Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

U1&2 Chemistry > U2 AOS 1 Chapter 10 C, D & E > Flashcards

U2 AOS 1 Chapter 10 C, D & E Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

acidic solution

A

greater concentration of hydronium ions than hydroxide ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

basic solution

A

greater concentration of hydroxide ions than hydronium ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

ionic product of water definition

A

Kw, concentration of ions present in water at 25degrees celcius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

autoionisation

A

process where an atom or molecule spontaneously forms ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

neutral solution

A

equal concentration of hydroxide and hydronium ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

pH

A

concentration of hydronium ions in a solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What happens if the temp and Kw value increases?

A

The concentration of hydronium ions would increase, pH decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

ionic product (kw) of water value

A

Kw = 1.00 x 10^-14M^2 (found by multiplying [H3O+] & [OH-]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

calculating pH (formula)

A

pH=-log[H3O+] OR [H3O+] = 10^-pH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

limitations of the pH scale

A

only works for aqueous solutions

Values only valid at 25oC (298 K)

goes beyond typical range of 0 - 14

can only be readily calculated with strong acids/bases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

natural indicator

A

an indicator made from naturally sourced substances eg. litmus paper

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

ph meter

A

instrument used to measure the pH of a solution through quantitative, specific measurement of difference of electrical potential

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Why can we calculate the pH of 1.00M HCl but not 1.00M CH3COOH?

A

HCl = strong acid, CH3COOH = weak acid, only in HCl [H3O+] = [HCl], in CH3COOH, concentration of hydronium cannot be determined from this info alone as it does not completely ionise.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

meters vs indicators

A

meter: quantitative, specific and highly accuracy, reproducible - no change between measurements

indicator: qualitatitive, approximated range of values - low accuracy, if true pH is on border if colour range, pH may differ greatly between trials

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

indicator

A

a substance that changes colour to indicate pH range

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

commercial indicator

A

an artificially prepared indicator

9
Q

combustion

A

fuel reacts w/ oxygen (burning)

10
Q

calcification

A

chemical process that forms calcium carbonate (CaCO3)

11
Q

decalcification

A

chemical process that breaks down calcium carbonate

12
Q

carbonic acid definition

A

formed by reaction of CO2 with H2O

12
Q

nitric acid definition

A

formed through a series of reactions in the atmosphere between nitrogen gas, oxygen gas and water

13
Q

sulfuric acid definition

A

formed through a series of reactions in the atmosphere between sulfur, oxygen gas and water

14
Q

normal rain acidity

A

acidic (5/6) due to dissolved CO2 creating carbonic acid

15
Q

acid rain

A

rain containing nitric and sulfuric acids eg. CO2(g) + H2O (l) <-> H2CO3 (aq) <-> H+ (aq) + HCO3- (aq)

16
Q

sulfuric acid formation

A

formation of dilute sulfuric acid through sulfur (in fossil fuels) given energy through combusion

17
Q

sulfuric acid formation equation

A

2SO2(g) + O2(g) + 2H2O(l) <-> 2H2SO4(aq)

18
Q

nitric acid formation

A

through fossil fuel combustion nitrogen gas reacts to form nitrogen oxide compounds (NOx) ie nitrogen monoxide (NO) or nitrogen dioxide (NO2)

19
Q

nitric acid formation equation

A
  1. 2N2(g) + 5O2(g) + 2H2O(l) <-> 4HNO3(aq)
20
Q

effects of acid rain (other than plants)

A
  1. runoff causes lake acidification - lowers pH, harms/kills aquatic life
  2. reactions w/ weather exposed metals
  3. reactions w/ limestone (CaCO3, readily reacts) i. CaCO3(s) + H2SO4(aq) -> CaSO4(aq) + CO2(g) + H2O(l) ii. CaCO3(s) + 2HNO3(aq) -> Ca(NO3)2(aq) + CO2(g) + H2O(l)
20
Q

effects of acid rain on plants

A
  1. toxic aluminium ions are absorbed = death Al(OH)3(s) + 3H+(aq) <-> Al3+(aq) + 3H2O(l)
  2. H+ ions cause essential growth ions (Ca2+, K+, Mg2+) to be released and washed away
  3. damage to waxy layer on leaves = death
21
Q

ocean acidification

A

accelerated absorption of CO2 by oceans, H+ ions are formed, carbonic acid (H2CO3) formed, pH decreases

22
Q

effects of ocean acidification

A

CaCO3 of marine invertebrates’ exoskeletons react w/ acidity = unable to grow/shells slowly dissolve

23
Q

why can oceans change in acidity over time?

A

due to reversible nature of some chemical reactions

24
Q

carbonic acid formation equation

A

CO2(g) + H2O(l) <-> H2CO3(aq)

25
Q

What is the equation for producing Al+ which harms plants?

A

Al(OH)3(s) + 3H+(aq) <-> Al3+(aq) + 3H2O(l)

26
Q

strength vs pH

A

strength = no of ions, pH = [H3O+]

therefore, higher strength of a base generally means higher number of OH- ions and a higher pH

higher strength of an acid generally means higher number of H3O+ ions and a lower pH

U1&2 Chemistry (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions