Calculate the solubility (in grams per 1.00×102mL of solution) of magnesium hydroxide in a solution buffered at pH = 12. Express your answer using two significant figures. I got S1 = 1.2×10^-8 which is correct but for this part i did not get it "How does this compare to the solubility of Mg(OH)2 in pure water? "Express your answer using two significant figures. please solve it i could not get the answer.

Rank each of the following compounds in decreasing order of reactivity towards Friedel-Crafts alkylation. Most reactive = 1; if a compound will not react, rank it as "non" rather than assigning a numerical value. Compound A: fluorobenzene Compound B: phenol Compound C: benzaldehyde Compound D: acetophenone

Determine the pH at the equivalence (stoichiometric) point in the titration of 41 mL of 0.25 M C6H5COOH(aq) with 0.27 M NaOH(aq). The Ka of benzoic acid is 6.5 x 10-5.

What volume, in liters, of 1.04 M KOH solution should be added to a 0.107 L solution containing 9.26 g of glutamic acid hydrochloride (Glu, FW = 183.59 g/mol; pKa1 = 2.23, pKa2 = 4.42, pKa3 = 9.95) to get to pH 10.37?

1) In H NMR spectroscopy, why is the peak for a vinyl proton, C=C-H, shifted downfield relative to that of an alkane proton, C(sp³)-H? Be sure to use the following terms in your answer: pi-electrons, induced magnetic field, and resonance.

2)  In H NMR spectroscopy, why is the peak for a -CH₂F group shifted downfield relative to that for a -CH₂Br group? Be sure to use the following terms in your answer: electronegative, deshielded, magnetic field, and frequency.

Table salt, NaCl(s), and sugar, C12H22O11(s), are accidentally mixed. A 3.50-g sample is burned, and 2.10 g of CO2(g) is produced. What was the mass percentage of the table salt in the mixture?

Calculate the expected change in temperature for 25.00 mL of 0.500 M HCl reacting with 25.00 mL of 0.500 M NaOH. The heat Capacity of the Calorimeter is 15.6 J C -1 and the molar Enthalpy of Neutralization is -55.83 kJ mole . (Remember to use -1 dimensional analysis)

Agree or disagree with the following statements. Support your answer with chemical reasoning, calculations, analogies, examples, etc.

a. Since sugar is soluble in water, the lattice energy must be greater than the hydrogen bonds holding water together.

b. The addition of salt to water raises the boiling point, lowers the freezing point, lowers the vapor pressure, and makes the water boil faster.

c. The three factors that determine how fast a chemical reaction occurs are concentration, half-life, and enthalpy

a. Write the chemical reactions whose equilibrium constants are Kb and Ka for imidazole and imidazole hydrochloride, respectively.

b. Calculate the pH of a solution prepared by mixing 1.00 g of imidazole with 1.00 g of imidazole hydrochloride and diluting to 100.0 mL. A: 7.27

c. Calculate the pH of the solution if 2.30 mL of 1.07 M HClO4 are added.

I just ned help with c please!

For the reactions shown below, we added 3.75 mL of 0.0420 M Na₂S to a test tube containing one of the two cations (Cu²⁺ or Cd²⁺) and recovered 0.0228 g of precipitate.

Cu(NO₃)₂(aq) + Na₂S(aq) → CuS(s) + 2 NaNO₃(aq)
Cd(NO₃)₂(aq) + Na₂S(aq) → CdS(s) + 2 NaNO₃(aq)

How much precipitate in moles would be recovered theoretically if the ion was Cu²⁺? (Enter an unrounded value. Use at least one more digit than given.)
mol

How much precipitate in moles would be recovered theoretically if the ion was Cd²⁺? (Enter an unrounded value. Use at least one more digit than given.)
mol

How much precipitate in grams would be recovered theoretically if the ion was Cu²⁺?


How much precipitate in grams would be recovered theoretically if the ion was Cd²⁺?


Based on the precipitate amount recovered, which of the two ions was in the unknown?

How do you know when it is acceptable to assume a heat capacity is constant and pull it outside of the integral?

In a reaction of Zn (0.53 g) & HCl what is the volume of Hydrogen gas generated? (assume atmospheric pressure)

Consider the equilibrium reaction shown below, which is first order with respect to each [A], [B], [C], and [D].

A + B = C + D with K1 for the forward reaction and K2 for the reverse reaction.

Use the following data:

For T=300K we have Keq= 9*10^-3 and K1=21.3 M^-1 sec^-1

For T=350K we have Keq= 1.6*10^-2 and K1= 3,696 M^-1 sec^-1

A) Find the activation energies for the forward and backward reaction (Eaf and Eab) and the pre-expontential factors (Af and Ab) in the Arrhenius rate expressions for k1 and k2.

B) A catalyst is added to the solution. It is found that the forward rate of the catalyzed reaction at 300 K, k1cat(300K), is equal to that for the uncatalyzed reaction (k1) at 600 K.

i) What is the equilibrium constant Keq(cat) of the catalyzed reaction at 300 K?

ii) What are the forward and backward activation energies (Ea(fc) and Ea(bc)) in the presence of the catalyst?

A single charcoal briquette has a mass of 0.1 kg, and is made up of almost entirely carbon. I want to burn that briquette in air in a sealed oven. When the combustion is complete, the gases in the oven will include CO2,O2,and N2, and the mole fraction of CO2 in this exhaust is 5%. How much air is needed (before the combustion)? Give your answer as kg, kg mole, and as a volume in m^3. For the last part, you'll use the ideal gas law. Assume that p= 1 atm, and T=400C

3,4-benzopyene (BP, C20H12) is a toxic aromatic hydrocarbon frequently found in polluted air. 5.0 liters of air (at standard temperature and pressure) is bubbled through 10 ml of dilute sulfuric acid, capturing the BP. 3.0 ml of this solution is diluted to 10 ml, and this final solution gives a fluorescence intensity of 205 (arbitrary units). A blank gave an intensity of 35 (same units). A solution containing 0.75 mg of BP per ml is prepared and 1.5 ml of the this solution is added to 3.0 ml of the initial BP solution, prior to dilution to 10 ml. This solution gives a fluorescence intensity of 294 (arbitrary units).

a) Calculate the mass of BP per liter of air.

b) Express this answer in terms of ppm and ppmv.