Acid and Base Problems
Ka stands for what
The equilibrium expression for a acid reaction
Which of the following salts will produce a basic solution when dissolved in water: NaNO3 NH4Cl, Na2CO3 or KBr. Explain your reasoning
NaNO3 and KBr
Does anyone know what a buffer is
Tell blood example
pH=pKa+log(A/HA)
Topics I can not fit/put in due to space or jeopardy hoeing bc it trying to make me pay lmao
-Phase Diagrams (what to use on a diagonal line or straight line)
-Vapor pressure
-Unit cells
-Molarity, Molality, Mass percent, mole fraction
-Rate laws (especially from a table)
-Integrated rate laws (zero, first, second order)
Jeopardy is a money hungry and I'm not going to pay 20 bucks. Here a list from exam 2 i couldn't cover
-Nuclear chemistry
-Q and K relationship
-the three rules to use to make finding K easier.
-The nuclear Particles
-Make sure to review slides bc yall know i be missing stuff. Yall would do great in the exam :) (trust in gunna)
conjugate base of the acid H2PO4-1
HPO4-2
Predict if the solution of ammonium nitrate (NH4NO3) will be acidic, basic, or neutral. Write the hydrolysis reaction if applicable.
Acidic.
NH4+H20 <-----> NH3+H30
NO3+H20 <------>HNO3+OH (omitted since HNO3 will continue to dissociate)
Rank the Acids from weakest to strongest
HCL
HF
HBr
HI
HF<HCL<HBr<HI
Which of the following will have the highest boiling pressure and why.
- H2O
- CH3CH2CH2CH2CH3
- NH3O
H2O
2CO+O2 <------->2CO2
Determine the equilibrium shift if we add more O2. Extra points to what happens.
It shifts to the Products. More CO2 is formed.
Calculate the pOH in a solution if the concentration of hydrogen ions[H+] is 2×10-6
Rank the following 0.10 M solutions in order of increasing pH: NaF, NH4CL , KBr. Provide a brief explanation for your ranking.
NH4Cl< KBr <NaF
Rank the following acids by strength
HCLO
HCLO3
HCLO4
HCLO2
HCLO< HCLO2<HCLO3<HCLO4
What is the freezing point of an aqueous solution of .300 m K3PO4
Kf=1.86
Kb=.512
-2.232
In the equilibrium mixtures for the reactions with the following set of K values, which has the largest
concentration of product molecules?
K=1
K=1x106
K=1x10-8
K=1x10-6
K=1x106
The base dissociation constant Kb for ammonia is 1.8×10-5. Calculate the pH of a .075 M solution of ammonia.
pH=11.07
Given a solution of potassium cyanide (KCN), write the hydrolysis equilibrium equation and calculate the pH of a 0.05 M KCN solution. The Ka for hydrogen cyanide is 4.9×10-10
pH=11.004
Write the expression for Ka phosphoric acid (H3PO4) and explain why each successive ionization becomes more difficult
HPO4-2 <------->H++PO4-3
131I has a half-life of 8.04 days. Assuming you start with a 1.53 mg sample of 131I, how many mg
will remain after 13.0 days
.499 mg
Consider this reaction:
NO(g) + CO(g) <----> 1/2 N2(g) + CO2(g) ΔH -374kJ
The conditions of temperature and pressure that favor the formation of CO2
If we Increase pressure and lower temperature that would favor the products.
A 0.20 M solution of acetic acid (HC2H3O2 has a pH of 2.72. Calculate the percent ionization of the acid in this solution.
.952 ionization
A 0.10 M solution of sodium hypochlorite (NaClO) is prepared. Sodium hypochlorite is a salt formed from the weak acid hypochlorous acid (HClO) and a strong base (NaOH). The Ka of hypochlorous acid is 3.0×10-8. Determine the pOH
pOH=3.73
In the following question which molecue is acting as the lewis base
AlCl3+Cl-→[AlCl4]-
Cl-
Calculate the half-life of an isotope if a sample was reduced to 65% of its original mass in 10.0 years
(hint:read the wording of the question)
T1/2=16.09
A<------>2B. K=6.53x10-6
If initial 4.00 M sample of A at 500K what is the equilibrium concentration for B
the molecules of 2B would be 1.142x10-3