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What is the molarity of the solution that was prepared by dissolving 3.2 g of sulfuric acid in water to a total volume of 500 mL
At room temperature (20), milk turns sour in about 63 hours. In a refrigerator at 3, milk can be stored three times as long before it sours.
Styrene, phenylethene, is treated with H3PO4, an acid whose conjugate base is a poor nucleophile.
Calculate the mass of sodium hydroxide needed to to prepare 100 mL of a 0.10 M solution?
If the highest possible oxidation state for the halogens is +7, and the lowest possible is -1 which of the following could not disproportionate?
1. Why was excess dry ice used in step 3 of the procedure? 2. Why do gas laws use degrees Kelvin rather than degrees Celsius? 3. Were you surprised at how accurately the mass of a molecule of CO 2 could be determined With such simple equipment?
Correct for the water vapor present in the wet dry ice experiment and compare and compare with the mean value for the dry ice experiment. Does the presence of water vapor affect the result?
Calculate the osmotic pressure of a solution containing 20.00mg of hemoglobin in 16.3mL of solution at 25 ? C The molar mass of hemoglobin
The equalibrium constant for the reaction AgBr(s) Ag^+(aq)+Br^-(aq) is the solubility product constant, Ksp=7.7x10^-13 at 25 degrees C. Calculate deltaG for the reaction
Determine the molarity of a solution prepared by dissolving 4.50 mol of NH4Cl in sufficient water to make 2.00 L of solution.
Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) If 1.26 L of H2 gas are formed at STP, how many g of HCl reacted?
Determine the boiling point of a solution of 22.5 g of fructose, C6H12O6 , in 294 g of phenol.
The Kp value was calculated as 8.491 g. What does the Kp value tell you about the solubility of benzoic in the two solvents dichloromethane and water
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