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12.00 grams of an unkown solid is dissolved in 200.0 grams of benzene. The mixtures freezes at 3.45 degrees celsius. Find the molar mass of the compound. The reezing point of benzene is 5.49 degree celcius.
50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH. How many mL of the base are required to reach the equivalence point? (Ka for HF is 6.8 x 10-4)
what is the pH of a solution of 125ml of 3.5 M of CH3COOH and 25ml of 1.25 M of NaOH ?
if a plant produces 5.06 mol of C6H12O6, how many moles of CO2 are needed?
Calculate w (in kJ) when 137 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 345 K:
The specific heat cacpacity of solid copper metal is 0.385/Jg-K. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0 0C to 77.5 0C
Nickel nitrate and potassium carbonate react to form nickel carbonate and potassium nitrate. How many milliliters of 0.55M Ni(NO3)¬2 are needed to react with 85 mL of 0.25M K2CO3?
Consider the following specific heats: copper, 0.384 J/g·?C; lead, 0.159 J/g·?C; water, 4.18J/g·?C; glass, 0.502J/g·?C. If the same amount of heat is added to identical masses of each of these substance
When 0.549 moles of a certain gas fill a balloon the volume is 75 mL. If enough of the same gas is added to the balloon until 1.44 moles of gas are present, what is the new volume of the balloon?
A 4.40 g nugget of pure gold absorbed 289 J of heat. The initial temperature was 21.0°C. What was the final temperature?
Derive the fractional compositions for monoprotic and diprotic systems showing the steps as clear as possible including a brief description of a fraction compostion plot.
Consider H2, D2, and H20, treated as ideal gases at pressures of 1 atm and temperatures of 293.2 K.
if you take a 12.5 mL portion of the stock solution and dilute it to a total volume of 0.600L what will be the concentration of the final solution?
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