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When answering, include an explanation, balanced chemical equations and/or calculations where appropriate.
In a acid-base titration, 33.65mL of an 0.148M HCl solution were required to neutralize 25.00mL of a NaOH solution. What is the molarity of the NaOH solution?
toothpaste contains 0.24% by mass sodium flouride used to prevent dental cavities. One tube contains 119g of toothpaste. How many moles of NaF are in the tube?
how many grams of NO2 will be produced when 2.0 L of nitrogen at 840 mmHg and 24 C are completely reacted N2+2 O2-----2 NO2
a gas occupies a volume of 458 ml at a pressure of 1.01kpa abd temperature of 295 k. when the pressure is changed the
The solution is titrated with a solution of sodium thiosulphate, starch solution being added near the endpoint. 29.8cm^3 of thiosulphate are required. Calculate the concentration of the thiosulphate solution.
What are the maximun number of electrons when n=4; n=5, ml=1; n=5, ms=+1/2; n=3, l=2; n=2, l=1. Please show all work.
The standard molar enthalpy of formation of ClF3 is -405 kJ. 1/2 Cl2(g) + 3/2 F2(g) → ClF3(g)
An apparataus has three bulbs, a,b, and c. a has h2o, co2, and n2 with a pressure of 564 mmHg, Bulbs b and c are empty. bulb a is 25 degrees celcius, b is -70 celcius and c is -190 celcius. how many moles of h2o are in the system if the stopcock b..
The reaction CH4+2O2==CO2+2H2O is exothermic. Which of the following will drive the reaction to the right? A. a decrease in temperature B. an increase in temperature C. addition of a catalyst D. removal of CH4
The resulting solution has an osmotic pressure of 0.605 atm at 25 C. Assuming that the organic compound is a non-electrolyte, what is its molar mass
What is the molarity of a hydrochloric acid solution if 40.0 mL of HCl is required to neutralize 2.43g of calcium carbonate (MM = 100.09 g/mol). 2 HCl(aq) + CaCO3(aq) --> CaCl2(aq) + H2O(l) + CO2(g)
hydrogen has two naturally occurring isotopes normal hydrogen h with atomic mass of 1 and deuterium d with atomic mass
The concentration of commercially available concentrated nitric acid is 70.0 percent by mass, or 15.9M in 100 grams of solution, there are 1.11 mol of HNO3. Calculate the volume of 100 g of solution
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