Q: A solution has a pH of 4. What is the concentration of hydrogen ions $$[H^+] in $$this solution?

$$[H^+] = 10$$^{-4}$$ \text{ M}$$

Question 1

Which of the following statements best explains why water is considered a versatile solvent in biological systems?

Accepted Answer

Water molecules are polar, allowing them to interact with and dissolve both ionic and polar substances.

Question 2

An atom of sodium (Na) has one electron in its outer shell. What is most likely to happen when sodium reacts with chlorine (Cl), which has seven electrons in its outer shell?

Accepted Answer

Sodium will transfer its electron to chlorine, forming an ionic bond.

Question 3

Which of the following best describes an isotope?

Accepted Answer

Atoms of the same element with different numbers of neutrons.

Question 4

A solution has a pH of 4. What is the concentration of hydrogen ions $$[H^+] in $$this solution?

Accepted Answer

$$[H^+] = 10$$^{-4}$$ 	ext{ M}$$

Question 5

Which property of water allows it to help maintain stable temperatures in living organisms?

Accepted Answer

High specific heat and high heat of vaporization

Question 6

What type of chemical bond is formed when two atoms share electrons equally?

Accepted Answer

Nonpolar covalent bond

Question 7

Which of the following best describes a buffer in biological systems?

Accepted Answer

A buffer is a combination of molecules that prevent sudden changes in pH by accepting or donating $$H^+$$ ions.

Question 8

If the molarity of $$OH^- in a $$solution is $$10^{-6} M$$, what is the pH of the solution?

Accepted Answer

pH = 8

Question 9

Which of the following is true about hydrogen bonds?

Accepted Answer

They are weak attractive forces between polar molecules, such as water.

Question 10

A molecule of water can dissociate into which two ions?

Accepted Answer

Hydrogen ion ($$H^+) $$and hydroxide ion ($$OH^-)$$

Question 11

Which of the following best explains why ice floats on water?

Accepted Answer

Ice is less dense than liquid water because water expands when it freezes.

Question 12

Which of the following is a correct statement about acids and bases?

Accepted Answer

An acid increases the concentration of $$H^+ in a $$solution.

Question 13

A solution has a pH of 9. Which of the following best describes this solution?

Accepted Answer

It is basic.

Question 14

Which of the following is the correct definition of molarity?

Accepted Answer

The number of moles of a substance per liter of solution.

Question 15

Which of the following best describes a polar covalent bond?

Accepted Answer

A bond in which electrons are shared unequally, resulting in partial charges.

Question 16

Which of the following is a real-life example of a mixture?

Accepted Answer

Air in the atmosphere

Question 17

If you add 1 mole of glucose ($$C_6H_{12}O_6$) to enough water to make 1 liter of solution, what is the molarity of glucose in the solution?

Accepted Answer

1 M

Question 18

Which of the following statements about electron shells is correct?

Accepted Answer

Electrons in shells farther from the nucleus have higher energy.

Question 19

Which of the following best explains why water has a high surface tension?

Accepted Answer

Hydrogen bonds between water molecules create a strong cohesive force at the surface.

Question 20

A buffer solution is prepared by mixing a weak acid and its conjugate base. What will happen if a small amount of strong acid is added to this buffer?

Accepted Answer

The buffer will neutralize the added acid, minimizing the change in pH.

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