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Many common weak bases are derivatives of , where one or more of the hydrogen atoms have been replaced by another substituent. Such reactions can be generically symbolized as where is the base and is the conjugate acid. The equilibrium-constant expression for this reaction is where is the base ionization constant. The extent of ionization, and thus the strength of the base, increases as the value of increases. Part A If for is 3.0×10-6, what is the of a 0.175 aqueous solution of ? Express your answer numerically. = Part B If for is 3.0×10-6, what is the percent ionization of a 0.325 aqueous solution of ? Express your answer numerically to three significant figures. percent ionization = Part C If for is 3.0×10-6 , what is the the for the following reaction? Express your answer numerically to two decimal places. =
What will happen to the equilibrium as OH- ions are added?
Compute the volume of the tank if the total pressure of the mixture is 44.08 psi at 86°F. What is the partial pressure of each constituent and the average molecular weight of the mixture
Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash
When CS2(g) (6.437 mol) and 51.91 grams of H2(g) in a 190.0 L reaction vessel at 983.0 K are allowed to come to equilibrium the mixture contains 1.444 mol of CH4(g). What concentration (mol/L) of CS2(g) reacted? CS2(g)+4H2(g) = CH4(g)+2H2S(g)
Write a balanced overall equation for each isomer of stilbene (cis and trans)
a 1004.0 g sample of calcium carbonate that is 95 pure gives 225 l of carbon dioxide at stp when reacted with an excess
Draw the Lewis structure of tartaric and malic acids in a way that shows the geometry of the acid functional groups. Indicate the hybridization of each carbon
A 0.13 M solution of a weak monoprotic acid has a pH of 4.11. what is the Ka of this weak monoprotic acid
A solution is prepared with 3.85 grams of an unknown compound in 100.0 grams of cyclohexane. The solution had a freezing point of 4.18 degree celcius (277.33 kelvins). What is the molar mass of the unknown compound?
A solution is prepared by mixing 20.0 mL of 0.025 M BaCl2 and 200. mL of 0.075 M K2SO4. What are the concentrations of barium and sulfate ions in this solution. Assume only SO42- ions (no HSO4? ) are present.
Celsius and heated to the temperature of 275 degree Celsius at a constant pressure of 0.975 atm. compute the work done?
What is the final concentration (in M) of 15.4 mL iron(III) chloride solution with an initial concentration of 1.94 M which is diluted with 19.5 mL of solvent
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