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At 298K, 125 ml of 0.60 M potassium hydroxide KOH is added to 175 ml of 0.40 M hydrochloric acid HCl. What is the final pH?
percentage of calcium carbonate in the sampledissolving 3.00 g of an impure sample of calcium carbonate in hydrochloric
From the solubility data given, calculate the solubility products for the following compounds: a) SrF2, 7.3 x 10^-2 g/L b) Ag3PO4, 6.7 x 10^-3 g/L
Calculate the pH of a buffer solution (consisting of 30mL 1.0M NaA + 30mL 1.0M HA and a pH of 4.75) mixed with 2mL of 1.0M NaOH. (In class we got a calculated pH of 4.63 for the mixture of the buffer solution with 2mL 1.
Calculate the pH at the points in the titration of 40.00 mL of 0.425 M NH3 for the reaction below. NH3(aq) + HNO3 ? NH4+(aq) + NO3?(aq) For NH3, Kb = 1.8x10-5. Enter your answer with 2 decimal places.
When heated, ammonium carbonate decomposes as follows. NH4CO2NH2(s) ->2 NH3(g) + CO2(g) At a certain temperature the equilibrium pressure of the system is 0.318 atm. Calculate KP for the reaction.
considering the given chemical reaction and given information about the reaction asnbsp3 ag bg rarr 2 cg dl where
PCBs are transported through the environment in the vapor phase to Lake Superior. Let's assume that the flux to this lake is almost all due to rainfall, which has an average PCB concentration of 30 ng/L. The average depth of Lake Superior is 150 m..
One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 77°C. Weights are removed suddenly from the piston to give the following sequence of three pressures.
Calculate the mass of sodium chloride that will result from the addition of 25.0g of sodium hydroxide to 0.140L of 4.00M hydrochloric acid
Describe a simple and practical way to make 1.00 L of this buffer solution, assuming a 1.0 M solution of the molecular base is available and that the chloride salt of the conjugate acid is available as a solid
Calculate the equilibrium partial pressure of bromine gas. No approximations can be made because the equilibrium constant is too large. I2 (g) + Br2 (g) 2IBr (g)
A 4.50-g sample of LIL at 25.oC dissolves in 25.0 mL of water also at 25.0C. The final equilibrium temperature of the resulting solution is 60.8C. What is the enthalp of solution of LICL expressed in kilojoules per mole?
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