Sodium benzoate (C6H5CO2Na) is used as a food preservative.

Part A

Calculate the pH in 0.052 M sodium benzoate; Ka for benzoic acid (C6H5CO2H) is 6.5×10−5.

Part B

Calculate the concentrations of all species present (Na+, C6H5CO−2, C6H5CO2H, H3O+ and OH−) in 0.052 M sodium benzoate.

Express your answers using two significant figures. Enter your answers numerically separated by commas.

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  Iodide ion is oxidized to hypoiodite ion, IO^- , by hypochlorite ion, ClO^-, in basic solution. The equation is

The following initial rate experiments were run and, for each, the initial rate of formation of IO^- was determined. Find the rate law and the value of the rate constant.

               Initial concentrations initial rate

please explain with steps.

In a heat of neutralization lab experiment, why do the temperatures of the acid and base must be the same? What happens if they are not the same?

Morpholine (C4H9NO) is a weak organic base with pKb=5.68.

Calculate the pH in a 1.10×10⁻²M morpholine solution.

Calculate the the concentration of C4H9NO in a 1.10×10⁻²M morpholine solution.

Calculate the the concentration of HC4H9NO+ in a 1.10×10⁻²M morpholine solution.

Calculate the concentration of H3O+ in a 1.10×10⁻²M morpholine solution.

Calculate the concentration of OH− in a 1.10×10⁻²M morpholine solution.

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(a) Derive a general expression for the energy difference between any two neighboring rotational state (i.e, the difference in energy between the L abd L+L states). (b) How does the energy difference change as L increases? (c) How does the energy difference change if the radius, r, of the rotating particle increases?

some of the hydrated salt spatter out the crucible because of a too rapid heating process. will the reported percent water in the hydrated salt be reported too high, too low, or unaffected? explain.

A typical relaxed sarcomere is about 2.3 μm in length and contracts to about 2 μm in length. Within the sarcomere, the thin filaments are about 1 μm long and the thick filaments are about 1.5 μm long.

Calculate the overlap of thick and thin filaments in the relaxed and contracted sarcomere.

what is the principle behind salt fractionation of proteins

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? %