Isis

Why was it necessary to use sodium sulfate in step 8 of the tert-butyl chloride experiment????

Why was sodium bicarbonate added to the separatory funnel in step #5 of the synthesis of tert-butyl chloride experiment?

For the reaction CO(NH2)2(aq) + H2O(l) → CO2(g) + 2NH3(g) ∆H° = +119.2 kJ and ∆S° = +354.8 J K-1. What is ∆GТ° for this reaction at 71 °C?

∆GТ° = ? kJ

When butter turns rancid, its foul odor is mostly that of butanoic acid, HC4C7O2, a weak monoprotic acid similar to acetic acid in structure. In a 0.0100 M solution of butanoic acid at 20 °C, the acid is 4.0% ionized.

Calculate the Ka of butanoic acid at this temperature.

Ka =

Calculate the pKa of butanoic acid at this temperature.

pKa =

Calculate the percentage ionization of acetic acid in solutions having concentrations of 5.0 M, 0.50 M, 0.050 M. How does the percentage ionization of a weak acid change as the acid becomes more dilute?

The percent ionization at 5.0 is %

The percent ionization at 0.50 is %

The percent ionization at 0.050 is %

Benzoic acid, HC6H5CO2, is a monoprotic acid (only one H+ ionizes) with a Ka = 6.5 × 10-5. Calculate [H+] and the pH of a 0.13 M solution of benzoic acid.

[H3O+] = ? M

pH = ?

What is the pH of a solution when 27.0 g of methylammonium chloride, CH3NH3Cl, is dissolved in enough water to make 496.4 mL of solution?

Kb = 4.3 × 10–4.

pH = ?

Salicylic acid reacts with acetic acid to form aspirin, acetyl salicylic acid. A 0.294 molar solution of salicylic acid has a pH of 1.74. Calculate the Ka and pKa of salicylic acid.

Ka =

pKa =

Given that HSO4- is a stronger acid than HPO42-, what is the chemical reaction if solutions containing these ions are mixed together? Include states in your answer.

What is the formula of the conjugate acid of dimethylamine, (CH3)2NH?

What is the formula of its conjugate base?

Kc = [conc of NO]^2 / {[conc of O2] * [conc of O2]) You get this from the reaction equation. The NO is squared because there are two molecules of NO created for each molecule of O2 and N2 that react.

Let's say x is the final conc of NO. From the equation, you know if x of NO is formed 1/2 * x of O2 and N2 must have reacted (1 mole of O2 + 1 mole of N2 = 2 moles NO)

4.8 * 10^-31 = x^2 / {[0.033 - 1/2 * x] * [0.01 - 1/2 * x]}

Solve for x, it's going to be a small number because the Kc is very small.

At 2000 ºC, the decomposition of CO2,

2CO2(g) ⇄ 2CO(g) + O2(g)

has Kc = 6.40 × 10-7. If a 3.00 L container holding 1.00 × 10-2 mol of CO2 is heated to 2000 ºC, what will be the partial pressure of CO (in atmospheres) at equilibrium? Enter your answer in scientific notation.

PCO = ?? × 10^?? atm

How many molecules of O2 are present at equilibrium? Enter your answer in scientific notation.

molecules of O2 = ?? × 10^?? molecules

The reaction

2NO(g) + O2(g) <—> 2NO2(g)

has KP = 9.61 × 1011 at 25 °C. Suppose a mixture of the reactants is prepared at 25 °C by transferring 0.977 g of NO and 674 mL of O2 measured at 36.3 °C and 820 torr into a 1 L vessel.

When the mixture comes to equilibrium, what will be the concentrations of each of the three gases?

[NO] =

[O2] =

[NO2] =

At 460 oC, the reaction

SO2(g) + NO2(g) ⇄ NO(g) + SO3(g)

has Kc = 85.0. Suppose 0.103 mol of SO2, 0.0566 mol of NO2, 0.0768 mol of NO, and 0.124 mol SO3 are placed in a 10.0 L container at that temperature. What will the concentrations of all the gases be when the system reaches equilibrium?

[SO2] = ? M

[NO2] = ? M

For SO2 I got .00475 and NO2 I got.00011 and it was marked wrong. Please help

What is the pH of a solution that has an OH- ion concentration of 1.3E-8 M? Put your answer to 3 significant figures.

Commercial, concentrated, hydrochloric acid has a concentration of 12 moles per liter. If the molarity of hydronium ions is assumed to also be 12 M, what is the concentration of hydroxide ions?

Assume you have 1.00 L of H2O. The density of H2O at 25C is 1.00g/mL. Show that the 'concentration of water in water' (The concentration of pure water) is ~ 55.5M

At 460 oC, the reaction

SO2(g) + NO2(g) ⇄ NO(g) + SO3(g)

has Kc = 85.0. Suppose 0.103 mol of SO2, 0.0566 mol of NO2, 0.0768 mol of NO, and 0.124 mol SO3 are placed in a 10.0 L container at that temperature. What will the concentrations of all the gases be when the system reaches equilibrium?

[SO2] = ? M

[NO2] = ? M

[NO] = ? M

At 460 oC, the reaction

SO2(g) + NO2(g) ⇄ NO(g) + SO3(g)

has Kc = 85.0. Suppose 0.103 mol of SO2, 0.0566 mol of NO2, 0.0768 mol of NO, and 0.124 mol SO3 are placed in a 10.0 L container at that temperature. What will the concentrations of all the gases be when the system reaches equilibrium?

[SO2] = ? M

[NO2] = ? M

[NO] = ? M

At 460 oC, the reaction

SO2(g) + NO2(g) ⇄ NO(g) + SO3(g)

has Kc = 85.0. Suppose 0.103 mol of SO2, 0.0566 mol of NO2, 0.0768 mol of NO, and 0.124 mol SO3 are placed in a 10.0 L container at that temperature. What will the concentrations of all the gases be when the system reaches equilibrium?

[SO2] = ? M

[NO2] = ? M

[NO] = ? M