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Two metal objects were found. One has a mass of 35 g and a volume of 5.5 mL and the other has a mass of 52 g with a volume of 6.1 mL. Comment on whether these are made of the same materials or not, and explain your response. The density is different in each, so they are made of different materials.
solution is needed to just neutralize excess acid after 20 mL of 0.500 M HCL was added to 1.00 g of the antacid, how many moles of acid can the antacid counteract per gram?
A quantity of 7.031 g of an organic compound is dissolved in water to make 282.0 mL of solution. The solution has an osmotic pressure of 1.43 atm at 27°C.
What are the pH values if you take into account that the 8.00 mL of 0.100 M acid was first diluted with 100 mL water?
Calculate the molarity of a Ca(OH)2 solution if it takes 25.0 mL to titrate 0.650 g of KHP in a standardization titration. (KHP has one H+ and a formula weight of 204.2 g/mol.)
A buffer is to be prepared with a pH of 4.5 from 0.1M solutions of sodium acetate and acetic acid. How many mL of 0.1M NaAc would have to be added to 100mL of 0.1M HAc to make the proper buffer solution?
How do you arrange PV=nRT to give equation relating pressure to concentration and use it to modify Beer's Law to apply to gas pressure? Write a formula that relates absorbance to gas pressure.
Calculate the initial rate of the NO reduction at 1100 K if 400.00 mg of NO and 600.00 mg of H2 are confined to a 5.00 L reaction vessel.
What is the sum of the charges on alanine, aspartic acid, and lysine? Describe how you could use salt solutions that contain cations to control the interaction between the stationary phase and the amino acids
the Cu^+ and I^- ions in equilibrium at 298 K are both equal to 1.03 x 10^-6 M, what is the value of delta G for the reaction?
Calculate the volume of 1 M solution of NaOH required to neutralize 20mL of 0.1 M acetic acid solution (final pH should ;be 7.0). (pKa of Acetic acid = 4.76).
At what temperature will a solution of 8.27 g CaCl2 in 45.0 g H2O begin to freeze? Assume complete dissociation
An element has 2 naturally occurring isotopes. Isotope 1 has 120.9038 amu and a relative abundance of 57.4%, and isotope 2 has a mass of 122.9042 amu. Find the atomic mass of this element and by comparing it to the periodic table identify it.
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