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Calculate the pH of an aqueous solution prepared to contain 1.3 x 10^-3 M sodium nitrite (NaNO2) if the acid dissociation equilibrium constant, Ka, for nitrous acid (HNO2) is 5.1 x 10^-4.
How many moles of bromine will react with 0.0500 mole of C2H2 in the reaction C2H2 + 2 Br2 -> C2H2Br4?
Calculate the number of moles of Ascobic acid in the 50.00 ml Sample. Titration Volumes of KIO3 Initial Buret reading/ml trial 1=12.54 trial 2=8.78 Final buret reading/ trial 1=38.74 trial 2=34.93 Volume of KIO used/ml trial 1=? trial 2=?
For alloys of two hypothetical metals A and B. Find out composition of phase boundary (or solubility limit) for both and phases at this temperature.
Which of the following is a statement of Hess's Law? Answer a. If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps
A sediment sample of clay was equilibrated with ammonium ion (NH4+). The ammonium ion was then displaced with Na+. The total amount of ammonium that had been adsorbed.
how many N2 molecules can be produced after the explosion of 2.37 kg of NH4NO3? (Molar mass of NH4NO3 is 80.06 g/mol.)
At what temperature will a gas be at if you allow it to expand from an original 456 mL at 65 celcius to 3.4 L?
Explain how FeBr3 assists the reaction. Br2 dissolves in a number of solvents, but we preferentially use glacial acetic acid.
The half life of Iodine-131 is 8.0252 days. If 14.2 grams of I-131 is released in Japan and takes 31.8 days to travel across the Pacific
A 19.0 kg piece of zinc at 67 degrees Celsius is placed in a container of water. The water has a mass of 23 kg and has a temperature of 9.4 degrees Celsius before the zinc is added. What is the final temperature of the water and zinc?
If 125 calories of heat is applied to a 60.0 grams piece of copper at 21.0 degrees Celsius, what will the final temperature be? The specific heat of copper is 0.0920 calories per grams times Celsius.
Consider 20.0 moles of CO2 in a 1.0 liter container at 300.0 K. What is the pressure predicted by the van der Waals equation.
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