Equilibria

Descrição

Quiz for A Level Chemistry topic of Equilibria
Megan Thomas
Quiz por Megan Thomas, atualizado more than 1 year ago
Megan Thomas
Criado por Megan Thomas aproximadamente 7 anos atrás
11
1

Resumo de Recurso

Questão 1

Questão
Acids are proton [blank_start]donors[blank_end]
Responda
  • donors

Questão 2

Questão
Acids are [blank_start]electron pair[blank_end] acceptors
Responda
  • electron pair

Questão 3

Questão
[blank_start]Strong[blank_end] acids completely dissociate
Responda
  • Strong

Questão 4

Questão
Weak acids [blank_start]partially[blank_end] dissociate to set up an equilibrium
Responda
  • partially

Questão 5

Questão
More H+ ions mean a stronger acid because there are [blank_start]more protons to donate[blank_end]
Responda
  • more protons to donate

Questão 6

Questão
Weaker acids dissociate less so equilibrium moves to the [blank_start]left[blank_end]
Responda
  • left

Questão 7

Questão
Strong bases completely dissociate into [blank_start]ions[blank_end] in an [blank_start]aqueous[blank_end] solution
Responda
  • ions
  • aqueous

Questão 8

Questão
[blank_start]Weak[blank_end] bases partially react to give ions. An equilibrium is set up when they dissolve in [blank_start]water[blank_end].
Responda
  • water
  • Weak

Questão 9

Questão
Buffer solutions are solutions which resist changes in [blank_start]pH[blank_end] when small quantities of [blank_start]acid[blank_end] or [blank_start]alkali[blank_end] are added.
Responda
  • pH
  • acid
  • alkali

Questão 10

Questão
The are two types of buffer solution, [blank_start]alkaline[blank_end] and [blank_start]acidic[blank_end].
Responda
  • alkaline
  • acidic

Questão 11

Questão
Buffer solutions must be made of [blank_start]weak[blank_end] acids and bases so that an [blank_start]equilibrium[blank_end] is present. This allows ions to be removed and produced. Strong acids can't be used as they fully dissociate so [blank_start]H+[blank_end] can't be removed.
Responda
  • weak
  • equilibrium
  • H+

Questão 12

Questão
Buffer solutions are found in the [blank_start]stomach[blank_end] and the blood.
Responda
  • stomach

Questão 13

Questão
Calculate the pH of 0.1M of HCl
Responda
  • 1
  • 2
  • 1.9
  • 12

Questão 14

Questão
The dissociation constant for a weak acid is given the symbol ...
Responda
  • Ksp
  • SpK
  • Ka
  • Kc
  • mol

Questão 15

Questão
Weaker acids dissociate less to give [blank_start]fewer[blank_end] ions so [blank_start]Ka[blank_end] is smaller but pKa is larger.
Responda
  • fewer
  • Ka

Questão 16

Questão
An acid with more [blank_start]Cl[blank_end] is a stronger acid because the anion is more stable due to electron [blank_start]withdrawing[blank_end] effect.
Responda
  • Cl
  • withdrawing

Questão 17

Questão
What is the symbol for the equilibrium constant?
Responda
  • Kw
  • mol
  • Ka
  • Kc

Questão 18

Questão
Calculate the pH of 0.001M NaOH...
Responda
  • 14
  • 3
  • 12
  • 11

Questão 19

Questão
Kw varies with temperature
Responda
  • True
  • False

Questão 20

Questão
Find the H+ conc in 0.01moldm-3 solution of NaOH...
Responda
  • 1x10 to the power of -12
  • 1
  • 12
  • 1x10 to the power of -2

Questão 21

Questão
Many indicators are [blank_start]weak[blank_end] acids as they [blank_start]partially dissociate[blank_end] in solution. The removal of the [blank_start]H+[blank_end] ion causes a colour change.
Responda
  • weak
  • partially dissociate
  • H+

Questão 22

Questão
Indicate on the image at what point in the titration a suitable indicator would change colour: For boxes you believe to be incorrect insert - x In the box you believe to be correct write - indicator
Responda
  • x
  • indicator
  • x
  • x
  • x

Questão 23

Questão
What is involved in the titration of these curves?
Responda
  • weak acid and weak base
  • strong acid and strong base
  • strong acid and weak base
  • weak acid and strong base

Questão 24

Questão
The 3 steps in calculating the pH of a buffer solution are as follows: 1- convert Ka to [blank_start]pKa[blank_end] using [blank_start]-log[blank_end] 2-place values into equation pH=pKa+ log [[blank_start]base[blank_end]] / [[blank_start]acid[blank_end]] 3- calculate the pH
Responda
  • pKa
  • base
  • acid
  • -log

Questão 25

Questão
At what point during an acid base titration does a concentrated acid = concentrated conjugate base
Responda
  • end point
  • neutralisation point
  • half point of neutralisation
  • initially ( as soon as the titration begins)

Questão 26

Questão
[blank_start]Le Chateliers[blank_end] principle may be used to predict whether or not an indicator will change colour.
Responda
  • Le Chateliers

Questão 27

Questão
pH + [blank_start]pOH[blank_end] = 14
Responda
  • pOH

Questão 28

Questão
Calculate the pH if H+ is 3x10 to the power of -4
Responda
  • 4.59
  • 3.52
  • 1.0007
  • 0.999

Questão 29

Questão
Calculate the H+ present in a solution of pH 12.7
Responda
  • -1.10
  • 1.10
  • 5.01 x 10 to the -12
  • 2.00 x 10 to the -13

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