Acids are proton
Acids are acceptors
acids completely dissociate
Weak acids dissociate to set up an equilibrium
More H+ ions mean a stronger acid because there are
Weaker acids dissociate less so equilibrium moves to the
Strong bases completely dissociate into in an solution
bases partially react to give ions. An equilibrium is set up when they dissolve in .
Buffer solutions are solutions which resist changes in when small quantities of or are added.
The are two types of buffer solution, and .
Buffer solutions must be made of acids and bases so that an is present. This allows ions to be removed and produced. Strong acids can't be used as they fully dissociate so can't be removed.
Buffer solutions are found in the and the blood.
Calculate the pH of 0.1M of HCl
1
2
1.9
12
The dissociation constant for a weak acid is given the symbol ...
Ksp
SpK
Ka
Kc
mol
Weaker acids dissociate less to give ions so is smaller but pKa is larger.
An acid with more is a stronger acid because the anion is more stable due to electron effect.
What is the symbol for the equilibrium constant?
Kw
Calculate the pH of 0.001M NaOH...
14
3
11
Kw varies with temperature
Find the H+ conc in 0.01moldm-3 solution of NaOH...
1x10 to the power of -12
1x10 to the power of -2
Many indicators are acids as they in solution. The removal of the ion causes a colour change.
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
What is involved in the titration of these curves?
The 3 steps in calculating the pH of a buffer solution are as follows:
1- convert Ka to using 2-place values into equation pH=pKa+ log [] / [] 3- calculate the pH
At what point during an acid base titration does a concentrated acid = concentrated conjugate base
end point
neutralisation point
half point of neutralisation
initially ( as soon as the titration begins)
principle may be used to predict whether or not an indicator will change colour.
pH + = 14
Calculate the pH if H+ is 3x10 to the power of -4
4.59
3.52
1.0007
0.999
Calculate the H+ present in a solution of pH 12.7
-1.10
1.10
5.01 x 10 to the -12
2.00 x 10 to the -13
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