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1. A buffer solution contains 0.477 M NH4Cl and 0.356 M NH3 (ammonia). Determine the pH change when 0.073mol NaOH is added to 1.00 L of the buffer.
pH after addition - pH before addition = pH change =
2. Determine the pH change when 0.090 mol KOH is added to 1.00 L of a buffer solution that is 0.384 M in HCN and 0.385 M in CN-.
3. How many moles of potassium hydroxide would have to be added to 250 mL of a 0.383 M hypochlorous acidsolution, in order to prepare an buffer with a pH of 7.270?________moles
4. An aqueous solution contains 0.485 M hydrocyanic acid.
How many mL of 0.347 M potassium hydroxide would have to be added to 225 mL of this solution in order to prepare an buffer with a pH of 9.090?
3. How many moles of potassium hydroxide would have to be added to 250 mL of a 0.383 M hypochlorous acidsolution, in order to prepare buffer with a pH of 7.270?
A buffer is prepared by mixing 453 mL of 0.143 M HCl with 983 mL of 0.848 M ammonia (NH3). Given that the Kb of NH3 is 1.8 x 10-5, calculate the pH of the solution.
In a laboratory experiment, a fermenting aqueous solution of glucose and yeast produces carbon dioxide gas and ethanol. The solution was heated by burning natural gas in a Bunsen burner to distill the ethanol that formed in the flask.
Consider a 53.5 g sample of H2O(g) at 117°C. What phase or phases are present when 134 kJ of energy is removed from this sample.
Find H+ and the pH of the following solutions a) .30M HBr b) a solution made by diluting 10.0 mL of 6.00 M HCl to .300 L with water
A mixture of p-nitroaniline and o-nitroaniline is separated by column chromatography. which compound will be eluted first? Give reason.
The molecular geometries for H2O and SO2 are bent. The H-O-H bond angle in H2O is about 109degrees, whereas the bond angle for O-S-O is about 120degrees, EXplain using lewis diagrams why the molecules have the same molecular geometry but different..
Find the concentration of Pb2 in 0.10 M KI saturated with PbI2. Include activity coefficients in your solubility-product expression.
What is the total vapor pressure 4 at 20° C of a liquid solution containing 0.30 mole fraction benzene, C6H6, and 0.70 mole fraction toluene, C6H5CH3? Assume that Raoult's law holds for each component of the solution.
What assumption did you make about the reaction of KMno4 solution and H2C2O4 solution in those determination that allowed you to consider k to be a constant
to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases.
Look up the accepted "actual" Ka value for acetic acid. How does your value compare? Calculate the percent error for your experimental value
What mass of sucrose should be combined with 453 of water to make a solution with an osmotic pressure of 8.00 at 320 ? (Assume the density of the solution to be equal to the density of the solvent.)
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