1) Give the formula of the conjugate base of HSO4. Give the formula for the conj
ID: 825319 • Letter: 1
Question
1) Give the formula of the conjugate base of HSO4.
Give the formula for the conjugate acid of HSO4.
2) Complete these Brønsted-Lowry reactions.
HS- + H+
HS- + OH-
3)Write the equilibrium constant expression for the reaction
A(s) + 3B(l) (arrows) 2c(aq) +D(aq)
in terms of [A], [B], [C], and [D].
K=
4) Each value below represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral.
pH=3.32, pH=12.89, pOH=1.88, pOH=11.72, (h+)=6.6 x 10^-3, (h+)=4.9 x 10^-12,
(OH-)=2.3 x 10^-13, (OH-)= 1.1 x 10^-4, (h+)=1.0 x 10^-7, pOH=7.00
5) What is the hydrogen ion concentration of a solution with pH = 4.75?
6)Determine the dissociation constants for the following acids. Express the answers in proper scientific notation where appropriate.
Acid pKa Ka
A 4.0 number= Which is the strongest acid?
A, B or C?
B 9.10 number=
C -2.0 number=
7) The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.150 M NaOH.
What volume of NaOH is needed to reach the end point of the titration?
What was the initial concentration of HCl?
8)Write the overall equation and net ionic equation for the reaction of HI (hydroiodic acid) and potassium hydroxide. Include phases (states) in your equations. Enter the formula for water as H2O.
overall equation:
reactants and products
Net ionic equation:
reactants and products
9) For the following chemical reaction
HCN(aq) + KOH(aq) (arrow going to right) H2O(l) +KCN(aq)
write the net ionic equation, including the phases.
10)Which three of the following statements accurately describe the blood buffering system in humans? The blood buffering system . . .
utilizes the acetic acid/acetate conjugate acid/base pair.
maintains the pH of blood near 7.4.
is facilitated by the enzyme carbonic anhydrase, which interconverts carbon dioxide and water to carbonic acid (ionizes into bicarbonate and H ).
utilizes the H2CO3/HCO3 conjugate acid/base pair.
depends on the ionization of H2PO4.
regulates the blood pH at 7.4 /- one pH unit.
11) Give the conjugate acid for each compound below.
Base Acid
HCO3?
SO42?.
NH3
12) Write the chemical equation for the reaction of carbonic acid (H2CO3) with water.
13) Calculate either [H3O ] or [OH
Explanation / Answer
1) H2SO4 is the conjugate acid
SO42?. is the conjugate base
2) HS- + H+ -----> H2S
HS- + OH- ------> H2O + S2-
3)
A(s) + 3B(l) <- -> 2C(aq) + D(aq)
Kc= products / reactants
Kc = [C]^2 [D] / [B]^3
[H+]= 10^-4.75=1.78 x 10^-5 M
because [H+][OH-]= Kw = 1.0 x 10^-14
[OH-]= 1.0 x 10^-14 / 1.78 x 10^-5 =5.62 x 10^-10 M
6)
7) M1 x V1 = M2 x V2
M1 x 10.0 = 0.220 x V2
V2 (volume of NaOH) = M1 x 10.0 / 0.220
M1 (initial concentration of HCl) = 0.220 x V2 / 10.0
from the above equations you need to know one unknown to solve the euations
8)
Overall Molecular equation
HI (aq) + KOH (aq) ? KI (aq) + H2O(l)
Full ionic equation
H+(aq) + I-(aq) + K+(aq) + OH-(aq) ? K+(aq) + I-(aq) + H2O(l)
Net ionic equation:
H+(aq) + OH-(aq) ? H2O(l)
9) The net ionic equation is:
H^+ (aq) + OH^- (aq) -> H2O (l)
Since the CN ion and the K ion are remaining aqueous, they are spectator ions and do not need to be included in the equation.
The H and the OH combine to for a liquid water which is a different state than (aq).
Whenever you have a reaction that has H^+(aq) and OH^-(aq) reacting to for H2O (l) that is called an acid base neutralization.
11) Give the conjugate acid for each compound below.
Base Acid
HCO3? H2CO3
SO42?. HSO4^-1
NH3 NH4+
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