Back to marketplace

Topic 8: Acids and Bases

No description yet. This curated deck is ready for daily study.

Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

#1
Front (Question)

Bronsted-Lowry Acid

Back (Answer)

proton (h+) donor

#2
Front (Question)

Bronsted-Lowry Base

Back (Answer)

proton (h+) acceptor

#3
Front (Question)

Lewis theory Acid

Back (Answer)

electron pair acceptor

#4
Front (Question)

Lewis Base

Back (Answer)

electron pair donator

#5
Front (Question)

enthalpy of neutralization

Back (Answer)

enthalpy change when an acid and a base react together to form 1 mole of h20

#6
Front (Question)

acid + metal reaction

Back (Answer)

salt + hydrogen

#7
Front (Question)

acid + base reaction

Back (Answer)

salt + water

#8
Front (Question)

acid + carbonate reaction

Back (Answer)

salt + water + carbon dioxide

#9
Front (Question)

neutralization reaction

Back (Answer)

exothermic reaction; when an acid and a base make salt and water

#10
Front (Question)

meausuring pH methods

Back (Answer)

• using pH meter • using universal indicator • electrical conductivity • H+ concentration

#11
Front (Question)

strong acids

Back (Answer)

(weak conjugate bases; ionize and dissosiate completly in solution)

#12
Front (Question)

strong acid examples

Back (Answer)

HCl HNO3 H2SO4

#13
Front (Question)

weak acid

Back (Answer)

partial dissociation/ionization in solution strong conjugate bases

#14
Front (Question)

weak acid examples

Back (Answer)

partially ionize/dissociate • H2CO3 • H3PO4 • CH3COOH

#15
Front (Question)

pH scale

Back (Answer)

pH + pOH= 14 7 is neutral

#16
Front (Question)

pH formula

Back (Answer)

-log (H+) 10^-pH

#17
Front (Question)

monoprotic vs. diprotic

Back (Answer)

monoprotic; 1 H ion (e,g, HCL) diprotic; 2 H ions (e.g. H2SO4)

#18
Front (Question)

how to distinguish between a strong or weak acid

Back (Answer)

• electrical conductivity • rate of reaction • pH

#19
Front (Question)

causes of acid depostion

Back (Answer)

• all rain water naturally acidic due to dissolved CO2 (carbonic acid) • wet acid deposition • dry acid deposition

#20
Front (Question)

nitrogen oxides

Back (Answer)

(NOx) origins; electiral storms, decomposition, bacteria ammonification, combustion - react with water to form nitrous acid and nitric acid - nitrogen and oxygen form nitrogen oxides

#21
Front (Question)

sulfur oxides

Back (Answer)

(SOx) origins; volcanoes and fossil fuel comustions -reacts with water to form sulfiric acid reaction of s+ o process; - SO2–> SO3–> Acids

#22
Front (Question)

effects of acid deposition on matierals

Back (Answer)

corrodes/oxidizes/erosion

#23
Front (Question)

effects of acid deposition on plants

Back (Answer)

prvents growth of plants access to nutrients limited damage to plant roots blocks stomata for gas exchange

#24
Front (Question)

effects of acid deposition on water

Back (Answer)

eutrophication ocean acidity oxyggen depletion animal suffer