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Question- Use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution that is 0.28M in formic acid (HCO2H) and 0.52M in sodium formate (HCO2Na).
Depict your complete computation
What would be the value of the change in concentration of C10H12/change in time during the same period of time? Explain why a catalyst for a forward reaction must also be a catalyst for the reverse reaction. Include an energy level diagram
The following question refers to a solution that contains 1.79 M hydrofluric acid, HF (Ka = 7.2 x 10^-2) and 3.00 M hydrocyanic acid, HCN (Ka = 6.2 x 10^-10). What is the pH of this mixture of weak acids
An organic acid contains 41.4% carbon, 3.47% hydrogen, and 55.1% oxygen by weight. A 0.080-mol sample of this compound weighs 11.60 g. What is the molecular formula of this acid
Identify each of the following substances as ionic, polar covalent, or nonpolar covalent. Also predict its solubility in water. 1. Calcium chloride (CaCl2) 2. Pentane (C5H12) 3.Methyl alcohol (CH3OH)
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 calculation?
An aqueous solution of ethanol, C2H5OH, is 19.00% ethanol by mass and has a density of 0.9700 g mL-1. Calculate the molarity of the ethanol solution.
Which of the following pH values would you expect from the addition of a small amount of a dilute solution of a strong base?
a container is kept at temperature of 400k. it contains 1l of oxygen and 2l of hydrogen. the pressure in the container
if 30.0ml of .150m calcium chloride is added to 15.0 ml of .100 m silver nitrate what will be the final concentration
Explain write a balanced redox reaction for the complete oxidation of ethene (H2C=CH2) to CO2 coupled to the reduction of sulfate to bisulfide. Note that the oxidation define of each carbon in ethene is -2.
The volumes listed correspond to the ½ equivalence point, equivalence point, 1 ½ equivalence point, and 2 equivalence point. The pH will equal pKa2 at the 1 ½ equivalence point, which is 11.55. Therefore, the [H+] = 10^(-11.55) = 2.81 x 10-12
calculate the unknown concentration for the analyte noted as (xM) from the potential data given at 25 oC Pt/Fe 2+ (0.05 M)//Ag+ (xM) /Ag.
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