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The molecular mass of 12C carbon-12 is exactly 12 g/mole. The molecular mass of 16O (oxygen-16) is 15.995 g/mole. Compute the reduced mass of 12C16O molecule.
A buffer is initially 0.180M in 4-nitrophenol (HC6H4NO3) and 0.200M in potassium 4-nitrophenolate (KC6H4NO3). The Ka of 4-nitrophenol is 3.8*10^-4 and the buffer has a pOH = 3.47. If 0.20g on NaOH were added to 100ml of this buffer what would the ..
Calculate the solubility of Fe3+ at a pH of 8.00, assuming that it is controlled by the hydroxide. Express the concentration in both mmol/L and ppm.
a solution is made by mixing 49.0 ml of ethanol c2h6o and 51.0 ml of water. assuming ideal behavior what is the vapor
what is the literature value for the Ksp of potassium hydrogen tartrate in water at 10, 22.5, 35, 50 degrees?
Briefly explain why you can make the assumption that all of the SCN- ion in solutions S2-S6 has been converted to FeNCS^2+ ion.
Decide whether to use acetic acid/acetate or formic acid/formate. Prepare .100 L of a pH 3.74 buffer with a total buffer strength of 0.100 M Calculate the volumes of acid and base necessary to make each buffer.
what is the specific heat for the metal if it takes 48.0j to raise the temperature of an 8.60g piece of unknown metal
How many moles of H+ ions are present in 1.9 L of 0.48 M hydrobromic acid.
Write the chemical equation for the dissociation of the salt into its ions. Write the expression for Ka or Kb and give the value of Ka or Kb 1. 1.0M NaC2H3O2 pH=7.45 2. 1.0M NaHCO3 pH=8.60 3. 1.0M Na2CO3 pH=11.62 4. 1.0m NH4Cl pH=3.98
A 322 mL container holds 0.146 g of Ne and an unknown amount of Ar at 35°C and a total pressure of 635 mmHg. Calculate the moles of Ar present.
A reaction has an activation energy of 195.0 kJ/mol. When the temperature is increased from 473.0K to 493.0K, what will the rate constant increase by a factor of
A 4.40 g nugget of pure gold absorbed 295 J of heat. The initial temperature was 21.0°C. What was the final temperature?
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