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What is the pH of a solution that is 0.125 M in methylamine (CH3NH2) and 0.175 M in methylamine chloride (CH3NH3Cl)?
A japanese car is advertised as having a gas mileage of 15 km/L. Convert this rating to miles per gallon.
A chemical reaction is known to occur spontaneously under standard conditions. Which of the following statements is/are true (more than one answer may be selected):
Calculate the mole fraction of benzene in a solution of benzene and toluene that has a total vapor pressure of 266mmHg at 60 degrees C. Note that both components contribute to the vapor pressure over the solution.
Calculate the mass of sodium chlorate that must be decomposed to form 6.5 g of oxygen. 2NaClO3(s) → 2NaCl(s) + 3O2(g)
Compute w when 181 grams of iron (III) oxide (MM = 159.7 g/mol) combines with excess carbon(C)) to produce carbon dioxide(CO 2 ) gas at 359 K: express your answer in kilo joules
What would the solubility of copper (II) tartrate be in a solution that contains 0.12 M sodium tartrate?
What is the pH of the buffer that results when 12.5 g of NaH2PO4 and 22.0 g Na2HPO4 are mixed and diluted with water to 0.500 L? (The acid dissociation constants for phosphoric
A solution was prepared to have a density of 1.20 g/mL and a molality of 2.24 m at 22oC. The Mm of the solute is 63.10 g/mol. (a) What is the molarity of the solution?
If, in a certain experiment, over a specific time period, 0.0035 mol PH3 is consumed in a 2.0 L container during each second of reaction, what are the rates of production of P4 and H2 in this experiment?
a nitrogen fertilizer that is manufactured from ammonia and carbon dioxide. 2 NH3(g) CO2(g) ? NH2CONH2(aq) H2O(l) What volume of ammonia at 45°C and 1.60 atm is needed to produce 908 g (2 lb) of urea?
what is the minimum number of moles of sodium hydroxide required of this hydrolysis reaction to go to completion and what is the limiting reagent in this experiment?
a student used a pH probe that was not properly calibrated. the probe reads the pH one unit higher than it should be. what would the calculated Ka value of the unknown acid
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