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A buffer was prepared by mixing 1.00 mole of ammonia and 1.00 mole of
ammonium chloride to form an aqueous solution with a total volume of 1.00
liter. To 500 mL of this solution was added 30.0 mL of 1.00 M NaOH. What
is the pH of this solution?
What is the name of CH3-C2H5C(CH3)-CH2-CH3
The oxyanions IO2- and ClO4- are respectively called:
A canister of butane gas (C4H10, MM=58.12 g/mol) used for portable cooking is available in a store in two sizes, 750 mL and 2.0 L. The 750 mL canister contains 85 g of butane gas with a pressure of 48 atm at 28 C. How many grams of butane gas are present in the bigger canister under the same condition of pressure and temperature?
Calculate the number of liters occupied at STP of 2.5 mol of nitrogen gas.
5. A 0.400 mg initial sample of radioactive iodine–123, used to treat thyroid cancer, decreases to 0.113 mg after 24.0 hrs. Determine the half–life of iodine–123.
how mineralization and immobilization are affected in waterlogged soils.
A 150 g of ammonium chloride solution is 15.00 % by mass with a density of 1.037 g/mL. Calculate molarity and molality of a solution
- Define oxidation and reduction reactions
- Balance redox reactions using the change in oxidation number method
- Identify the reaction occurring in the different parts of the cell
- Define reduction potential, oxidation potential, and cell potential
- Calculate the standard cell potential
- Relate the value of the cell potential to the feasibility of using the cell to generate an electric current
- Describe the electrochemistry involved in some common batteries:
a. Leclanche dry cell
b. Button batteries
c. Fuel cells
d. Lead storage battery
- Apply electrochemical principles to explain corrosion Explain the electrode reactions during electrolysis Describe the reactions in some commercial electrolytic processes
How many liters of 0.55 M HCl is required to neutralize 1.10 g of sodium carbonate
(Na2CO3)? (molar mass of Na2CO3 = 105.99 g/mol)
2HCl + Na2CO3 → 2NaCl + H2CO3
