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A 0.0678g sample of tin sulfate was dissolved in dilute HCl and treated with 10% BaCl2 solution. The BaSO4 precipitate weighed 0.0737 g. Determine the formula of this sulfate of tin.
When the gas is not flowing, the pressure is the same everywhere in the pipe. How high above the bottom of the manometer would the mercury be in the arm connected to the pipe?
What mass of NH4Cl should the student dissolve in the solution to turn it into a buffer with pH =8.77
Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed.
What is the osmotic pressure of a solution made from dissolving 85.0g of glucose in 800ml of water at 19.0 C.
What volume will 5.6 moles of Sulfur hexafluoride (SF6) gas occupy if the temperature and pressure of the gas are 128 deg C, and 9.4 atm?
Calculate the value of deta S when 1.20 mol CH3OH (l) of is vaporized at 64.7 C. The normal boiling point of methanol is 64.7 C, and its molar enthalpy of vaporization is delta H = 71.8 KJ/mol.
A liquid that has a density of 0.80 0.01g/ml and 0.80-0.01 g/ml is insoluble in cyclohexane. what is the liquid? what is the boiling point of cyclohexane at 600 mm hg?
At some temperature,a 100-L reaction vessel contains a mixture that is initially 1.00 mol CO and 2.00 mol H2. The vessel also contains a catalyst so that the following equilibrium is attained:
we used 5 different concentration levels to test the absorbtion a potato slice had (to increase its weight) then we had to make a scatter plot chart and find the isotonic point
When N2O5 (g) is heated it dissociates into N2O3 (g) and O2(g) according to the following reaction: N2O5(g) N2O3(g) + O2(g) Kc= 7.75 at a given temperature. The N2O3(g) dissociates to give N2O(g) and O2(g) according the following reaction:
The poison strychnine is a weakly basic compound with Kb = 1.8e-6. What is the pH of a 0.058M solution of strychnine
A solution is prepared by condensing 4.00L of a gas, measured at 27°C and 746mmHg pressure into 58.0g of benzene. Calculate the freezing point of this solution.
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