How to calculate unreacted concentration of A at 2hr when rate = k[A]¹[B]¹ (first order both A and B) and rate = k[A]⁰[B]⁰ (zero order both A and B) ?

A + B --> C, 1hr: A 75% reacted

The total of all carbonate species in lake water is 0.001 M, and the lake pH is 8.

Calculate the concentration of each of the individual carbonate species.

Explain in detail the experimental procedure you would use for determining the concentration of acetic acid in an aged wine sample. ( Answer in detail)

If the pH of a 2.54-cm rainfall over 3700 km2 is 3.20, how many kilograms of sulfuric acid, H2SO4, are present, assuming that it is the only acid contributing to the pH? For sulfuric acid, Ka1 is very large and Ka2 is 0.012.

Express your answer to two significant figures and include the appropriate units.

Consider the evaporation of methanol at 25.0 ?C :
CH3OH(l)?CH3OH(g) .

Why methanol spontaneously evaporates in open air at 25.0 ?C : Methanol evaporates at room temperature because there is an equilibrium between the liquid and the gas phases. The vapor pressure is moderate (143 mmHg at 25.0 degrees centigrade), so a moderate amount of methanol can remain in the gas phase, which is consistent with the free energy values.

A.) Find ?G? at 25.0 ?C .

B.) Find ?G at 25.0 ?C under the following nonstandard conditions:
(i)PCH3OH= 158.0mmHg

C). Find ?G at 25.0 ?C under the following nonstandard conditions:
(ii) PCH3OH= 110.0mmHg

D.) Find ?G at 25.0 ?C under the following nonstandard conditions:
(iii) PCH3OH= 11.0mmHg

The density of balsa wood is 18.9 pounds per cubic ft. What is the weight, in kg, of a piece of balsa wood 2.0 inches by 4.0 inches by 10.0 inches?

Revised Question: How can I obtain molarities of the final solutions with this information that I was told to record in Chem 1 Lab? It asks for a molarity of the final solution for EACH part. As in, does (AI) has its own molarity of the solution and (A2) has its own molarity if the final solution or does A1 and A2 have the same molarity of the solution? Same thing for Bl and B2.

Part: AI.

Mass of Cu(CH3COO)2•H2O: 2.495 g

Moles of Cu(CH3COO)2•H2O: 199.654 g/mol

Molarity of final solution: ???

A2.

Volume of Solution AI used: 10 mL

Molarity of final solution: ???

( I got 1.2 M from the data of Al and A2 but is that the molarity of the final solution for both Al and A2?)

*NOTE: My professor did not have us collect the direct data for a volume for Part A1. It was not in our procedures or table. But if it helps once we weighted the mass of Cu(CH3COO)2•H2O = 2.495 g, we then added 25 mL of distilled water to the 50 mL beaker to dissolve it. This is why I got confused when first calculating part A1.

Part:BI.

Molarity of stock KMnO4: 0.02011 M

Volume of stock: 20 mL

Molarity of final solution: ???

B2.

Volume of solution BI used: 10mL

Molarity of final solution: ???

(I got 0.04022 M for the molarity of the final solution from both sets of data but is that the molarity for Bl and B2?)

Part: CI.

Molarity of stock K2CrO4: 1.25 x 10^-3 M

Volume of stock solution used (V1): 7 mL

Volume of stock solution used (V2): 10 mL

Molarity of final solution: ???

( I got the molarity of the final solution = 8.75 x 10^-4 M)

A1 volume=25ml

In the determination of the solubility for copper (II) iodate, what common ion of the same concentration (for example, 0.010 M Cu2+ or 0.010 M IO3-) would have a greater effect on reducing the solubility of Cu(IO3)2? Why?

15). Classify each of these substances as an element, a compound, or a mixture.

a). A sample of “laughing gas” (dinitrogen monoxide, also called nitrous oxide)

b). Steam coming from a pan of boiling water

c). A bar deodorant soap

d). A sample of copper

e). A cup of mayonnaise

f). The helium filling a ballon

Every weak acid has the following unique characteristic(s):

a. at the 50% titration point the pH = pKa

b. the best buffering occurs +/- one pH unit of the pKa

c. the change in pH with added acid or base is the least when pH = pKa

d. the shape of the titration curve is essentially the same for all weak acids

e. all of the above

If the pH of a buffer with a pKa of 6 changes from pH 6 to 7 how does the [A-]/[HA] ratio change:

a. from 1/10 to 1/1

b. from 10/1 to 1/1

c. from 1/1 to 1/10

d. from 1/1 to 10/1

e. from 1/10 to 10/15

If the hydrogen ion concentration of a solution is 10^-5 M, what is the hydroxyl ion concentration:

a. 10^-5

b. 10^-1

c. 10^-2

d. 10^-9

e. 10^-5

What is the pH of a buffer with a pKa of 5 when the ratio of [A-]/[HA] is 10/1:

a. 3

b. 4

c. 5

d. 6

e. 7

If the pH is 8 what is the pOH:

a. 8

b. 4

c. 6

d. 12

e. 1

Which carbohydrate is converted by the human body to glucose by conversion of a carbonyl to an enol, then back to a carbonyl?

How long does it take to deposit a coating of gold 1.00 um thick on a disk-shaped medallion 4.00cm in diameter and 2.00mm thick at constant current of 86A? The density of gold 19.3 g/cm³ and the gold is from an Au(III) solution. (answer in seconds please!)

What is the pH of the titration solution when 25.0 mL of .200 M aqueous formic acid, HCO₂H, is titrated with 50.0 mL of 0.100 M aqueous potassium hydroxide, KOH? The K_a for formic acid is 1.8x10^-4.

A. 8.52

B. 7.00

C. 5.71

D. 8.29

E. 10.26

PT1. Oxygen and sulfur have similar chemical properties due to having six valence electrons.  Both form molecules with two hydrogen atoms.  Surprisingly, water (H₂O) is a liquid, yet H₂S is a gas, even though sulfur is much larger and heavier than oxygen.  Why? Explain fully.

PT2.

The ion product of water, K_w=[H⁺][OH-] = 0 x10^-14  (3 points)

1. Why is a solution at pH 7.0 said to be neutral?
2. What is the H⁺ concentration and pH of a 1mM solution of NaOH?
3. If the pH of a solution is 5.0, what is the concentration of OH^- ions?

1. To identify a diatomic gas (X2 ), a researcher carried out the following experiment: She weighed an empty 4.8-L bulb, then filled it with the gas at 1.60 atm and 29.0 ∘C and weighed it again. The difference in mass was 8.7 g . Identify the gas.

2.Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 745 mmHg and a temperature of 35 ∘C . What would the pressure be if the can were heated to 1290 ∘C ?