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1) The titration of 0.50 M NH3 with 0.50 M HCL results in a final endpoint and a concentration of 0.25 M NH4 Cl with essentially all the NH3 complete conversion to NH4^+ . The Kb of NH3 is 1.8 x10^-5, and the Kw is 1x10^-14.
Use the Ka of NH4 to estimate the pH at the endpoint of this titration.
What volume of .250 M calcium chloride would be required to precipitate silver chloride if it is mixed with 600.0 ml of 0.650 M Silver nitrate.
Which of the following compounds is expected to have the highest boiling point? octane, 2,3-dimethylhexane, 2,2,3,3-tetramethylbutane
Explain briefly that how HCl could test for limestone's presence , use the balanced chemical equation for this and then describe specific reaction that takes place?
In combustion studies of the use of H2 as an alternative fuel, HO is sometimes formed in flames by the reaction, H(g) + 1/2 O2(g) HO(g) Use the data below to calculate the value of Kc
corrosion technologist pipetted a 100.00 mL hard water sample and titrated it with 37.64 mL of 0.01 M EDTA solution for a total hardness endpoint
How many mL of 0.380 M solution can be prepared by dissolving 4.00g of Ca(OH)2 in water?
Calculate Ka and Original Concentration of Weak Base, You have a solution of a weak base, the pH of which is 10.7532. If 10.000 mL of this solution will neutralize 6.655 mL of 0.07667
a sample of gas occupoes 17ml at -112 degrees C. what volume does the sample occupy at 70 degrees C.
Marble (calcium carbonate) reacts with hydrochloric acid solution to form calcium chloride solution, water, and carbon dioxide.
A disinfectant solution is made by dissolving 4.50 g of hydrogen peroxide (H2O2) in 143.2 g of water. Calculate the mass percentage of hydrogen peroxide in the solution. What is the concentration of hydrogen peroxide in parts per million? What is ..
a sample of gas at 77 degreees celsius and 1.03 atm occupies a volume of 2.02L. What volume would this gas occupy at 107 degreees celcius and 0.789 atm.
What volume, in liters, of O2 at 35°C and 1.19 atm can be produced from the decomposition of 10.0 g KNO3? 2 KNO3(s) → 2 KNO2(s) + O2(g)
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