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The student dissolved 2.570 grams of acid in 50 mL of distilled water. He then titrated the unknown acid with a standardized NaOH solution. Unfortunately, the student over shot the end point and had to back titrate the solution with 3.50 mL of 0.99897 M HCl. Once the final end point was determined, the student has added a total of 33.55 mL of a 1.0446 M NaOH solution. How many moles of OH were used to reach the end point? How many moles of H from HCl were used for back titration? How many moles of H from the solid were neutralized? What is the equivalent mass of the unknown acid?
The activation energy of a certain reaction is 45.3kJ/mol . At 24{~}^{\circ}\rm C , the rate constant is 0.0160s^{-1} . At what temperature in degrees Celsius would this reaction go twice as fast?
Determine the partial pressure and total pressure of the gases and Find the partial pressure of carbon dioxide in a gas mixture
In the commercial manufacture of nitric acid, how many liters of nitrogen dioxide will produce 30 liters of nitric oxide given that both gases are at STP? 3NO2 + H2O-> 2HNO3 +NO
how many milliliters of 0.54M HCL solution are needed to react completely with 4.6g of zinc to form zinc (II) chloride?
What mass of CCl4 will be formed if 1.20 moles of methane react with 1.55 moles of chlorine?
Determine how much heat is released when 14.8 kilo grams of Ethylene forms and The Hydrogen gas is collected over H2O(water) at a temperature of twenty five degree celsius and a total pressure =762 mmHg. (The ideal gas law constant R = 0.0821L*atm/..
In a calorimeter, 100 g of ice melts at 0oC. The enthalpy of fusion of the ice is 334 J/g. How much heat was absorbed.
What is the pH when 100 mL of 0.1 M HCl is titrated with 50 mL of 0.2 M NaOH?
If 5.25mL of 0.1000 M NaOH solution is needed to just neutralize excess acid after 20.00 mL of HCl was added to 1.00 g of an antacid, how many moles of acid can the antacid counteract per gram?
A sample of nitrogen gas in a 4.4-L container at a temperature of 35°C exerts a pressure of 3.7 atm. Calculate the number of moles of gas in the sample.
Calculate the amount of heat released when 5.3 moles of steam at 100 degrees celscus turns to water at the same temperature
Given that Iron(III) oxide or ferric oxide (molar mass = 159.7 g/mol) reacts with Carbon monoxide (molar mass = 28.0 g/mol).
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