Q: Which equation correctly represents molarity ($$M) of a $$solution?

$$M = \frac{\text{moles of solute}}{\text{volume of solution in liters}}$$

Q: Which formula represents normality ($$N) in $$terms of equivalents and volume?

$$N = \frac{\text{equivalents of solute}}{\text{volume of solution in liters}}$$

Question 1

Which of the following best describes a concentrated solution?

Accepted Answer

A solution with a large amount of dissolved solute.

Question 2

In the image provided, which direction represents increasing concentration of the red dye in water?

Accepted Answer

From left to right

Question 3

If you add more solute to a fixed amount of solvent, what happens to the concentration of the solution?

Accepted Answer

The concentration increases

Question 4

Which equation correctly represents molarity ($$M) of a $$solution?

Accepted Answer

$$M = \frac{	ext{moles of solute}}{	ext{volume of solution in liters}}$$

Question 5

A student prepares a solution by dissolving 10 g of NaCl in 100 mL of water. Which term best describes this solution compared to a solution made by dissolving 2 g of NaCl in 100 mL of water?

Accepted Answer

Concentrated

Question 6

Which of the following statements about normality ($$N) is $$correct?

Accepted Answer

Normality is the number of equivalents of solute per liter of solution.

Question 7

What is the main difference between molarity and normality?

Accepted Answer

Molarity is based on moles, normality is based on equivalents.

Question 8

A solution is described as dilute. Which of the following is most likely true?

Accepted Answer

It contains a small amount of solute.

Question 9

If a chemist wants to increase the concentration of a solution, which action should they take?

Accepted Answer

Add more solute

Question 10

Which of the following best describes a real-life scenario involving a concentrated solution?

Accepted Answer

A cleaning product with a high amount of dissolved chemicals

Question 11

A laboratory technician needs to prepare 1 L of a 2 M NaOH solution. How many moles of NaOH are required?

Accepted Answer

2 moles

Question 12

Which formula represents normality ($$N) in $$terms of equivalents and volume?

Accepted Answer

$$N = \frac{	ext{equivalents of solute}}{	ext{volume of solution in liters}}$$

Question 13

A solution is made by dissolving 5 g of glucose in 100 mL of water. If another solution is made by dissolving 5 g of glucose in 500 mL of water, which solution is more concentrated?

Accepted Answer

The solution with 100 mL of water

Question 14

Which of the following is a common misconception about concentrated solutions?

Accepted Answer

They are always colored.

Question 15

A student observes that a solution is very light in color compared to another solution of the same solute. What can they infer about the concentration?

Accepted Answer

The solution is more dilute.

Question 16

Which of the following best explains why molarity and normality are not always equal for a given solution?

Accepted Answer

Normality depends on the type of reaction and the number of equivalents involved.

Question 17

A solution contains 0.5 moles of H$$_2SO$_4 in 1 L of $$water. What is the normality of the solution for acid-base reactions?

Accepted Answer

$$N = 1$$

Question 18

Which of the following would NOT affect the concentration of a solution?

Accepted Answer

Changing the temperature

Question 19

A chemist dilutes a concentrated acid solution by adding water. What happens to the concentration?

Accepted Answer

The concentration decreases

Question 20

Which of the following is the best example of a dilute solution in everyday life?

Accepted Answer

Tap water with a small amount of chlorine

Concentration of Solutions: Molarity vs. Normality

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