Question 1

Which property of water allows it to move upward through the stem of a plant against gravity, and what molecular interaction is primarily responsible for this property?

Accepted Answer

Cohesion; hydrogen bonds between water molecules

Question 2

Water is described as a polar molecule. What does this mean in terms of its molecular structure?

Accepted Answer

The molecule has an uneven distribution of charge, with partial positive and negative ends

Question 3

Which of the following best explains why water is an excellent solvent for ionic and polar substances?

Accepted Answer

Water's polarity allows it to surround and separate ions and polar molecules

Question 4

A scientist adds a strong acid to a buffer solution. What is the expected effect on the pH, and why?

Accepted Answer

The pH will remain relatively stable because the buffer neutralizes added H$$^+$$ ions

Question 5

Which equation correctly represents the relationship between pH and hydrogen ion concentration?

Accepted Answer

$$\mathrm{pH} = -\log_{10}[\mathrm{H}^+]$$

Question 6

Why does ice float on liquid water, and what is the biological significance of this property?

Accepted Answer

Ice is less dense than liquid water due to its crystalline structure; this prevents bodies of water from freezing solid

Question 7

A solution has a pH of 4. How many times greater is the hydrogen ion concentration compared to a solution with pH 7?

Accepted Answer

1000 times greater

Question 8

Which of the following best describes a buffer solution?

Accepted Answer

A solution that resists changes in pH when small amounts of acid or base are added

Question 9

What is the main reason water has a high specific heat capacity?

Accepted Answer

Hydrogen bonds between water molecules absorb heat when they break and release heat when they form

Question 10

Which of the following statements about acids and bases is correct?

Accepted Answer

A base decreases the concentration of H$$^+$$ ions in a solution

Question 11

A beaker contains a solution with a weak acid and its conjugate base. What will happen if a small amount of strong base is added?

Accepted Answer

The weak acid will neutralize the added base, and the pH will change only slightly

Question 12

Which of the following best explains why water is considered a polar covalent molecule?

Accepted Answer

Oxygen is more electronegative than hydrogen, creating partial charges

Question 13

If a solution has a [H$$^+$$] of $$1 	imes 10$$^{-9}$$ M, what is its pH?

Accepted Answer

$$9$$

Question 14

Which of the following is an example of adhesion in water?

Accepted Answer

Water molecules forming hydrogen bonds with glass

Question 15

A solution is made by dissolving NaCl in water. Which term best describes NaCl in this context?

Accepted Answer

Solute

Question 16

Which of the following statements about hydrogen bonds in water is correct?

Accepted Answer

Hydrogen bonds form between the hydrogen atom of one water molecule and the oxygen atom of another

Question 17

A patient is suffering from acidosis (low blood pH). Which of the following would help stabilize their blood pH?

Accepted Answer

Adding a buffer solution containing a weak base and its conjugate acid

Question 18

Which of the following best describes the role of buffers in biological systems?

Accepted Answer

Buffers prevent drastic changes in pH by neutralizing added acids or bases

Question 19

Which of the following is true about strong acids and bases compared to weak acids and bases?

Accepted Answer

Strong acids and bases dissociate completely in water

Question 20

A student mixes equal volumes of a strong acid and a strong base. What is the expected pH of the resulting solution?

Accepted Answer

The pH will be neutral, around 7

Properties of Water and Acid-Base Chemistry in Biology

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