Acid-Base Chemistry and pH Measurement Quiz

Hydrochloric acid dissociates completely in water.

A neutral solution has an equal concentration of H+ and OH- ions.

Hydrochloric acid is composed of hydrogen and chlorine atoms.

Citric acid is naturally occurring in citrus fruits and gives them a sour taste.

Acids commonly have a sour taste.

Strong bases dissociate completely in water, releasing OH- ions.

Weak acids partially dissociate in water, resulting in a pH higher than 7.

Bases often feel slippery due to their ability to react with oils and greases.

Ammonia partially dissociates in water, releasing OH- ions.

The pH is determined by the concentration of H+ ions, which is high in a strong acid.

Phenolphthalein changes color at the equivalence point of a titration.

A buffer solution maintains a stable pH by resisting changes in acidity or alkalinity.

Sodium hydroxide is a strong base, fully dissociating in water to produce a high concentration of OH- ions.

The high concentration of H+ ions results in a low pH.

NH3 acts as a base and NH4+ as its conjugate acid, differing by one proton.

Acetic acid is a weak acid, partially dissociating and resulting in a pH above 7.

Even at low concentration, sodium hydroxide fully dissociates, resulting in a high pH.

The high concentration of H+ ions in a strong acid solution yields a low pH.

Nitric acid is a strong acid with a high concentration of H+ ions.

Even at low concentration, strong acids like hydrochloric acid result in a low pH.

Potassium hydroxide, a strong base, produces a high concentration of OH- ions, resulting in a pH above 7.

Increasing H+ concentration lowers the pH.

A Lewis acid accepts an electron pair.

A Lewis base donates an electron pair.