Chem test review #2
Calulate the pH of a 0.05M Solution of KOH
-log(0.05)=1.30 14-1.30=12.7
Calculate the pH of 0.296M HNO3(aq)
-log(0.296)=0.529
2SO2(g) + O2(g)--->2SO3(g) Which explains what happens after the addition of oxygen gas (assume constant temperature).
2SO2(g) + O2(g)--->2SO3(g) the amount of SO3(g) increases and the value for k stays the same
Which is the strongest acid in the following? A. HClO2 B. HCLO C. HBrO D. HlO E. HOAt
A. HClO2
Which of the following species cannot act as a lewis base? A. Mg^2+ B. O^2- C. OH^- D. H2O E. H2O2
A. Mg^2+
Of the following equilibrium's, only__________ will shift to the left in response to a decrease in volume. A. H2(g) + Cl2(g)-->2HCl(g) B. 2 SO3(g)-->2 SO2(g) + O2(g) C. N2(g) + 3 H2(g)--> 2 NH3(g) D. 4 Fe (s) + 3 O2(g)-->2 Fe2O3(s) E. 2 HI (g)-->H2(g) + I2(g)
B. 2SO3(g)--->2SO2(g) + O2(g)
Determine whether the following oxides produce an acidic, basic, or neutral solution when dissolved in water. CaO SO2
Basic-CaO Acidic-SO2
Which of the following is a conjugate acid/base pair? A. HCL/OCL- B. H2SO4/SO4^2- C. NH4+/NH3 D. H3O+/OH- E. More than one
C. NH4+/NH3
Using the following Ka values, indicate the correct order of base strength. HNO2 Ka=4.0x10^-4 HF Ka=7.2x10^-4 HCN Ka=6.2x10^-10
CN->NO2->F->H2O>Cl-
AgBr(s) + 2CN-(aq)-->Ag(CN)2^-(aq) + Br(aq) The species that are acting as a Lewis acid and Lewis base, respectively are? A. AgBr and Ag(CN)2^- B. Ag(CN)2^- and Ag+ C. Ag+ and Br- D. Br- and CN- E. Ag+ and CN-
E. Ag+ and CN-
In which of the following reactions would increasing pressure at constant temperature change the concentration of reactants and products, based on Le Chateliers principle? A. N2(g) + 3H2(g)--->2NH3 (g) B. N2O4(g)--->2NO2(g) C. N2(g) + 2O2(g)--->2NOz(g) D. 2N2(g) + O2(g)--->2N2O(g) E. all of the above
E. all of the above
In which of the following reaction does the H2PO4- ion act an acid?
H2PO4- + H2O--->H3O+ + HPO4^2-
The dihydrogenphosphate ion H2PO4-, has both a conjugate acid and a conjugate base. They would be________?
H3PO4, HPO4^2-
The effect of a catalyst on an equilibrium is to___________?
Increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture
Consider the gaseous reaction CO(g) + Cl(g)--->COCL2(g) What is the expression for Kp in terms of K?
K/(RT)
Equilibrium is reached in chemical reaction when?
The rates of the forward and reverse reaction become equal
What is K for the system 2CU(s) + O2(g)--->2Cu2O(s)
[(K1)/(K2)]^1/2
Which of the following expression is the correct equilibrium constant expression for; CO2(g) + 2H2(g)---->CH3OH(g)
[CH3 OH] -------------- [CO2] [H2]^2
The expression of the Keq for the following reaction will not include__________________? A(g)+B(g)--->C(l)+D(g)
[C]
Which of the following is the equilibrium constant expression for the dissociation of the weak acid HOCl?
[H+][OCL-] ------------ [HOCl]
Consider the following equilibrium; H2(g) + I2(s)--->2HI(g) What is the proper Keq expression?
[HI]^2 ------- [H2]
Solid sodium carbonate (Na2CO3) is?
basic
H2CO3
carbonic acid, weak
2A(g)--->2B(g) + C(g) At a particular temperature, k=1.6x10^4 Addition of chemical B to an equilibrium mixture of the above will _______________?
cause [A] to increase
Raising the pressure by lowering the volume of the container will?
cause [A] to increase
What will change the equilibrium constant?
changing temperature
HCLO3
chloric acid, strong
HCLO2
chlorous acid, weak
Consider the following equilibrium; 2CO2(g)--->2CO(g)+O2(g) DeltaH*=-515KJ Le Chatelier's principle predicts that an increase in temperature will________________?
decrease the value of the equilibrium constant
A(g) + B(g)-->C(g) + D(g) You have gases A,B,C & D at equilibrium. Upon adding gas A, the value of k what happens?
does not change, as long as the temperature is constant
The pH of a 1.0M sodium acetate solution is?
greater than 7.0
HBR
hydrobromic acid, strong
HCL
hydrochloric acid, strong
HF
hydrofluoric acid, weak
HI
hydroiodic acid, strong
H2S
hydrosulfuric acid, weak
HCLO
hypochlorous acid, weak
The reaction is exothermic: 2SO2(g)+O2(g)--->2SO3(g) Le Chateliers principle predicts that_____________ will result in an increase in the number of moles of SO3(g) in the raction container. (3p)
increasing the amount of SO2
If the concentration of the product were to double, what would happen to the equilibrium constant?
it would change its value
HNO3
nitric acid, strong
A solution in which the POH is 12.6 would be described as?
pH=14-12.6=1.4 Very acidic
Calculate the [H^+] in a solution that has a pH of 2.13
pH=2.13 10^-2.13=7.41x10^-3
HCLO4
perchloric acid, strong
H3PO4
phosphoric acid, weak
The equilibruim constant for the gas phase reaction; N2(g) + 3H2(g)--->2NH3(g) Keq=4.34x10^-3 at 300*c At equilibrium____________________?
reactants predominate
H2SO4
sulfuric acid, strong
At equilibrium_______________?
the rates of the forward and reverse reactions are equal
How do equilibrium concentration of the reactants compare to the equilibrium concentration of the product?
they are much smaller
