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An aqueous solution that is 15.0 percent sulfuric acid (H2SO4) by mass has a density of 1.221 g/mL. Determine the molarity of the solution.
What is the pH of a solution that is formed at 25C by combining 300 mL of 0.040 M NaOH with 400 mL
the normal boiling point for mercury is 357c. what is the boiling point at an elevation where the atmospheric pressure is 635 torr.
A buffer is made up 0.24 M propanoic acid, CH3CH2COOH, a weak monoprotic acid, and 0.17 M of sodium propanoate, CH3CH2COONa. What is the pH of the solution.
What is the osmotic pressure of a solution made from dissolving 95.0 g of glucose, C_6H_{12}O_6, in 725 mL of water at 39.0 degrees C?
A solution of ammonia and water contains 3.20×10^25 water molecules and 8.10×10^24 ammonia molecules. How many total hydrogen atoms are in this solution?
"A student titrated a 10 mL sample of a saturated solution of borax. If the titration required 23.95 mL of 0.2556 M HCL to reach the endpoint, calculate the equilibrium molar concentration of B4O5(OH)(4 in the saturated solution"
Concetrated acedic acid is a Class II combustible liquid. What is the molecular weight of acetic acid that will form 2 moles of CO2 assuming complete combustion.
Calculate the mass of Nitrogen at room temperature dissolved at room temperature in an 80 L aquarium. Assume a total pressure of 1 atm and .78 mole fraction.
Molecular and ionic equations, What would be the proper balanced molecular and net ionic equations for each of these neutralization reactions?
a 720-mL sample of water was cooled from 60 degrees celsius to 10 degrees celsius. How much heat was lost?
An 11.0 gram sample of CaCl2(s) is dissolved in 125 grams of water with both substances at 25.0°C. If the final temperature of the mixture is 39.2 °C.
At 0.0oC, if the volume of air is 2.5 mL and the pressure of the atmosphere that day is 835 mmHg, what is the number of moles of air?
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