chem Flashcards

Question

Fill in the blank: A _______ is a solution that can conduct electricity due to the presence of ions.

Answer 1

[electrolyte]

Answer 2

A laboratory method used to determine the concentration of a solution by reacting it with a solution of known concentration ## Footnote This process often involves the use of an indicator to visually signal the endpoint.

Answer 3

To signal the endpoint of the reaction by changing color ## Footnote Common indicators include phenolphthalein and methyl orange.

Answer 4

False ## Footnote Acids have a pH less than 7.

Answer 5

Completely dissociates into ions ## Footnote Examples of strong acids include hydrochloric acid (HCl) and sulfuric acid (H₂SO₄).

Answer 6

An acid that partially dissociates in water ## Footnote Examples include acetic acid (CH₃COOH) and citric acid.

Answer 7

The salt is formed from the cation of the base and the anion of the acid ## Footnote For example, sodium chloride (NaCl) is formed from hydrochloric acid and sodium hydroxide.

Answer 8

The point at which the reactants have completely reacted, indicated by a color change ## Footnote The endpoint is not always the same as the equivalence point.

Answer 9

False ## Footnote While many acids can be corrosive, some are safe to handle in dilute forms.

Answer 10

Produces carbon dioxide, water, and a salt ## Footnote The general reaction can be represented as: acid + carbonate → salt + CO₂ + H₂O.

Answer 11

A displacement reaction producing hydrogen gas and a salt ## Footnote For example, zinc reacting with hydrochloric acid produces zinc chloride and hydrogen gas.

Answer 12

It indicates that the amount of titrant added is stoichiometrically equivalent to the amount of substance in the sample ## Footnote This is the point at which the reaction is complete.

Answer 13

To determine the concentration of an unknown solution ## Footnote Titrations are widely used in chemistry, biology, and environmental science.

Answer 14

Metals ## Footnote Example: Hydrochloric acid + Magnesium → Magnesium chloride + Hydrogen (HCl + Mg → MgCl₂ + H₂)

Answer 15

Salt + Water ## Footnote Example: Sulfuric acid + Sodium hydroxide → Sodium sulfate + Water (H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O)

Answer 16

Salt + Water ## Footnote Example: Nitric acid + Copper(II) oxide → Copper nitrate + Water (2HNO₃ + CuO → Cu(NO₃)₂ + H₂O)

Answer 17

Salt + Water + Carbon dioxide ## Footnote Example: Hydrochloric acid + Calcium carbonate → Calcium chloride + Water + Carbon dioxide (2HCl + CaCO₃ → CaCl₂ + H₂O + CO₂)

Answer 18

Ca(OH)₂ (aq) ## Footnote Also known as limewater

Answer 19

Positively charged hydrogen ions (H+) ## Footnote The presence of H+ ions is what makes a solution acidic.

Answer 20

Negative hydroxide ions (OH–) ## Footnote The presence of the OH– ions is what makes the aqueous solution an alkali.

Answer 21

To show how acidic or alkaline a solution is ## Footnote It measures the amount of hydrogen ions present in solution.

Answer 22

An acid reacts with an alkali ## Footnote The H+ ions react with the OH– ions to produce water.

Answer 23

Water ## Footnote The reaction is represented by the net ionic equation: H+ (aq) + OH– (aq) ⟶ H2O (l).

Answer 24

No ## Footnote For example, when a metal reacts with an acid, a salt is produced but no water forms.

Answer 25

7 ## Footnote This is considered neutral on the pH scale.

Answer 26

To raise the pH ## Footnote Some crops cannot tolerate pH levels below 7.

Answer 27

* Limestone * Quicklime ## Footnote These bases help to raise the pH of the soil.

chem Flashcards

chem (54 cards)