Questão 1
Questão
Acids are proton [blank_start]donors[blank_end]
Questão 2
Questão
Acids are [blank_start]electron pair[blank_end] acceptors
Questão 3
Questão
[blank_start]Strong[blank_end] acids completely dissociate
Questão 4
Questão
Weak acids [blank_start]partially[blank_end] dissociate to set up an equilibrium
Questão 5
Questão
More H+ ions mean a stronger acid because there are [blank_start]more protons to donate[blank_end]
Questão 6
Questão
Weaker acids dissociate less so equilibrium moves to the [blank_start]left[blank_end]
Questão 7
Questão
Strong bases completely dissociate into [blank_start]ions[blank_end] in an [blank_start]aqueous[blank_end] solution
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].
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.
Questão 10
Questão
The are two types of buffer solution, [blank_start]alkaline[blank_end] and [blank_start]acidic[blank_end].
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.
Questão 12
Questão
Buffer solutions are found in the [blank_start]stomach[blank_end] and the blood.
Questão 13
Questão
Calculate the pH of 0.1M of HCl
Questão 14
Questão
The dissociation constant for a weak acid is given the symbol ...
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.
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.
Questão 17
Questão
What is the symbol for the equilibrium constant?
Questão 18
Questão
Calculate the pH of 0.001M NaOH...
Questão 19
Questão
Kw varies with temperature
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
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
Questão 25
Questão
At what point during an acid base titration does
a concentrated acid = concentrated conjugate base
Questão 26
Questão
[blank_start]Le Chateliers[blank_end] principle may be used to predict whether or not an indicator will change colour.
Questão 27
Questão
pH + [blank_start]pOH[blank_end] = 14
Questão 28
Questão
Calculate the pH if H+ is 3x10 to the power of -4
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