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How many grams of sodium lactate should be added to 1.00 L of 0.160 M lactic acid to form a buffer solution with pH = 4.10? Assume that no volume change occurs when the sodium lactate is added.
Description of Lipids 1) What are the ingredients of a cephalin? 2) Which fatty acid is always unsaturated in a cephalin? Why?
consider an irreversible adiabatic expansion of an ideal gas against a constant external pressure. derive a formula
A buffer is prepared by combining 25 mL of .50 M NH3(aq) with 25 mL of .20 M HCl. What is the pH of the buffer? (Ka(NH4^+)=5.6 x 10^-10)
the energy of a vibrating molecule is quantized much like theenergy of an electron in the hydrogen atom. the energy
Describe the use of light absorbing reagents in amino acid chromatography. What are these reagents used for? Name two reagents that are commonly used and describe how they react with amino acids.
A solution is prepared by mixing 77.0 mL of 5.00 M HCl and 11.0 mL of 8.00 M HNO3. Water is then added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for this solution.
what is the molarity of the solution formed by mixing 0.20 mol of sodium hydroxide with enough water to make 150 ml of solution
Calculate the cell potential for the following reaction as written at 75 °C, given that [Zn2 ] = 0.870 M and [Ni2 ] = 0.0130 M. The standard cell potential for the half reaction of Zn is 0.76 written as Zn (s) --> Zn2+ + 2e-
calculate th volume of a chlorine solution ( in milliliters) a homeowner should add to her swimming pool if the solution contains 8.00 percent chlorine by mas and there are 5.63 x 10^4 gallons of water in the pool (1 gal = 3.79; density of liquids..
It required 50.00 mL of 0.1565 M KMnO4 to titrate 2.878 g of the solution containing hydrogen peroxide. What was the mass percentage of H2O2 in the solution
consider the titration of 39.0 mL of 0.240 M HF with 0.215M NaOH. Calculate the ph at the following points. calculate the ph after the addition of 9.75 mL of base.
what are possible sources of error that might lead to an erroneous determination of the concentration of the acetic
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