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A 0.3500 g sample of brass is analyzed by the procedure in the above exercise. The Beer's Law constant for the copper ammonia complex is determined to be 7.50 x 10^-1 mL/mg. The absorbance of solution Y is found to be 0.115. What was the percent of copper in the brass sample?
What is the expected freezing point of an aqueous solution of 2.62 kg of nitric acid, HNO3 , in a solution with a total mass of 5.91 kg? Assume that the nitric acid is completely ionized.
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
Solve Virial equation (the virial equation expanded in 1/ Vm )are expansions in p and 1/Vm,respectively
A 100 mL buffer solution initially has 1.00 M HClO (Ka = 3.0 × 10-8) and 0.75 M NaClO. What is the new pH when this 100 mL of 0.10 M NaOH is added to the initial buffer solution?
Determine the mass of precipitate (in grams) that forms when 213.8 mL of 0.132 M CaCl2 solution is reacted with excess AgNO3 solution.
Find the intrinsic conductivity for germanium. (Assuming ni = 2.5x 1019/m3 at room temperature.)
Explain why a buffer made of equal concentrations of CH3COOH and CH3COO- does not change in pH when a small amount of NaOH (a strong base) is added to the solution. Does the NaOH dissociate into ions when it is added to the solution?
Is 1-propanol soluble in hexane? Why or why not? What is the sketched formula for ethyl methyl ester and is it an isomer of butanoic acid? If not, what is the isomer of butanoic acid?
what is the theoretical yield of zinc iodide, if a 2.0-g sample of zinc was used with 6.5 grams of iodine
Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1.
what is a good conductor at high temperature and a poor conductor at low temperature? YBa2Cu3O7 GaAs S Cu
Which metal hydroxide will precipate first? Why? Ksp Ni(OH)2 = 6.0x10-16 Ksp Ce(OH)3 = 6.0x10-22 Ksp Cu(OH)2 = 4.8x10-20
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