Calculate the concentration of all species present in a 0.01 M aqueous solution of ammonia. The pKa of the ammonium ion is 9.24.

A.)Calculate [H⁺] (express the result in molar units using three significant figures and scientific notation).

B.)Calculate [OH^-] (express the result in molar units using three significant figures and scientific notation).

C.)Calculate [NH+4]  (express the result in molar units using three significant figures and scientific notation).

D.)Calculate [NH3]  (express the result in molar units using three significant figures and scientific notation).

E.)What is the pH of the solution?

Here's the measurements from my expirement.
(reaction 1)
0.502 g Cu (s)
4.0 mL HNO3
100 mL DI water

(reaction 2)
30 mL 3.0 M NAOH

(reaction 3)
nothing was added.

(reaction 4)
200 mL of DI water
15 mL of 6.0 M HCl

(reaction 5)
2.003 g Zn
10 mL 6M HCl
5 mL methanol
5 mL DI water
43.492 g mass of evaporating dish
44.549 g mass of evaporating dish with solid

Here are the reactions:
reaction 1: theoretical mass of copper (II) nitrate formed
Cu+4HNO3-->Cu(NO3)2+2NO2+2H2O

reactoin 2: theoretical mass of copper (II) hydroxide formed
Cu(NO3)2+2NaOH-->Cu(OH)2+2NaNO3

reaction 3: theoretical mass of copper (II) oxide formed
Cu(OH)2-->CuO+H2O

reaction 4: theoretical mass of copper (II) sulfate formed
CuO+H2SO4-->CuSO4+H2O

reaction 5: theoretical mass of copper formed
Zn+CuSO4-->ZnSO4+Cu

Can somebody show me how to work the first one at least, so then maybe I can figure the rest out. I just do not know where to start.

The values of specific gravity are:

Standard Sugar Solution # 1= 1.014

Standard Sugar Solution # 2= 1.028

Standard Sugar Solution # 3= 1.042

Show your calculations below.

3. Plot data points of the 3 standard sugar solutions on a graph. Include the data point for distilled water. Then draw the calibration graph. Label the x-axis & the y-axis.

Y acess: 1.05 1.04 1.03 1.02 1.01 1.00 0.99 X acess: 0 , 2, 4, 6, 8, 10, 12

4. Determine the sugar concentration for Coke & Gatorade by using your calibration graph. Indicate on the calibration graph how you determine the concentrations of each solution.

Information recorded in the lab experiment:

Part C: Specific gravity of sugar solutions:

Standard Sugar Solutions/ Mass of Sugar/ Voume of Solution/ Specific Gravity

#1 / 18.00g / 500.0mL / 1.014

#2 / 36.00g / 500.0mL / 1.028

#3 / 53.00g / 500.0mL / 1.042

Part B: Specific gravity of soft/sports drinks:

Solution / Specific Gravity

Coke / 1.049

Gatorade / 1.024

5. Using the information (Sugar content and Serving Size) on the nutrition label of each drink, determine the concentration of sugar in each drink. Show your calculations.

6.Calculate the absolute errors of measured sugar concentrations by using the values determined in the previous problem as reference values

PLEASE HELP!

In an acid-base titration experiment, 50 mL of a 0.05 M solution of acetic acid (Ka = 1.75 x 10-5 ) was titrated with a 0.05M solution of NaOH at 25 oC. The system will acquire this pH after addition of 40 mL of the titrant:

Answer: 5.36

How do you solve this?

Given 100.0 ml of a buffer that is 0.50 M in HOCl and 0.40 M in NaOCl, what is the pH after 10.0 ml of 1.0 M NaOH has been added?

(Ka for HOCl =3.5 x 10^-8)

A 10 g object at 50^oC is placed in 100 g water at 39.8^oC in a calorimeter. The temperature of the water and the object equilibrated at 40.0^oC. Identify the metal.

Please explain this. Thanks!

The objective of this experiment is to identify real world applications of quantum mechanics. Write a paper with a minimum of 1200 words discussing real world applications of quantum mechanics. Do NOT copy and paste off the internet!

A 10 g ice cube at 0^oC is melted in 100 g water initially at 20^oC. The equilibrium temperature of the mixture is 10.93^oC.

Calculate:

a) The heat lost by the water.

b) The heat gained by the melted water of the ice cube.

c) The heat absorbed by the ice to achieve melting.

Given the following reactions:

COBr₂ (g) --------------- > CO (g) + Br₂ (g)              K = .190 at 73 °C

2 BrCl (g) ------------ > Br₂ (g) + Cl₂ (g)          K = 310 at 73 °C (estimated)

Find the equilibrium constant at 73 °C for: CO + BrCl ------- > COBr₂ + Cl₂

Sulfuryl chloride,SO2Cl2,a compound with very irritating vapors, is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature it decomposes. Given: SO2Cl2 (g)  SO2 (g) + Cl2 (g) Kc = 0.0450 A sample of 6.70 g SO2Cl2 was placed in a 1.00 L container and heated to 375 oC a. Calculate the concentrations of all species after equilibrium is reached (Assume, in this case that “x” is neg. for computation purposes). Show with approximation if possible.

100 moles/hour of pure ethane at 25 degrees Celsius and 1.0 atm are burned with 50.0% excess air producing a desired product of carbon dioxide and an undesired product of carbon monoxide. The fractional conversion of the ethane is 80.0% (on a molar basis). 95% of ethane that reacts goes to carbon dioxide. Determine the molar flow rate and molar composition of the gaseous product stream, which is at 400 degrees Celsius and 1.0 atm.

Completely label your diagram, list the temperature, pressure, flow rate, and composition (mole fractions with indexes) for eac stream, supply values and units for knowns and question marks for unknowns.

Chemical Reactions:
I: __C2H6 + __O2 ---> __CO2 + __ H2O
II: __C2H6 + __O2 ---> ___CO + ___H2O

Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution:

Part A) 0.15M HF

Part B) 0.15M NaF

Part C) a mixture that is 0.15M in HF and 0.15M in NaF

A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 ∘C. The initial concentrations of Pb2+ and Cu2+ are 5.00×10−2 M and 1.50 M , respectively

What is the initial cell potential?

0.51V

What is the cell potential when the concentration of Cu2+ has fallen to 0.200 M ?

0.45V

Part C What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.360 V ?

I need help with Part C

A sample of carbonic acid (0.125 L, 0.199 M, pK_a1 = 6.35, pK_a2 = 10.33) was titrated with 1.75 M NaOH. Calculate the pH at the following points:

Before the titration.

At the 1st midpoint.

At the 1st stoichiometric (equivalence) point.

At the 2nd midpoint.

At the 2nd stoichiometric (equivalence) point.