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Equilibria

Description

Quiz for A Level Chemistry topic of Equilibria
Megan Thomas
Quiz by Megan Thomas, updated more than 1 year ago
Megan Thomas
Created by Megan Thomas about 7 years ago
12
1
0

Resource summary

Question 1

Question
Acids are proton [blank_start]donors[blank_end]
Answer
  • donors

Question 2

Question
Acids are [blank_start]electron pair[blank_end] acceptors
Answer
  • electron pair

Question 3

Question
[blank_start]Strong[blank_end] acids completely dissociate
Answer
  • Strong

Question 4

Question
Weak acids [blank_start]partially[blank_end] dissociate to set up an equilibrium
Answer
  • partially

Question 5

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

Question 6

Question
Weaker acids dissociate less so equilibrium moves to the [blank_start]left[blank_end]
Answer
  • left

Question 7

Question
Strong bases completely dissociate into [blank_start]ions[blank_end] in an [blank_start]aqueous[blank_end] solution
Answer
  • ions
  • aqueous

Question 8

Question
[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].
Answer
  • water
  • Weak

Question 9

Question
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.
Answer
  • pH
  • acid
  • alkali

Question 10

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

Question 11

Question
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.
Answer
  • weak
  • equilibrium
  • H+

Question 12

Question
Buffer solutions are found in the [blank_start]stomach[blank_end] and the blood.
Answer
  • stomach

Question 13

Question
Calculate the pH of 0.1M of HCl
Answer
  • 1
  • 2
  • 1.9
  • 12

Question 14

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

Question 15

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

Question 16

Question
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.
Answer
  • Cl
  • withdrawing

Question 17

Question
What is the symbol for the equilibrium constant?
Answer
  • Kw
  • mol
  • Ka
  • Kc

Question 18

Question
Calculate the pH of 0.001M NaOH...
Answer
  • 14
  • 3
  • 12
  • 11

Question 19

Question
Kw varies with temperature
Answer
  • True
  • False

Question 20

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

Question 21

Question
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.
Answer
  • weak
  • partially dissociate
  • H+

Question 22

Question
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
Image:
Ck12 Screenshot 21 19 2 (binary/octet-stream)
Answer
  • x
  • indicator
  • x
  • x
  • x

Question 23

Question
What is involved in the titration of these curves?
Image:
Screen Shot 2017 10 04 At 11.59.47 Am (binary/octet-stream)
Answer
  • weak acid and weak base
  • strong acid and strong base
  • strong acid and weak base
  • weak acid and strong base

Question 24

Question
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
Answer
  • pKa
  • base
  • acid
  • -log

Question 25

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

Question 26

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

Question 27

Question
pH + [blank_start]pOH[blank_end] = 14
Answer
  • pOH

Question 28

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

Question 29

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