CHM 230 Exam 3
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Last updated 1:45 PM on 3/31/23
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35 Terms
1
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How do you find Q
use inital molarities to find K
2
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If Q> K the equilibrium shifts
left
3
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If Q < K the equilibrium shifts
right
4
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If Q = K then the system is
at equilibrium
5
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What is the relationship between delta G and K
delta G= -RT \* lnK
6
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the position of K is dependent on
temperature
7
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an acid is a compound that _____ H+
donates
8
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a base is a compound that _____ H+
accepts
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ph=
\-log\[H3O+\]
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\[H30+\]=
10^-pH
11
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What is the equation for the autodissociation of water?
2H20-→ H3O+ + OH-
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kw = (number)
1x 10^-14
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kw = (expression)
\[H30+\] x \[OH-\]
14
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what = 14
pH + pOH
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ability to donate H+ is dictated by
Ka
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What are the 7 strong acids
HCl, HBr, HI , HNO3, H2SO4, HCLO3, HCLO4
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by definition a strong acid has ( )= ( )
\[HA\]=\[H3O+\]
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What is the acid dissociation expression
HA (aq) + H20 (l) -→ H30+ (aq) + A- (aq)
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Weak acids have a Ka
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higher Ka =
stronger acid
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When do you not need to solve a quadratic
\-when x to intial M is less than 5%
\-or when intial M: K is > 1000
\-or when intial M: K is > 1000
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When does the assumption fail
\-when Ka gets close to 1
\-when HA gets small
\-when HA gets small
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% ionization=
amount H30+/ M\[HA\]
24
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What is the conjugate base of hydocyanic acid, HCN
CN-1
25
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What is the conjugate acid of hydrogen sulfate anion HSO4-1
H2SO4
26
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Which of these weak acids is the strongest?
\-propanic acid Ka= 1.4 x 10^-5
\-phenol Ka= 1.3 x 10 ^-7
\-benzoic acid Ka= 6.8 x 10^-5
\-ammonium cation, Ka= 5.6 x 10^-10
\-propanic acid Ka= 1.4 x 10^-5
\-phenol Ka= 1.3 x 10 ^-7
\-benzoic acid Ka= 6.8 x 10^-5
\-ammonium cation, Ka= 5.6 x 10^-10
benzoic acid
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Which acid is the strongest
\-HCLO4
\-HNO3
\-HCLO2
\-HBrO3
\-HCLO4
\-HNO3
\-HCLO2
\-HBrO3
HClO4
28
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Which of these ionic compounds will create a neutral solution when dissolved in water?
\-ammonium nitrate
\-sodium perchlorate
\-sodium carbonate
\-iron (II) chloride
\-ammonium nitrate
\-sodium perchlorate
\-sodium carbonate
\-iron (II) chloride
sodium perchlorate
29
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Which of these ionic compounds will create a BASIC solution when dissolved in water?
\--ammonium nitrate
\-sodium perchlorate
\-sodium carbonate
\-iron (II) chloride
\--ammonium nitrate
\-sodium perchlorate
\-sodium carbonate
\-iron (II) chloride
sodium carbonate
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Which of these could you add to solution of HCN to make a buffer?
\-potassium nitrate
\-lithium cyanide
\-water
\-sulfuric acid
\-potassium nitrate
\-lithium cyanide
\-water
\-sulfuric acid
lithium cyanide
31
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Suppose you need to make a buffer with a pH= 8.50
Which of these systems would be the best choice?
\-pyruvic acid/pyruvate pka= 2.55
\-acetic acid/acetate pka=4.74
\-phenol/phenolate pka= 9.89
\-boric acid/borate pka= 9.27
\
Which of these systems would be the best choice?
\-pyruvic acid/pyruvate pka= 2.55
\-acetic acid/acetate pka=4.74
\-phenol/phenolate pka= 9.89
\-boric acid/borate pka= 9.27
\
\-boric acid/borate pka= 9.27
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The graph shows that starting at time=0 the equilibrium is moving…
to the right (toward products)
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Based on the graph what should be the coefficients for ABC
1,2,2
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Which reaction has the LARGEST value for equilibium constant K
A+D→ AD
35
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Which reaction has the SMALLEST value for equilibrium constant K
A+C-→ AC