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A 0.160-mole quantity of NiCl2 is added to a liter of 1.20 M NH3 solution. What is the concentration of Ni2 ions at equilibrium? Assume the formation constant* of Ni(NH3)62 is 5.5 × 108.
Sam was standardizing her 4mL iron solution (50 ppm concentration) , but did not exactly add 4.0 mL. Instead he added 4.50mL.
A sample of H2SO4 contains 1.11 grams of H (1.01 g/mol). How many moles of H2SO4 (98.02 g/mol) are present?
The solubility of lanthanum iodate at a certain temperature is 9.55 x 10^-4. What is the Ksp of this compound at that temperature
Consider barium hydroxide, Ba(OH)2, a white powdery substance. Student A prepares a solution of Ba(OH)2 by dissolving 4.23 g of Ba(OH)2 in enough water to make 455 ml of solution.
Calculate the pH at the equivalence point for the titration of 0.200 M methylamine (CH3NH2) with 0.200 M HCl.
not enough air is pumped into a raft to completely fill it out. the atmospheric pressure is 14.7 psi. what is the pressure of the air inside the raft?
After emptying the water and drying the flask, it was filled with ethylene glycol. it now weighed 338.72 grams. what is the specific gravity of the ethylene glycol?
calculate the freezing point depression for the solution b). calculate the molality of the solution
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide: 4HCL(aq) + MnO2(s) ----> MnCl2(aq) + 2H2O(l) + Cl2(g)
Sulfuryl chloride (SO2Cl2) in the gas phase decomposes to sulfur dioxide and chlorine gas. A) what is the rate law? B) What is the value of the rate constant (k)?
A 26.1 g sample of pure iron at 77°C is dropped into 93 g of water at 17°C. What is the final temperature of the water-iron mixture.
The density of aluminum is 2.70 g/cm3. What is the volume of one mole of aluminum?
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