Acids and Bases Quiz & Flashcards

Acids have a sour taste, whereas bases have a bitter taste and slippery feel.

A weak acid only partially dissociates, causing a slight decrease in pH.

Water autoionizes into hydronium and hydroxide ions.

Neutralization involves an acid and a base reacting to form salt and water.

The pH is 2 because the concentration of H+ ions is 0.01 M, which is 10^-2.

A [H+] concentration of 10^-7 M corresponds to a neutral pH of 7.

Acids release hydrogen ions (H+) in solution.

The conjugate base of HCl is the chloride ion (Cl-) after HCl donates a proton.

Strong bases completely dissociate in water, releasing hydroxide ions.

Sulfuric acid (H2SO4) is a common strong acid that fully dissociates in water.

NH3 acts as a base by accepting a proton from water.

Buffers help maintain a constant pH by neutralizing added acids or bases.

A pH of 3 indicates an acidic solution, as it is below 7.

Bases release hydroxide ions (OH-) in solution.

An acid reacts with a metal carbonate to form salt, water, and carbon dioxide gas.

Bases have a slippery feel and turn red litmus paper blue.

A strong acid will neutralize a weak base, forming water and a salt.

Water is amphoteric, meaning it can act as both an acid and a base.

As a solution becomes more basic, the pH increases.

0.1 M NaOH, a strong base, has a pH around 13 due to its complete dissociation.

Weak acids partially dissociate in water, unlike strong acids which fully dissociate.

Acetic acid is the main component of vinegar, giving it its sour taste.

When NH3 accepts a proton, it forms the conjugate acid NH4+.

A pH of 8 indicates a slightly basic solution, just above neutral.

Sodium bicarbonate neutralizes acids by reacting to form salt, water, and carbon dioxide.

A catalyst speeds up a reaction without being consumed, but doesn't affect the equilibrium position.

A buffer resists changes in pH, so adding a small amount of acid causes little change.

The pH is 3 because the concentration of H+ ions is 0.001 M, which is 10^-3.

Ammonia is a weak base that partially accepts protons in solution.

As pH increases, the solution becomes more basic, increasing hydroxide ion concentration.

A strong acid and a strong base neutralize each other to form a neutral solution.

The pH scale is logarithmic, with each unit representing a tenfold change in H+ concentration.

Buffers resist changes in pH, so adding a strong base causes only a slight increase in pH.

Sulfuric acid (H2SO4) can donate two protons, making it a diprotic acid.

The pOH is 4, so pH = 14 - 4 = 10, indicating a basic solution.

Carbon dioxide forms carbonic acid when dissolved in water.

Buffers are composed of a weak acid and its conjugate base to resist pH changes.

Increasing temperature decreases pH as water ionizes more at higher temperatures.

Rainwater is slightly acidic due to dissolved carbon dioxide forming carbonic acid.

Acetic acid is a weak acid, so its pH will be less than 7 but different from 0.5 M HCl.

In acidic solutions, hydrogen ions (H+) are more concentrated than hydroxide ions.

Sodium hydroxide is commonly used in soap making due to its strong basic properties.

Adding a strong acid increases hydrogen ion concentration, thus decreasing the pH.

Aluminum chloride can accept electron pairs, functioning as a Lewis acid.

Sodium hydroxide is a strong base, likely having a pH close to 14.

A lower pKa value indicates a stronger acid, as it dissociates more easily.

Ammonia reacts with water to produce OH- ions, which are responsible for its basicity.