For each strong base solution, determine [H3O+], [OH−], pH, and pOH.

Part A 8.86×10⁻³ M LiOH

Part B 8.86×10⁻³ M LiOH

Part C 1.14×10⁻² M Ba(OH)2

Part D 1.14×10⁻² M Ba(OH)2

Part E 2.1×10⁻⁴ M KOH

Part F 2.1×10⁻⁴ M KOH

Part G 4.8×10⁻⁴ M Ca(OH)2

Part H 4.8×10⁻⁴ M Ca(OH)2

Cd2+ and Pb2+ ions in a polluted water sample are measured by complexation. In a first titration, 50.00 mL of water at pH 10 is titrated by 40.09 mL of 0.004870 M EDTA. In a second titration, a 75.00 mL aliquot of water is first treated with an excess of KCN to mask the cadmium in Cd(CN)4 2- before being titrated by 31.44 mL of the same EDTA solution. Calculate the concentrations of Cd2+ and Pb2+ in the polluted water sample. Cd2+ + 4 CN- <===> Cd(CN)4 Kf = 1.0 x 10^19 Cd2+ + Y4- <===> CdY2- Kf = 2.9 x 10^16 Pb2+ + Y4- <===> PbY2- Kf = 1.1 x 10^18 aY4- = 0.36

What mass of HCl gas must be added to 1.00 L of a buffer solution that contains [aceticacid]=2.0M and [acetate]=1.0M in order to produce a solution with pH = 3.73?

For each of the following strong base solutions, determine [OH−],[H3O+], pH, and pOH.

Part A

0.20 M NaOH

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

Part B

Express your answer to two decimal places. Enter your answers numerically separated by commas.

Part C

1.4×10⁻³ M Ca(OH)2

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

Part D

Express your answer to two decimal places. Enter your answers numerically separated by commas.

Incorrect; Try Again; 5 attempts remaining

Part E

4.6×10⁻⁴ M Sr(OH)2

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

Part F

Express your answer to two decimal places. Enter your answers numerically separated by commas.

Part G

8.8×10⁻⁵ M KOH

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

Part H

Express your answer to two decimal places. Enter your answers numerically separated by commas.

You are attempting a recrystallization of the world’s only sample of charliebionic acid with a small amount of an unknown impurity.   The acid is not soluble at all in water. The acid is very soluble in hot ethanol but only slightly soluble at room temperature. But as the solution cooled to room temperature, no precipitate formed. However, when the solution was cooled in an ice bath solid immediately formed. This solid was dried and the melting point measured. The melting point showed that the impurities remained.

What is the most likely reason that no crystals formed at room temperature?

Why is the charliebionic acid still impure after recrystallization?

Propose a last minute addition to this procedure that might correct this situation and form pure crystals at room temperature from this sample.

A 1000.-mL solution of hydrochloric acid has a pH of 1.6. Calculate the mass (g) of HCl dissolved in the solution.

1:

A piece of solid magnesium is reacted with hydrochloric acid to form hydrogen gas:

Mg_(s) + 2 HCl_(aq) à MgCl_2(aq) + H_2(g)

What volume of hydrogen gas (in mL) is collected over water at 25 °C by reaction of 0.450 g of Mg (AW = 24.3 g/mol) with 5.00 mL of 1.0 M HCl? The barometer records an atmospheric pressure of 762 torr and the vapor pressure of water at this temperature is 23.35 torr.

2:

Given the following balanced chemical reactions and their enthalpies, calculate the enthalpy of reaction for 2C(s) + H₂(g) ---> C₂H₂(g):

3:

A 10.00 mL aliquot of 0.100 M NaOH is added to 15.00 mL of 0.100 M HCl (don't try this at home, since acids and bases react violently to produce water and heat!) in a coffee cup calorimeter. The initial temperature of the two dilute liquids were both 25.0 ºC and the final temperature of the mixture was found to be     37.8 ºC. What is the (molar) heat of reaction for the neutralization?

4:

The heat of vaporization for toluene is 38.06 kJ/mol and the normal boiling point is 111 ºC. Using the Clausius-Clapeyron equation, calculate the vapor pressure of toluene at room temperature (25 ºC).

5:

What is the equilibrium constant for a weak acid HA that dissociates 1% at an initial concentration of 0.05 M according to the following balanced chemical equation?

HA_(aq) ↔ H⁺_(aq) + A^-_(aq)

Compounds A and B have the following vapor pressures:

150oF: PA=600mmHg PB=500mmHg

200oF: PA=1000mmHgPB=950mmHg

Assume that these compounds form ideal solution, calculate the vapor mole fraction of A and the total pressure VLE when the liquid mole fraction of A is 0.50 and the temperature 175oF.

1000 mol/min of a mixture of 90 mol% air and 10 mol% HCl enters an absorber column and is contacted with a stream of pure water entering the column at the rate 300 moles/min. 90% of HCl in the feed gas is absorbed by water. The two exit streams are gas stream (air+HCl) and liquid stream (water+HCl), respectively.

1. Draw and label a flowchart.

2. Define a basis of calculation.

3. Carry out a degree of freedom analysis and determine flow rates in mole/min and compositions in mole fractions of the exit streams.

A) For the reaction: 3A(g)+2B(g)⇌C(g) Kc = 63.4 at a temperature of 377 ∘C .

Calculate the value of Kp. Express your answer numerically.

B) For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 2.91×10⁻² at a temperature of 229 ∘C .

Calculate the value of Kc. Express your answer numerically.

C) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) K = 0.155 at 1774 ∘C .

What is Kp for the reaction at this temperature? Express your answer numerically.

D) For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp = 4.40×10⁻³ at 271 ∘C .

What is K for the reaction at this temperature? Enter your answer numerically.

E) The following reaction was performed in a sealed vessel at 772 ∘C : H2(g)+I2(g)⇌2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.00M and [I2]=2.80M. The equilibrium concentration of I2 is 0.0400 M . What is the equilibrium constant, Kc, for the reaction at this temperature?

Express your answer numerically.

Thank you so much in advance!

Calculate the pH and concentration of all species of malonic acid (C3H4O4) in each of the follwing solutions.

K1=1.42*10^-3, K2=2.01*10^-6

0.100 M NaC3H3O4 solution

0.100 M Na2C3H2O4 solution

When doing Paper Chromatography,

1.What would you expect to see if the paper had been touched by fingers after developing with solvent, but before staining with ninhydrin?

2.Why does the filter paper need to be stapled so that the edges do not touch each other? What would occur if it were done incorrectly?

compared to a heavier liquid fuel like gasoline, why might ethylene be a more desirable source? (Think about thermodynamic features, such as ideality, as well as other factors such as weight, cost, storage, etc.

Calculate the pH of a 0.15 M lithium acetate (ka = 1.8 x 10 -5) .