As the concentration of both hydrochloric acid and acetic acid approach .0001 M, the pH values are converging. Why does this occur?

Mg(s)+2H2O(l)→Mg(OH)2(s)+H2(g).Calculate the number of grams of Mg needed for this reaction to release enough energy to increase the temperature of 75 mL of water from 21 ∘C to 76 ∘C. Calculate the standard enthalpy change for this reaction.

in the synthesis of propyl acetate 4ml of propanol and 4.5 ml of acetyl chloride was used what is the percent yield if a mass product of 3.04 grams ? was obtained

In a reaction bromobenzene is reacting with NO2+ cation to form C6H4NO2Br +C6H3N2O4Br +C6H2N3O6Br Determine the m/z values for bromobenzene and its potential mono-, di-, and tri-nitro derivatives.

What is the conjugate acid of each of the following bases? Write the equilibrium reactions in aqueous solution for each base.
1) Se^2-.
2) HPO₄^2-.
3) ClO3^-.
4) [Co(NH₃)₅(OH)]²⁺.
5) SeO₄^-.

Classify each of the following reactants and products as an acid or base according to the Bronstead theory:

H3PO4 + C6H5O- >><< H2PO4- + C6H5OH

Identify the group or period that contains the noble gases.

Identify the group or period that contains B, N, and F

Drag the appropriate elements to their respective bins.

• S
• Ne
• Si
• Ag
• Hg

• Metals

• Metalloids (semimetals)

• Nonmetals

The bacterium nitrobacter can oxidize nitrite to nitrate as a source of energy for growth. Write a balanced chemical reaction for the reaction of oxygen (g) with nitrite (aq) to form nitrate (aq). The heat of formation of nitrite (aq) is -104.6 kJ/mol. The free energy of formation for nitrate (aq) is -37.2 kJ/mol. The data for nitrate (aq) and O2 are in the back of your book. Use this information to determine the heat of reaction and the free energy of reaction for the conversion of nitrite to nitrate. Then determine K for this reaction and ∆S for this reaction. Finally determine the absolute entropy of nitrite (aq) based on this data.

delta G for O2 = 0

delta H for O2 = 0

delta G for NO3 = -108.74

delta H for NO3 = -205

Please explain, Im so confused!

A. What is the vapor pressure in atm of a solution at 25 oC produced by dissolving 138.4 g of dextrose (C6H12O6) in 376.4 g of water? Vapor pressure of water at 25 oC = 0.0313 atm

B. An 18.3 g of an unknown non-ionizing solute is added to 88.8 g of water. If the boiling point of the solution is 101.4, what is the molar mass of the solute?

C. How many moles of ions are present in an ideal solution that is produced by dissolving 18.1 g of Cu(NO₃)₂ in 341 g of water?

How to calculate theoritical NOx and SO2 (mg/Nm3) in gases at coal fired power plant, if known :

Coal Calorific Value = 4500 kcal/kg
Fuel consumption = 180 t/h
Excess air = 18%
Oxygen in exhaust gases = 5%
Flue Gas Temperature in exhaust gases = 135 deg C

Carbon Content = 30.110
Hydrogen Content = 3.610
Oxygen Content = 9.850
Sulfur Content = 0.330
Nitrogen Content = 0.700
Ash Content = 5.740
Moisture Content = 32.530

Thank you!

Determine the coordination number and oxidation number of the metal in each molecule: 1) [Co(en)2Cl2]SCN ; 2) Na2[PdBr6] ; 3) [Pt(en)2](ClO4)2 ; 4) [Co(NH3)4(OH2)2]Cl3.

Calculate molar solubility of ZnCO₃ in a buffer solution of pH = 7

A 1.0-L buffer solution contains 0.100 molHC2H3O2 and 0.100 molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5 Calculate the pH of the solution upon addition of 39.8 mL of 1.00 MHCl to the original buffer.

(19) Ammonium formate, NH4(HCOO), dissolves in water to give ammonium ions and formate ions. These ions then undergo an unfavorable and endothermic Brønsted acid- base reaction according to this equation:

NH4+ (aq) + HCOO– (aq) NH3 (aq) + HCOOH (aq)

Keq < 1 (at 298 K)

∆H_orxn > 0

(a) (8 pts.) Calculate Keq and ∆G_orxn (at 298 K) for equation (19).

(b) (6 pts.) Qualitatively, would one expect ∆S_orxn for equation (19) to be positive or negative? Briefly justify your answer.

(c) (10 pts.) If 1.00 mol NH4(HCOO) is dissolved in 1.00 L water at 298 K, what is the pH of the solution?

(d) (7 pts.) The solution from part (c) (1.00 mol NH4(HCOO) in 1.00 L water) can be made into an effective buffer at pH = 3.00 by the addition of either NaOH or HCl. Specify whether NaOH or HCl would be required, and whether more than 0.500 or less than 0.500 mol of the reagent would be needed.

(e) (8 pts.) Consider the solution from part (c) (1.00 mol NH4(HCOO) in 1.00 L water at 298 K). For each of the changes below, circle the effect on the concentration of NH3 (aq) at equilibrium after the change is made, and briefly give the reasoning for your choice.

NH4+ (aq) + HCOO– (aq) NH3 (aq) + HCOOH (aq)

Keq < 1 (at 298 K)

∆H_orxn > 0
(i) The temperature of the solution is increased to 340 K.

[NH3] increases [NH3] decreases [NH3] does not change

Explanation:

(ii) The volume of the solution is increased to 2.00 L by adding 1.00 L water.

[NH3] increases [NH3] decreases [NH3] does not change

Explanation:

The common laboratory solvent ethanol is often used to purify substances dissolved in it. The vapor pressure of ethanol, CH3CH2OH, is 54.68 mm Hg at 25 °C. In a laboratory experiment, students synthesized a new compound and found that when 30.10 grams of the compound was dissolved in 269.1 grams of ethanol, the vapor pressure of the solution was 53.72 mm Hg. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight of this compound? ethanol = CH3CH2OH = 46.07 g/mol. what is the molar weight?