12.0 M solution.

Question 11

How many moles of OH^- ions are present in 422 mL of a 1.21 molar solution of Ba(OH)₂?

Accepted Answer

Ba(OH)₂ dissociates into one Ba²⁺ ion and two OH⁻ ions. Therefore, a 1.21 M solution of Ba(OH)₂ will produce 2 * 1.21 M = 2.42 M of OH⁻ ions. The volume of the solution is 0.422 L. Thus, the moles of OH⁻ ions = 2.42 M * 0.422 L = 1.02 mol.

Question 12

How many moles of NO₃^- ions are present in 533 mL of a 0.111 molar solution of Ca(NO₃)₂?

Accepted Answer

The solution contains 0.111 moles of Ca(NO3)2 per liter. Since each formula unit of Ca(NO3)2 produces 2 NO3- ions, the moles of NO3- ions are 2 * 0.111 mol/L * 0.533 L = 0.118 mol.

Question 13

How many grams of AgNO₃ are present in 50.0 mL of a 12.0 M AgNO₃ solution? Molar Mass(AgNO₃) = 169.88 g/mol

Accepted Answer

The answer of How many grams of AgNO₃ are present...

Question 14

How many grams of sodium chloride are needed to prepare 1.4 L of a 1.0 molar solution of sodium chloride?

Accepted Answer

To calculate the amount of sodium chloride needed to prepare a 1.0 molar solution in 1.4 L of solution, we use the formula:
moles = concentration x volume
Moles of NaCl = 1.0 mol/L x 1.4 L = 1.4 mol
The molar mass of NaCl is approximately 58.44 g/mol.
The amount of NaCl needed is:
mass = moles x molar mass = 1.4 mol x 58.44 g/mol = 81.816 g
Rounding to the nearest gram gives 82 g. Therefore, the answer is A) 82 g.

Question 15

How many moles of Na₃PO₄ are present in 5.00 mL of a 0.226 molar solution?

Accepted Answer

First, we need to determine the formula weight of Na₃PO₄: Na₃PO₄ = 23.0 + 32.1 + (4x16.0) + 30.9 + (4x16.0) + 32.1 + (4x16.0) = 322.2 g/mol Next, we can use the formula: moles = concentration (in mol/mL) x volume (in mL) to calculate the number of moles of Na₃PO₄ in 5.00 mL of the 0.226 molar solution: moles = 0.226 mol/mL x 0.00500 L = 0.00113 mol Finally, we can convert moles to scientific notation to match the format in the answer choices: moles = 1.13 x 10^-3 mol Therefore, the answer is choice A: 1.13 x 10^-3 mol.

Question 16

How many moles of Ca²⁺ ions are present in 15.6 mL of a 1.21 molar solution of CaCl₂?

Accepted Answer

To find the moles of Ca²⁺ ions, use the formula: moles = molarity × volume (in liters). Convert 15.6 mL to liters (0.0156 L) and multiply by the molarity (1.21 mol/L) to get 0.018876 mol, which rounds to 0.0189 mol.

Question 17

How many grams of potassium sulfate are needed to prepare 2.44 L of a 0.0333 molar solution of potassium sulfate?

Accepted Answer

Firstly, we need to calculate the number of moles of potassium sulfate required to prepare the solution.

Molarity = moles of solute / liters of solution

0.0333 M = x / 2.44 L

x = 0.081132 moles

Next, we need to use the molar mass of potassium sulfate to convert moles to grams.

molar mass of K2SO4 = 174.259 g/mol

mass = moles x molar mass

mass = 0.081132 mol x 174.259 g/mol

mass = 14.2 g

Therefore, the answer is D) 14.2 g.

Question 18

How many grams of solute is present in 164.1 mL of 0.207 M calcium acetate, Ca(C₂H₃O₂)₂? Molar Mass(Ca(C₂H₃O₂)₂) = 158.17 g/mol

Accepted Answer

The answer of How many grams of solute is present...

Question 19

How many moles of K⁺ ions are present in 2.00 L of a 0.211 molar solution of K₂SO₄?

Accepted Answer

We need to use the mole concept and stoichiometry to determine the number of moles of K⁺ ions in the given solution. First, we need to write a balanced equation for the dissociation of K₂SO₄: K₂SO₄ -> K+ + ⁺ From the equation, we see that one mole of K₂SO₄ dissociates to form one mole of ⁺ ions. Next, we use the formula: moles = molarity x volume to calculate the number of moles of K₂SO₄ in 2.00 L of a 0.211 molar solution: moles of K₂SO₄ = 0.211 mol/L x 2.00 L = 0.422 mol Since one mole of K₂SO₄ dissociates to form one mole of ⁺ ions, the number of moles of ⁺ ions in 2.00 L of the solution is also 0.422 mol. Therefore, the answer is B, 0.844 mol (since there are two different ions present in one mole of ⁺).

Question 20

How many grams of silver nitrate (AgNO₃) are present in 255 mL of 2.50 M silver nitrate solution? Molar Mass(AgNO₃) = 169.87 g/mol

Accepted Answer

The answer of How many grams of silver nitrate (AgNO₃)...

Quiz 4: Chemical Reactions in Solution

How many grams of NaCl are required to prepare 500. mL of an aqueous 0.500 M NaCl solution? MM(NaCl) = 58.44 g/mol

How many moles of H₂SO₄ are present in 211 mL of a 4.36 molar solution?

How many grams of NH₃ are present in 2.50 L of 3.00 M NH₃ solution? Molar Mass(NH₃) = 17.03 g/mol

How many grams of HCl are present in 2.50 L of 3.00 M HCl solution? Molar Mass(HCl) = 36.46 g/mol

How many milliliters of 1.50 M KOH solution are needed to provide 0.125 moles of KOH?

What volume in milliliters of a 0.200 M NaCl solution is required to provide 1.00 grams of NaCl? Molar Mass(NaCl) = 58.44 g/mol

How many moles of KNO₃ are present in 45.6 mL of a 3.11 molar solution?

How many grams of NaF are needed to make 250 mL of a 0.22 molar solution?

How many grams of KCl is required to prepared 500 mL of a 2.50 M aqueous solution of KCl? Molar Mass(KCl) = 74.55 g/mol

How many grams of H₂SO₄ are present in 75.0 mL of 12.0 M H₂SO₄? Molar Mass (H₂SO₄) = 98.09 g/mol

How many moles of OH^- ions are present in 422 mL of a 1.21 molar solution of Ba(OH) ₂?

How many moles of NO₃^- ions are present in 533 mL of a 0.111 molar solution of Ca(NO₃) ₂?

How many grams of AgNO₃ are present in 50.0 mL of a 12.0 M AgNO₃ solution? Molar Mass(AgNO₃) = 169.88 g/mol

How many grams of sodium chloride are needed to prepare 1.4 L of a 1.0 molar solution of sodium chloride?

How many moles of Na₃PO₄ are present in 5.00 mL of a 0.226 molar solution?

How many moles of Ca²⁺ ions are present in 15.6 mL of a 1.21 molar solution of CaCl₂?

How many grams of potassium sulfate are needed to prepare 2.44 L of a 0.0333 molar solution of potassium sulfate?

How many grams of solute is present in 164.1 mL of 0.207 M calcium acetate, Ca(C₂H₃O₂) ₂? Molar Mass(Ca(C₂H₃O₂) ₂) = 158.17 g/mol

How many moles of K⁺ ions are present in 2.00 L of a 0.211 molar solution of K₂SO₄?

How many grams of silver nitrate (AgNO₃) are present in 255 mL of 2.50 M silver nitrate solution? Molar Mass(AgNO₃) = 169.87 g/mol

Quiz 4: Chemical Reactions in Solution

How many grams of NaCl are required to prepare 500. mL of an aqueous 0.500 M NaCl solution? MM(NaCl) = 58.44 g/mol

How many moles of H2SO4 are present in 211 mL of a 4.36 molar solution?

How many grams of NH3 are present in 2.50 L of 3.00 M NH3 solution? Molar Mass(NH3) = 17.03 g/mol

How many grams of HCl are present in 2.50 L of 3.00 M HCl solution? Molar Mass(HCl) = 36.46 g/mol

How many milliliters of 1.50 M KOH solution are needed to provide 0.125 moles of KOH?

What volume in milliliters of a 0.200 M NaCl solution is required to provide 1.00 grams of NaCl? Molar Mass(NaCl) = 58.44 g/mol

How many moles of KNO3 are present in 45.6 mL of a 3.11 molar solution?

How many grams of NaF are needed to make 250 mL of a 0.22 molar solution?

How many grams of KCl is required to prepared 500 mL of a 2.50 M aqueous solution of KCl? Molar Mass(KCl) = 74.55 g/mol

How many grams of H2SO4 are present in 75.0 mL of 12.0 M H2SO4? Molar Mass (H2SO4) = 98.09 g/mol

How many moles of OH - ions are present in 422 mL of a 1.21 molar solution of Ba(OH) 2?

How many moles of NO3 - ions are present in 533 mL of a 0.111 molar solution of Ca(NO3) 2?

How many grams of AgNO3 are present in 50.0 mL of a 12.0 M AgNO3 solution? Molar Mass(AgNO3) = 169.88 g/mol

How many grams of sodium chloride are needed to prepare 1.4 L of a 1.0 molar solution of sodium chloride?

How many moles of Na3PO4 are present in 5.00 mL of a 0.226 molar solution?

How many moles of Ca2+ ions are present in 15.6 mL of a 1.21 molar solution of CaCl2?

How many grams of potassium sulfate are needed to prepare 2.44 L of a 0.0333 molar solution of potassium sulfate?

How many grams of solute is present in 164.1 mL of 0.207 M calcium acetate, Ca(C2H3O2) 2? Molar Mass(Ca(C2H3O2) 2) = 158.17 g/mol

How many moles of K+ ions are present in 2.00 L of a 0.211 molar solution of K2SO4?

How many grams of silver nitrate (AgNO3) are present in 255 mL of 2.50 M silver nitrate solution? Molar Mass(AgNO3) = 169.87 g/mol

How many moles of H₂SO₄ are present in 211 mL of a 4.36 molar solution?

How many grams of NH₃ are present in 2.50 L of 3.00 M NH₃ solution? Molar Mass(NH₃) = 17.03 g/mol

How many moles of KNO₃ are present in 45.6 mL of a 3.11 molar solution?

How many grams of H₂SO₄ are present in 75.0 mL of 12.0 M H₂SO₄? Molar Mass (H₂SO₄) = 98.09 g/mol

How many moles of OH^- ions are present in 422 mL of a 1.21 molar solution of Ba(OH) ₂?

How many moles of NO₃^- ions are present in 533 mL of a 0.111 molar solution of Ca(NO₃) ₂?

How many grams of AgNO₃ are present in 50.0 mL of a 12.0 M AgNO₃ solution? Molar Mass(AgNO₃) = 169.88 g/mol

How many moles of Na₃PO₄ are present in 5.00 mL of a 0.226 molar solution?

How many moles of Ca²⁺ ions are present in 15.6 mL of a 1.21 molar solution of CaCl₂?

How many grams of solute is present in 164.1 mL of 0.207 M calcium acetate, Ca(C₂H₃O₂) ₂? Molar Mass(Ca(C₂H₃O₂) ₂) = 158.17 g/mol

How many moles of K⁺ ions are present in 2.00 L of a 0.211 molar solution of K₂SO₄?

How many grams of silver nitrate (AgNO₃) are present in 255 mL of 2.50 M silver nitrate solution? Molar Mass(AgNO₃) = 169.87 g/mol