In a reaction of an unknown metal that follows the generic reaction (unbalanced) given below,

M(s) + HCl(aq) → MCl2 (aq) + H2 (g)

a. 0.0900 g of metal is reacted with 50.00 mL of 0.100 M HCl. Once the reaction is complete, the reaction mixture is titrated with 0.1375 M NaOH. It requires 16.35 mL of NaOH to reach the endpoint. What is the molecular weight of the metal that was reacted?

b. What is the identity of the metal that was reacted?

Compare and contrast Native -PAGE, SDS-PAGE, size-exclusion chromatography, and affinity chromatography, ion exchange chromatography. How are components separated by these procedures and how are they detected? Explain details. hHow are each of these techniques carried out?

15mL of bromobenzene to grams to moles

6mL of nitric acid to g to moles

the limiting reactant of the two/ explain

theoretical yield of product

How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 5.00? (pKa of acetic acid = 4.75)

Which solution should be mixed with 50.0 mL of 0.100M ammonia, (NH₃), to make

an effective buffer?

Select one:

a. 50.0 mL of 0.200 M HCl

b. 25.0 mL of 0.200 M HCl

c. 50.0 mL of 0.100 M HCl

d. 25.0 mL of 0.100 M HCl

A sample of solid CaCO3 is added to an empty reaction vessel, which is then sealed. After awhile, the following reaction reaches a state of dynamic equilibrium.

CaCO3(s)---------> CaO(s) + CO2(g), H = 178 kJ (per mol CO2)

Briefly explain how the equilibrium values of the mass of CaO and the pressure of CO2 are affected by the

following actions.

a) increasing the temperature
b) removing a small amount, but not all, of the CaCO3
c) transferring the equilibrium mixture to a larger reaction vessel
d) adding a small amount of LiOH(s), which reacts with CO2 to give Li2CO3(s) and H2O(l)

It is of interest to decide if an analytical separation of the metal ions can be effected by selective precipitation of carbonates from a solution that is 9.84×10-2 M in Fe2+ and 9.84×10-2 M in Ni2+. NiCO3 Ksp = 6.60×10-9 FeCO3 Ksp = 3.50×10-11 To analyze this problem, answer the following questions.

(a) What carbonate concentration is needed to precipitate 99.9% of the metal that forms the least soluble carbonate? M

(b) When 99.9% of the least soluble carbonate has precipitated, will all of the metal that forms the more soluble carbonate still remain in solution? (yes/no)

(c) What is the upper limit on the carbonate ion concentration if the more soluble compound is not to precipitate? M

(d) If the [CO32-] is at this upper limit, what percentage of the metal that forms the least soluble carbonate remains in solution? %

Describe the components of a HPLC. How would you improve the accuracyof the analysis, if necessary?

In the solution containing both 0.10 M acetic acid and 0.10 M sodium acetate, the acetic acid undergoes ionization. The chemical equation for this ionization reaction is the same as for a solution containing acetic acid alone. The difference is that the initial concentration of acetate ion (before any ionization reaction occurs) for the solution containing acetic acid alone is zero, whereas the initial concentration of acetate ion is 0.10 M in your solution containing both acetic acid and sodium acetate. Calculate the percent ionization and the expected initial pH for the solution that contained both 0.10 M acetic acid and 0.10 M sodium acetate. (Hint: Again, you will need to use Ka for acetic acid.) Percent Ionization Calculated pH

calculate the mass in grams of 7.88 mol of RbMnO4

Balance the following reaction, which occurs in basic solution.

MnO₄^-(aq) + Br^-(aq) --> MnO₂(s) + BrO₃^-(aq)

Please show your work.

Please explain all answers

1) Phenol was the first antiseptic. It has the chemical composition 76.57% C, 6.43% H, 17.00% O. The molecular weight of phenol was determined by mass spectroscopy to be 94.114 g/mol. What is the molecular formula for phenol?

2) A 3.5514 g of a chromium oxide was found to contain 2.4299 g of chromium and 1.1215 g oxygen. What is the empirical formula for this chromium oxide?

3) Phosphoric acid is produced by the reaction of calcium phosphate, Ca3(PO4)2, with sulfuric acid. How much phosphoric acid can one make from exactly one US ton (2000 lbs) of calcium phosphate?

The energy efficency ratio of a refrigerator that consumes 1800 W of electricty to remove 12,000 BTU/h of heat does not exceed 3.5. True or False?

Consider the Arrhenius equation.

K= Ae^-Ea/RT

Discuss the effect of changing the basicity of the nucleophile would have on the activation energy, and therefore on the rate constant. Describe the molecularity and rate law of the reaction. How could this be determined experimentally?

in a 1x10^-8 M solution of HNO3(aq) at 25C identify the relative molar amounts of these species from least to most

OH- , H2O , HNO3 , H3O+ , NO3-