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In an aqueous solution of a weak acid, HA, the assumption is often made that [HA]equilibrium = [HA]initial. This approximation is reasonable if the initial concentration of the acid is sufficiently large compared to Ka.
What multiple of Ka must the initial concentration of a weak acid exceed, for the initial concentration and the equilibrium concentration to be within 9.40 percent of each other?
What the most reactive in water, magnesium , calcium , or aluminum , why?
How much heat is liberated at constant pressure when 68.2mL of liquid benzene (C6H6, d=0.874g/mL) reacts with 54.2mL of 2.82M nitric acid
Given that a 12.00 g milk chocolate bar cotains 9.200 g of sugar, calculate the percentage of sugar preset in 12.00 g of mike chocolate. express your aswer numerically
Problem- A 0.2277 g sample contained only NaCl and KBr. It was dissolved in water and titrated with a 0.04811 M solution of AgNO3. Complete titration of both halides was found to require 51.27mL of the AgNO3 solution. Calculate the weight percent ..
when a 1421 J of heat energy is added to 39.5 g of hexane, C6H14, the temperature increases by 15.9 degree centegrade. Calculate the molar heat capacity
Explain what is the empirical formula of the compound. Combustion engage reacting with excess O2. Presume that all the carbon ends up in CO2 as well as all the hydrogen ends up in H2O. As well assume that all the nitrogen ends up in the NH3 in the..
Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)
Explain the volume of flask E is twice that of flask B. Define what is the partial pressure of Ne relative to the overall pressure when the two flasks are connected together
Slope a is greater than b. What can you conclude regarding the sensitivity of used analytical method for components A and B
If you have 50 ml of a buffered solution of 0.15M HNO2 and 0.05M NaNO2, how many ml of 0.2M HCl can you add before the pH changes significantly
How many grams of KOH are required to neutralized 300ml of 5.0 N HN03 solution.
Four liters of water are equilibrated with a gas mixture containing carbon dioxide at a partial pressure of .3 atm. Henry's law constant for H2CO3* solubility is 2.0 g/L-atm.
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