In my lab we found OUR average molarity to be 0.83334 M, but we used 3% H2O2 (hydrogen peroxide), so I'm not sure how to do this or what numbers to even use.

7. Convert the average molarity of hydrogen peroxide into % (wt) of hydrogen peroxide (the density of the solution = 1.009g/ml).

8. Comparing the above calculated % of hydrogen peroxide with the known (labeled on the bottle) value, calculate the % experimental error.

The first four peaks in the X-ray powder diffraction pattern of sodalite are at 2 values of 9.97°, 14.12°, 17.32° and 20.02°. The radiation used for the experiment was Cu K with  = 1.5418 Å. Determine the lattice type and calculate the length, a, of the cubic unit-cell.

FeS can be roasted in O 2 to form FeO, according to the reaction 2FeS + 3O 2 2FeO + 2SO 2 If the slag (solid product) contains 80% FeO and 20% FeS , and the exit gas is 100% SO 2 , determine the extent of reaction and the initial moles of FeS. Use 100 lb as the basis. [0.557; 1.341 lb-mol]

A sample is analyzed to determine its iron content Fe2+ via a redox titration with potassium chromate as the titrant. In the titration Fe2+ is oxidized to Fe3+ and CrO4 2- is reduced to Cr 3+. What is the percent by mass of iron in the sample if 0.9087g of the sample required 45.68mL of a 0.04322 M K2CrO4 solution to reach the endpoint?

I worked out the balanced equation to be:

8H+ + 3Fe2+ + CrO4 2- = 3Fe3+ + Cr3+ + 4H2O

What is the mechanism by which solute is dissolved in non polar solvents? Explain briefly. (5 mark)

Part B What mass of carbon dioxide is produced from the complete combustion of 6.90×10−3 g of methane? Express your answer with the appropriate units.

Part C What mass of water is produced from the complete combustion of 6.90×10−3 g of methane? Express your answer with the appropriate units. Part D What mass of oxygen is needed for the complete combustion of 6.90×10−3 g of methane? Express your answer with the appropriate units   

The equilibrium constant for the reaction of fluorine gas with bromine gas at 300 K is 54.7 and the reaction is: Br2(g) + F2(g) ⇔ 2 BrF(g) What is the equilibrium concentration of fluorine if the initial concentrations of bromine and fluorine were 0.121 moles/liter in a sealed container and no product was present initially?

In each pair, indicate which substance has the stronger intermolecular forces and explain your reasoning: (a) Ne, Ar; (b) NF3, BF3; (c) SiH4, GeH4; (d) NaF, HF.

1. Calculate the dilution factor and final concentration of the following target analytes:

20 mL of target analyte (2.5 M), to a final volume of 100 mL

2 mL of target analyte (3.23 ppm), to a final volume of 0.05 L.

5 mL of target analyte (15.9032 %), to a final volume of 1 dL.

1 dL of target analyte (4.0989 M), to a final volume of 0.25 L

0.025 L of target analyte (1.8982 g / L), to 79 g of ethanol.

10 mL of target analyte (2.0902 g / L), to 66.5 g of dichloromethane.

A solution containing a mixture of metal cations was treated with dilute HCl and a precipitate formed. The solution was filtered and H2S was bubbled through the acidic solution. A precipitate again formed and was filtered off. Then, the pH was raised to about 8 and H2S was again bubbled through the solution. This time, no precipitate formed. Finally, the solution was treated with a sodium carbonate solution, which resulted in formation of a precipitate. Which metal ions were definitely present, which were definitely absent, and which may or may not have been present in the original mixture? Ag+, Zn2+, Co2+, Li+, Cu2+, Ca2+, Fe2+, Sn2+, Mg2+, Hg22+ Sb3+, Hg2+, Pb2+

1. Add the periodic trend of electronegativity to your periodic table.
2. On your periodic table underline the elements that make up the 7 diatomic molecules (from chapter 6.6) and add the periodic trends of ionization energy, atomic size, and metallic character (chapter 4.8).

Please explain...

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?

a. an indicator with Ka = 10–13

b. an indicator with Ka = 10–14

c. an indicator with Ka = 10–10

d. an indicator with Ka = 10–8

e. an indicator with Ka = 10–11

An indicator HIn has Ka = 1 × 10–8. At pH = 6.0, what is the ratio HIn/In– ?

a. 1/100

b. 10/1

c. 1/1

d. 100/1

e. none of these

balance redox reaction that occurs in acidic conditions. what are coefficients for H + & Fe3+ once reaction is balanced? write it as H+=#; Fe +3 = #

Fe2+(aq)+Mn04-(aq) -> Fe3+(aq)+Mn2+(aq)

1. Ph of H3O+ of 5.7x10^3
2. Ph of a 1.5x10^-2 m for HBr

3. ph of 3.24x10^-4 m of hypochlorous acid ka2.9x10^-8