Assuming complete disassociation of electrolytes which of these aqueous solutions has the LOWEST freezing point (reminder 1 molal=1 mol kg-1) 0.15 molal KCl 0.20 molal methanol 0.40 molal methanol 0.10 molal K2O 0.10 molal KCln

Determine whether or not Hg2Br2 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part B

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Part C

Determine whether or not Mg(OH)2 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part D

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Part E

Determine whether or not CaCO3 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part F

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Part G

Determine whether or not AgI will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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A 23.33-mL solution containing 1.718 g Mg(NO₃)₂ is mixed with a 30.50-mL solution containing 1.467 g NaOH. Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive. If a species fully precipitates, type 0.

a.) ______ M Mg²⁺

b.) ______ M NO₃^-

c.) ______ M Na⁺

d.) ______ M OH^-

Use Avagadros number to calculate the number of molecules of H2S, the number of atoms of H, and the number of atoms of S, in 5.25 moles of H2S. Show all work and keep track of units and significant figures.

Why can the values of the apparant rate constant, Kapp, differ but the values of the true rate constant, k, be indentical in a reaction. An example of a reaction this can happen in is CH3COOCH3 + H20 → CH3OH + CH3COOH

What will the final temperature of 400 mL sample of water at 39.2°C be if 36,555 J of heat were added.

a.88.1°C

b.58.2°C

c.77.0°C

d.61.0°C

How much heat is produced when 6.26g of zinc metal reacts with oxygen gas under standard conditions? Use standard enthalpies of formation provided in your textbook.

a. 35.5 kj

b.267 kj

c.1021 kj

68.7 kj

Ethanol, C2H5OH, is used as a primary fuel for motor vehicles in some countries like brazil,The balanced chemical equation for the combustion reaction is

C2H5OH(l) + O2(g)-------- CO2(g) + H2O(g)

The density of the ethanol is 0.7893g/mL .Determine the enthalpy of combustion of exactly 2L of ethanol.

a. -3.31 x 10^4 kj

b.-4.68 x 104

c.-1.11 x 104 kj

d.1.69 x 10^4 kj

Determine the [OH?] of a solution that is 0.115M in CO32-.

The kb value for CO32- is 2.1e-4.

Determine the pH and pOH of a solution that is .115 M in CO32-

Phosphorous acid, H3PO3(aq), is a diprotic oxyacid that is an important compound in industry and agriculture.

pKa1 = 1.30

pKa2 = 6.70

Calculate the pH for each of the following points in the titration of 50.0 mL of a 2.7 M H3PO3(aq) with 2.7 M KOH(aq).

A) before addition of any KOH

B) after addition of 25.0 mL of KOH

C) after addition of 50.0 mL of KOH

D) after addition of 75.0 mL of KOH

E) after addition of 100.0 mL of KOH

Describe the acidity and pKa of hydrogen atoms that are bonded to carbon atoms adjacent to alkenes, as compared to hydrogen atoms bonded to tertiary alkanes. What happens to leaving groups that are found in the same adjacent position?

3. Ion exchange chromatography

a) how can the texhnique be used for qualitative and quantitative purposes

b) what are the major advantages and limitations of the technique

c) describe the nature of the signal (what is actually being detected)

What are the intermolecular forces involved with CO2?

A system contains a 0.1 molar solution of NaCl and a 0.01 M solution of NaCl separated by an oherise impermeable membrane hat contains a special sodium-conducting pore called an ionophore. The 0.1M solution is inside the membane and the 0.01 Molar solution is outsie the membrane. This ionophore allows free diffusion of the Na+ ions, but not Cl- ions. T=300K, R= 8.31 J/K/mol, F= 96500 J/mol/volt...

a) what is the total chemical potential difference, that includes concentration dependent potential and electrical potential, in Joules/mol (outside minus inside) for the sodium ions?

b) considering that chemical potential can have both a concentration dependent component and an electrical component, what is the electrical potential, in volts, of the inside of the memebrane with respect to the outside?

c) what is the chemical potential difference in Joule/mol (inside minus outside) for the chloride ions.

When a conductor e.g. metal or carbon is immersed in a electrolyte, electric double layer will be formed at the interface of the solid electrode and electrolyte. The equilibrium potential is related to the double-layer formed at the interface. Under the certain circumstance, the double-layer on the interface can disappear, the potential at which no double-layer is called “point of zero charge”. Please explain how it happens. (hint: the double layer is formed due to the difference of free energy between the electrode material and electrolyte. How to stop electron flow?)

A 10.0 mg sample of a nonvolatile organic compound is dissolved in 1.0 g of camphor, resulting in a depression of the freezing point of 1.33 K.

(You will be required to look some things up for this problem.)

Calculate the molar mass of the organic solute.

Calculate the vapor pressure of camphor over the solution.

how does titration of a strong monoprotic acid with a strong base differ from a titration for a weak monoprotic acid with a strong base with respect to the following a) quantity of base required to reach the equivalance point b) ph at the beginning of the titration c) ph at the equivalance point d) ph after addition of a slight access of base e) choice of indicator for determining the equivalence point