Start Discovering Solved Questions and Your Course Assignments
TextBooks Included
Active Tutors
Asked Questions
Answered Questions
What would be the relative standard deviation in the molarity of the base if the standard deviation in the measurement of mass in a.) is .002g and this uncertainty limits the precision of calculatio
Calculate the rms (average) speed of PH3 atoms or molecules at 123 oC. Use R = 8.314 kg-m2/K-s2-mol for the value of the gas constant. The average speed of a PH3 atom/molecule at 123 oC is 539 m/s.
Calculate the molar mass of the unknown gas. Remember that the faster the rate of effusion, the shorter the time required for effusion; that is, rate and time are inversely proportional.
If 1L of .15M NaOH is unprotected from mmol of CO2, what will be its new molarity when it is standardized agains a standard solution of HCl using
The boiling points of HCl and CO2 are nearly the same (-85 degrees C and -78 degrees C). Explain why CO2 can be removed from an aqueous solution by boiling briefly while essentially no HCl is lost e
what is the structure of an ester of 2-methylpropionic acid that has the molecular formula: C8H13ClO2 and 5 signals in its 1H NMR spectrum?
Calculate the mass in grams of copper initially present in the penny based on the concentration of copper in the sample, the total volume of the sample, the dilutions to the original stock, and the
Values for Ksp at O degrees C, 50 degrees C, and 100 degrees C are 1.14X10^-15, 5.47X10^-13, and 4.9X10^-14 respectively. Calculate the pH for a neutral solution at each of these temperatures.
Consider the titration of 30.0 ml of 0.048 M NH3 with 0.025M HCl. Calculate the pH after the following volumes of titrant have been added.
Why are the standard reagents used in neutralization titrations generally strong acids and bases rather than weak acids and bases?
Compare in your mind 3 different liquids: pure ethanol, a 50% ethanol/water mixture and a 50 % ethanol/methanol mixture. Rank these three liquids in order of increasing Ptotal when each liquid is in
Calculate the pH at the equivalence point for titrating 0.170 solutions of each of the following bases with 0.170 M HBr
Calculate the solubilities of the following compounds in a .0333M solution of Mg(CIO4)2 using 1. activities and 2. molar concentrations
Looking at the effect of ionic strength on activity coefficients, why would the initial slope for Ca2+ be steeper than that of K+
A 50mL portion of a solution containing .2g of BaCl2.2H20 is mixed with 50mL of a solution containing .3g of NaIO3. Assume the solubility of Ba(IO3)2 in water is small.
The mercury in a .8142g sample was precipitated with excess of H5IO6. The precipitate was filtered and washed free of the precipitating agent, and .4114g was recovered. Calculate the % of Hg2Cl2 in
the liberated CO2 was collected on calcium oxide and found to weigh .0515g. Calculate the percentage of aluminum in the sample
2121g sample of an organic compound was burned in a stream of oxygen adn the CO2 produced was collected in a solution of barium hydroxide. Calculate the percentage of carbon in the sample if .6006 g
treatment of .25g sample of impure potassium chloride with excess AgNO3 resulted in formation of .2912g AgCl. Calculate the % of KCl in the sample.
what is the equilibrium partial pressure of water vapor above a mixture of 44.0 g H2O and 56.0 g CHOCH2CH2OH at 35 Degree C. The partial pressure of pure water at 35.0 degree C is 42.2 mmHg. Assume
What is the change of molar Gibbs energy for the freezing of water at -10C? The vapor pressure of H2O (liquid, -10C) is 286.5Pa. The vapor pressure of H2O (solid, -10C) is 260Pa. At -10C the molar v
An ideal gas at 300K has an initial pressure of 15 bar and is allowed to expand isothermally to a pressure of 1 bar. Calculate the maximum work that can be obtained from the expansion
What weight of sodium formate must be added to 400mL of 1M formic acid to produce a buffer solution that has a pH of 3.50
The mole fraction of oxygen in the atmosphere is .21. If the barometric pressure is 0.975 atm, what is the concentration of oxygen in water? Kh=1.3 x10^-3 M/atm
which of the following aqueous solutions will freeze at the lowest temperature? a. 0.10 m KCl, b. 0.20 m C6H12O6 (glucose), c. 0.050 m AlCl3, d. 0.15 m SrBr2, e. all of the above freeze at the same