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1) What volume is required to prepare 250.0ml of 2.00MHCl solution from 12.0M HCl
2) Balance the following reaction and predict the number of moles of SO2 required to completely react with 3.0 moles of 0.2 SO2+O2---->SO3
The solubility of the K3[Fe(C2O4)3].3H2O product at 00C is 4.7 g per 100 g water. Given this, calculate the maximum percent yield of product for your own reactant quantities.
when NaOH is added to this solution, a white precipitate forms. Using an equation, provide the identity of the white precipitate and explain its formation.
flask and allowed to reach equilibrium at a given temperature, what is the final concentration of cl2 In the flask?
If 450 g SO2 escaped into the atmosphere and all the escaped SO2 were converted to H2SO4. How many grams of H2SO4 would be produced in the atmosphere?
Calculate the OH- of each aqueous solution with the following H3O+ A baking soda 1.1 X 10-8 M B orange juice 2.1 X 10-4
If a buffer solution is 0.260M in a weak base (Kb=5.6x10^-5) and 0.550M in its conjugate acid, what is the pH.
The dipole moment of HBr (a polar covalent molecule) is 0.784 (debye), and its percent ionic character is 11.6 . Estimate the bond length of the bond in picometers.
A solution that contains 87.2g of an unknown compound in 392.4g of water freezes at -8.00 degrees C. Calculate the molar mass(in units of g/mol) of the solute. Kf of water is 1.86 degrees C/m.
It decomposes into its elements. Write the balanced equation for this reaction. If 71.8 g of Hgo is decomposed, calculate the volume of oxygen at STP
verify the law of multiple proportions for an element X, which forms oxides having percentages of X equal to 77.4%, 63.2%,69.6% and 72.0%
calculate the ph of buffer solution made from .20 M HC2H3O2 and .050 M C2H3O2 that has an acid dissociation constant for HC2H3O2 of 1.8*10-5.
At 125°C, Kp = 0.25 for the following reaction. 2 NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) A 1.00 L flask containing 14.8 g NaHCO3 is evacuated and heated to 125°C.
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