Question 11 pts

A solution is composed of a solute dissolved in a solvent. The solvent is present in the large amount, whereas the solute is present in the smaller amount. If 20 grams of NaCl are dissolved in 50 grams of water, what is the solute?

a) A mixture of NaCl and water

b) Water

c) NaCl

 

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Question 21 pts

The mass/mass percent concentration is the mass of solute divided by the mass of the solution times 100.

A solution is made by dissolving 15.0 g of glucose C6H12O6 in 100.0 g of water. Calculate the mass percent of glucose in this solution.

a) 15.0%

b) 0.130%

c) 0.150%

d) 13.0%

 

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Question 31 pts

Molarity is the number of moles of solute in 1 liter of solution. If you are given the mass of the solute, be sure to convert it to moles before calculating molarity.

A solution is made by dissolving 0.50 moles of solid NaOH in enough water to make 1.0 L of solution. Calculate the molarity (M) of this solution.

a) 0.50 M

b) 1.0 M

c) 2.0 M

d) 5.0 M

 

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Question 41 pts

Molarity is the number of moles of solute in 1 liter of solution. If you are given the mass of the solute, be sure to convert it to moles before calculating molarity. A solution is made by dissolving 2.50 moles of solid NaOH in enough water to make 100 mL of solution. Calculate the molarity (M) of this solution.

a) 10.0 M

b) 2.5 M

c) 25.0 M

d) 0.25 M

 

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Question 51 pts

Molarity is the number of moles of solute in 1 liter of solution. If you are given the mass of the solute, be sure to convert it to moles before calculating molarity. A solution is made by dissolving 74.55 g of solid KCl in enough water to make 1.00 L of solution. Calculate the molarity (M) of this solution.

a) 2.00 M

b) 0.500 M

c) 1.00 M

d) 0.746 M

 

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Question 61 pts

Molarity is the number of moles of solute in 1 liter of solution. If you are given the mass of the solute, be sure to convert it to moles before calculating molarity.

A solution is made by dissolving 4.35 g of solid NaOH in enough water to make 50.0 mL of solution. Calculate the molarity (M) of this solution.

a) 87.0 M

b) 0.109 M

c) 4.35 M

d) 2.18 M

 

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Question 71 pts

The molarity or volume needed to prepare a dilute solution can be determined by the equation: M1V1 = M2V2 where M1 and V1 are the molarity and volume of the first solution, and M2 and V2 are the molarity and volume of the second solution.

What molarity of nitric acid (HNO3) was used if 2.00 L must be used to prepare 4.5 L of a 0.25 M HNO3 solution?

a) 4.35 M

b) 2.18 M

c) 87.0 M

d) 0.56 M

 

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Question 81 pts

The molarity or volume needed to prepare a dilute solution can be determined by the equation M1V1= M2V2> where M1 and V1 are the molarity and volume of the first solution and M2 and V2 are the molarity and volume of the second solution. 

 

What volume of 12 M nitric acid (HNO3) must be used to prepare 4.5 L of 0.25 M HNO3 solution?

a) 4.5 L

b) 3.0 L

c) 0.094 L

d) 0.25 L

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