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What is the freezing point of a solution made by mixing 1.40 mol sodium sulfate, Na2(SO4), 1750 g H2O? (Kfp=1.86 C/m)
1.500 g of Mg(s) was combined with 125.0 mL of 1.0 M HCl. The initial temperature was 25.0oC and the final temperature was 72.3oC.
Write down the second period elements (ie. lithium through neon), on order of increasing first ionization energy and Write the electron configuration for a gallium atom.
A solution of phosphoric acid was made by dissolving 10 g of H3PO4 in 100 ml of water. The resulting volume was 104 mL. Calculate the density, mole fraction, molarity, and molality of the solution. Assume water has a density of 1.00 g/cm3
When 5.25 g of sodium oxalate is reacted with 5.25 g of calcium chloride, how many grams of sodium chloride and calcium oxalate are formed?
Determine the molarity of a solution of the weak acid HCl)2; Ka = 1.10*10^-2 if it has a ph of 1.25.
2 FeBr3(aq) + 3 Na2CO3(aq) Fe2(CO3)3(s) + 6 NaBr(aq) what is the net ionic eqation for this molecular equation.
The [OH-] = 1.3 x 10^ -6 M for a 0.025 M solution of a weak base. Calculate the value of Kb for this weak base.
Compute the equilibrium partial pressures of Carbon dioxide and CO gases. If equilibrium constant Kp for this reaction =1.52,
Calculate the amount of heat trasnferred when 3.55 g of Mg(s) reacts at constant pressure. 2Mg(s) + 02(g) ---> 2MgO(s) heat= -1204kJ
NH4CO2NH2(s)->2NH3(g) +CO2(g) (at equilibrium) starting with only the solid it is found at 40C the total gas pressure is 0.363 atm calculate equilibrium constant Kp
would a given amount of flourine react with different masses of the two hydrogen isotopes? Does this violate the law of definite proportions.
how many grams of HNO3 must be dissolved to make 25L of a solution that has a pH of 1.5
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