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Calculate the pH at the points in the titration of 40.00 mL of 0.425 M NH3 for the reaction below. NH3(aq) + HNO3 ? NH4+(aq) + NO3?(aq) For NH3, Kb = 1.8x10-5. Enter your answer with 2 decimal places. Enter scientific notation as 1.23E4. (a) When 11.50 mL of 0.470 M HNO3 have been added. (b) When 65.00 mL of 0.470 M HNO3 have been added.
what is the annual cost of operation in a 70°F room if the door is opened 10 times a day with an average heat gain per opening of 200 kJ? How much would it cost to keep the inside at 35° F? Show work.
Consider that there are two sources of OH-in this procedure. Also, an excess of 3 mL will need to be added to your calculated value in order to suppress the hydrolysis of Al 3+.
A sample of propane,C3H8 , contains 18.0 moles of carbon atoms. How many total moles of atoms does the sample contain? Express the total number of moles of carbon and hydrogen numerically.
A balloon of methane gas, CH4, has a temperature of - 2.0 Degrees Celsius and contains 2.35 g of the gas. What is the temperature of the gas in kelvins
The total volume of seawater is 1.5X10^21 L. Assume that seawater contains 3.1 percent sodium chloride by mass that its density 1s 1.03 g/mL. Calculate the total mass of sodium chloride.
At 27°C, a sample of sulfur dioxide (SO2) has a volume of 30.0 mL.
A chemist prepares a solution of potassium permanganate by measuring out 33.g of potassium permanganate into a 450ml volumetric flask and filling the flask to the mark with water. Calculate the molarity
Based on the force vs atomic spacing and energy vs atomic distance curves explain why some materials have high strength and high melting temperatures
If the ph of Rainfall in Upstate New York is Found to be 4.0, and if the acidity is half due to Nitric acid (HNO3) and half due the two Hydrogen Ions released by Sulfuric acid
What mass of sucrose should be combined with 452 g of water to make a solution with an osmotic pressure of 8.90 atm at 270 K?
prepare 10 ml of solution that represents a 4 fold dilution of the stock solution
what was the mass (g) of molecular oxygen from the air that combined with the substance to produce the dense gas? B. What is the ratio of the weight of oxygen burned to the weight of the dense gas produced?
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