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Problem- A solution is made of 50mL of 0.01 Pb(NO3)2 and 40mL of 1M KCI. What are the equilibrium concentrations of Pb2+ and Cl- if Ksp of PbCl2= 1.6x10^-5? use an ICE table to show how it dissociates as in a common ion problem
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calculate the empirical formula for the bismuth oxide, 89.7% Bi and 10.3 O. and percent composition
0 .15m h2CO3 and 0.80 m of NaHCO3 are dissolved what is the ph of resulting solution
A gaseous reaction occurs at a constant pressure of 50atm and releases 61.5kJ of heat. Before the reaction, the volume of the system was 7.00L. After the reaction, the volume of the system was 2.60L.
a chemical engineer studying the properties of fuels placed 1.467 g of a hydrocarbon in the bomb of a calorimeter and
Consider two jars. One jar contains 100 blue spheres, and the other jar contains 25 each of red, blue, green, and yellow colors mixed together. If you were to remove 30 spheres from the jar containing the mixture (assume you get a representative d..
Consider the reaction. N2(g) + O2(g) --> 2NO(g) How many moles of NO are obtained when 0.029 mol of N2 is completely reacted
At 373 K, Keq = 2.39 for the following reaction: SO2Cl2(g) = SO2(g) + Cl2(g) In an equilibrium mixture of the three gases, the partial pressures of SO2Cl2 and SO2 are 3.31 atm and 1.59 atm, respectively.
write a detailed mechanism for the reaction of salicylic acid with acetic anhydride showing clearly the function of the catalyst, sulfuric acid.
Briefly explicate why the concentrations of HC2H3O2 and C2H3O2- ion change when you add 0.10M HCl solution to the HC2H3O2-NaC2H3O2 buffer solution. State an appropriate chemical equation showing the changes that occur.
The flask is then rinsed with 64.6 mL of distilled water and is then used to prepare a standard solution of KNO3. Compute the molar concentration of Cl- in the standard KNO3 solution if the flask is rinsed only one time with distilled water.
Problem- Part 1) What is the major organic product when (R)-3-methyl-1, 2-epoxybutane reacts with butylmagnesium bromide?
What is the pH of a buffer prepared by adding 0.809mol of the weak acid HA to 0.305mol of NaA in 2.00L of solution? the dissociation constant Ka of HA is 5.66x10^-7
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