10649548
Descripción
Test por Megan Thomas, actualizado hace más de 1 año
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Creado por Megan Thomas
hace alrededor de 7 años
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Pregunta 1
Pregunta
Acids are proton [blank_start]donors[blank_end]
Respuesta
-
donors
Pregunta 2
Pregunta
Acids are [blank_start]electron pair[blank_end] acceptors
Respuesta
-
electron pair
Pregunta 3
Pregunta
[blank_start]Strong[blank_end] acids completely dissociate
Respuesta
-
Strong
Pregunta 4
Pregunta
Weak acids [blank_start]partially[blank_end] dissociate to set up an equilibrium
Respuesta
-
partially
Pregunta 5
Pregunta
More H+ ions mean a stronger acid because there are [blank_start]more protons to donate[blank_end]
Respuesta
-
more protons to donate
Pregunta 6
Pregunta
Weaker acids dissociate less so equilibrium moves to the [blank_start]left[blank_end]
Respuesta
-
left
Pregunta 7
Pregunta
Strong bases completely dissociate into [blank_start]ions[blank_end] in an [blank_start]aqueous[blank_end] solution
Respuesta
-
ions
-
aqueous
Pregunta 8
Pregunta
[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].
Respuesta
-
water
-
Weak
Pregunta 9
Pregunta
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.
Respuesta
-
pH
-
acid
-
alkali
Pregunta 10
Pregunta
The are two types of buffer solution, [blank_start]alkaline[blank_end] and [blank_start]acidic[blank_end].
Respuesta
-
alkaline
-
acidic
Pregunta 11
Pregunta
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.
Respuesta
-
weak
-
equilibrium
-
H+
Pregunta 12
Pregunta
Buffer solutions are found in the [blank_start]stomach[blank_end] and the blood.
Respuesta
-
stomach
Pregunta 13
Pregunta
Calculate the pH of 0.1M of HCl
Respuesta
-
1
-
2
-
1.9
-
12
Pregunta 14
Pregunta
The dissociation constant for a weak acid is given the symbol ...
Respuesta
-
Ksp
-
SpK
-
Ka
-
Kc
-
mol
Pregunta 15
Pregunta
Weaker acids dissociate less to give [blank_start]fewer[blank_end] ions so [blank_start]Ka[blank_end] is smaller but pKa is larger.
Respuesta
-
fewer
-
Ka
Pregunta 16
Pregunta
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.
Respuesta
-
Cl
-
withdrawing
Pregunta 17
Pregunta
What is the symbol for the equilibrium constant?
Respuesta
-
Kw
-
mol
-
Ka
-
Kc
Pregunta 18
Pregunta
Calculate the pH of 0.001M NaOH...
Respuesta
-
14
-
3
-
12
-
11
Pregunta 19
Pregunta
Kw varies with temperature
Respuesta
- True
- False
Pregunta 20
Pregunta
Find the H+ conc in 0.01moldm-3 solution of NaOH...
Respuesta
-
1x10 to the power of -12
-
1
-
12
-
1x10 to the power of -2
Pregunta 21
Pregunta
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.
Respuesta
-
weak
-
partially dissociate
-
H+
Pregunta 22
Pregunta
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
Respuesta
-
x
-
indicator
-
x
-
x
-
x
Pregunta 23
Pregunta
What is involved in the titration of these curves?
Respuesta
-
weak acid and weak base
-
strong acid and strong base
-
strong acid and weak base
-
weak acid and strong base
Pregunta 24
Pregunta
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
Respuesta
-
pKa
-
base
-
acid
-
-log
Pregunta 25
Pregunta
At what point during an acid base titration does
a concentrated acid = concentrated conjugate base
Respuesta
-
end point
-
neutralisation point
-
half point of neutralisation
-
initially ( as soon as the titration begins)
Pregunta 26
Pregunta
[blank_start]Le Chateliers[blank_end] principle may be used to predict whether or not an indicator will change colour.
Respuesta
-
Le Chateliers
Pregunta 27
Pregunta
pH + [blank_start]pOH[blank_end] = 14
Respuesta
-
pOH
Pregunta 28
Pregunta
Calculate the pH if H+ is 3x10 to the power of -4
Respuesta
-
4.59
-
3.52
-
1.0007
-
0.999
Pregunta 29
Pregunta
Calculate the H+ present in a solution of pH 12.7
Respuesta
-
-1.10
-
1.10
-
5.01 x 10 to the -12
-
2.00 x 10 to the -13
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