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A 340.0 mL buffer solution is 0.170 M in HF and 0.170 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? If the same volume of the buffer was 0.330 M in HF and 0.330 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00?
A coffee-cup calorimeter is calibrated by adding 1840 J of heat to the water in the calorimeter and measuring a 1.72C rise in temperature.
Prepare the molecular formula for given compounds and determine the amount of molecules present and write the molecular formula and determine how many grams of each you have
At 700 K the equilibrium constant for the reaction CCl4(g) C(s) + 2 Cl2(g) is Kp = 0.76. A flask is charged with 2.00 atm CCl4, which then reaches equilibrium at 700 K.
Urea (NH2CONH2) an important nitrogen fertilizer is produced industrially by the reaction 2NH3(g)+CO2(g)--->NH2CONH2(aq)+ H2O(l) given that ?G^degree = -13.6KJ, calculate ?Gat 298K for the following sets of conditions
How many kilograms of CO2 are produced from the complete combustion of 1.00L of gasoline assume that the gasoline has the formula C8H18.
A total of 0.155 of this subunit was dissolved in enough water to produce 2.00 of solution. At 28 the osmotic pressure produced by the solution was 0.138 . What is the molar mass of the protein?
NH4CO2NH2(s)->2NH3(g) +CO2(g) (at equilibrium) starting with only the solid it is found at 40C the total gas pressure is 0.363 atm calculate equilibrium constant Kp
A certain quantity of a gas occupies 61.3 mL at 68C. If the pressure remains constant, what would the volume of the gas be at 17C?
how many milliliter of 0.165M KMnO4 are needed to react with 108.0ml of 0.165 M oxalic acid? How many milliliter of 0.165M oxalic acid are required to react with 108ml of 0.165M KMnO4
Our quality control department is being moved to a different location and will not be able to handle any projects for a few weeks.
An expanding gas does 150.0 J of work on its surroundings at a constant pressure of 1.01 atm. If the gas initially occupied 68.0 mL, what is the final volume of the gas.
In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 mL of acid in a flask. You quickly add 23.75 mL of 0.0502 M NaOH but overshoot the end point
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