What is the pH of a buffer solution prepared by adding 15.0 g of ammonia chloide to 5.00 L of 0.200 M ammonia? Ka of ammonium is 5.8 x 10^-10
2) What is the pH of the buffer after 90.0mL of 2.00 M HCl are added?
3) What is the pH of the buffer if 15.00 g of NaOH is added to the original buffer solution?
In: Chemistry
40.00 mL of a 0.1000 M carbonic acid (H2CO3) was titrated with 0.2000 M sodium hydroxide.
carbonic acid pka1:6.35 pka2:10.33
1.Calculate the volume of sodium hydroxide required to reach the first equivalence point.
2.Calculate the volume of sodium hydroxide required to reach the second equivalence point.
3.Write the balanced acid-base reaction and calculate the pH before the addition of sodium hydroxide.
4.Write the balanced acid-base reaction and calculate the pH after the addition of 12.00 mL of sodium hydroxide
5.Write the balanced acid-base reaction and calculate the pH after the addition of 20.00 mL of sodium hydroxide
6. Write the balanced acid-base reaction and calculate the pH after the addition of 30.00 mL of sodium hydroxide
7.Write the balanced acid-base reaction and calculate the pH after the addition of 40.00 mL of sodium hydroxide
8.Write the balanced acid-base reaction (paper only) and calculate the pH after the addition of 44.00 mL of sodium hydroxide
In: Chemistry
to a 100.0 mL volumetric flask are added 1.00 mL volumes of three solutions: .0100 M AgNO3, .205 M NaBr, and .100 M NaCN. The mixture is diluted with deionized water to the mark and shaken vigerously. What mass of AgBr would precipitate from this mixture? Hint: The Ksp of AgBr is 5.4 x 10-13 and the Kf of Ag(CN)2- is 1.0 x 10^21
In: Chemistry
For the reaction shown below, the initial concentrations for reactants and products are as follows: [A] = 0.27 M, [B] = 0.0640 M, [C] = 0.0134 M, and [D] = 1.47 M. If the equilibrium constant for the reaction is KC = 0.802, which direction does the reaction have to shift to reach equilibrium?
A + 3B ⇌ 2C + 3D
Enter 1 if it shifts left, 2 if it shifts right, or 3 if it's already at equilibrium.
In: Chemistry
A sample of carbonic acid (0.125 L, 0.199 M, pKa1 = 6.35, pKa2 = 10.33) was titrated with 1.75 M NaOH. Calculate the pH at the following points:
Before the titration.
At the 1st midpoint.
In: Chemistry
why are thermoset plastics not affected by solvents to the same extent as thermoplastics?
In: Chemistry
Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react.
PCl3(g) + Cl2(g) ⇌ PCl5(g)
The equilibrium constant for the reaction is KC = 37.8 at 110 °C. If 0.887 mol of phosphorus trichloride is added to 0.550 mol of chlorine in a 1.02-L reaction vessel at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride?
Report your answer to THREE significant figures.
In: Chemistry
500 lbm/min hydrocarbon feed is pumped into the feed point halfway to the top of a distillation tower. The tower feed point is 40.0 feet above holding tank for the hydrocarbon. The pressure in the holding tank is 25.0 psia. The pressure in the tower at the feed point is 85.0 psia. Assume the energy lost due to friction is negligible. There is no significant change in velocity. The hydrocarbon density is 55.0 lbm/ft 3 . Calculate the pump power required in hp and watts.
In: Chemistry
A mixture of gases is at equilibrium:
4 NO (g) → 2 N2O (g) + O2 (g) ∆H = -199.5 kJ
(a) Does the equilibrium shift to the left or to the right when some O2 (g) is removed from the reaction mixture?
(b) Does the equilibrium shift to the left or to the right when some NO (g) is added to the reaction mixture?
c) In which direction does the equilibrium shift as the temperature is lowered?
(d) In which direction does the equilibrium shift as pressure is applied to the system?
In: Chemistry
A volume of 13.96 mL of 0.1060 M NaOH solution was used to
titrate a 0.618 g sample of unknown containing
HC7H5O3.
What is the molecular mass of
HC7H5O3? (report answers to 4 or 5
significant figures) 1.3812×102
g/mol
What is the percent by mass of
HC7H5O3 in the unknown?
In this problem what mass of sample in grams would be needed to
deliver about 23.40 mL in the next trial?
In the second trial above, exactly 1.032 g was transferred into a
flask to be titrated. If the initial buret reading is 0.10 mL,
predict what the final buret reading be. ?
In: Chemistry
In Southern Ontario, during freezing weather CaCl2 is spread on icy highways to melt the ice. Calculate the freezing point lowering and freezing point of a solution containing 250 g of CaCl2 in 500.0 g of water.
In: Chemistry
Fe(II) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, wheich converts Fe(II) to insoluble Fe(III):
4Fe(OH)+(aq)+4OH-(aq)+O2(g)+2H2O(l) arrow 4Fe(OH)3(s)
How many grams of O2 are consumed to precipitate all of the iron in 5.0 x 101 mL of 0.065 M Fe(II)?
Please explain!
In: Chemistry
1.a.) The heat of hydrogenation of cyclohexane is -120kJ/mol. The heat of hydrogenation benzene is -208kJ/mol. Is the heat of hydrogenation of benzene more or less than you would expect
1.b.) This is the value different from the expected?
In: Chemistry
How much energy per mole is required to transfer acetic acid, a byproduct of ethanol metabolism from blood to urine. The relevant concentrations are 39.00 and 742.00 ppm respectively and you are running a fever at 39oC. State your answer in kJ/mol. (Donnan Potential Question)
EDIT: ITS ASKING FOR HOW MUCH ENERGY IN KJ/MOL IS NEEDED TO TRANSPORT ACETIC ACID FROM BLOOD TO URINE.
In: Chemistry