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Question- For CsCl, calculate the density using the radius values of Cs (167pm) and Cl(181pm). Illustrate complete Procedure please
A 0.7818g sample containing phosphate (PO4 3-) was dissolved. The phosphate was precipitated as MgNH4PO4 by addition of aqueous Mg2+ followed by addition of aqueous ammonia. After filtration and washing,
Calculate the pZn of a solution prepared by mixing 25.0 mL of 0.0100 M EDTA with 50.0 mL of 0.00500 M Zn2+. Assume that both the Zn2+ and EDTA solutions are buffered with 0.100 M NH3 and 0.176 M NH4Cl to provide a constant pH of 9.00.
What volume (in mL) of 0.566 M solution of potassium hydroxide can be made from 58.9 mL of a 1.87 M solution? Assume the volumes are additive.
Suppose that a 4.0 L sample of gas at 1.0 atm is heated from 44°C to 53°C, during this process the volume doubles. What will the final pressure of the gas sample be
Why we have a decrease in in the volume of the crude organic product during the extraction with HCl. What causes this decrease
how many grams of dry nh4cl need to be added to 2.30 l of a 0.100 m solution of ammonianh3 to prepare a buffer solution
Compound A C8H10 yields theoreticlly three substitution products, C8H9Br, on reaction with Br2. Suggest two possible structures for A. Draw them
Hypothetical element X has 3 stable isotopes. The relative peak intensities are 62.05 for 180.0 u, 100.0 for 184.0 u, and 80.45 for 186.0 u. Explain what is the average atomic mass for X
What is the resulting pH 2)More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 64.0mL
An equilibrium mixture at 225 degrees contains 0.14M NH3 and0.19 M H2 for the reaction of 3H2+N2=2. If the Kc at this temp is 1.0*102, what is the equilibrium concentration of N2
Write a balanced equation for the neutralization of each of the following. Express your answer as a chemical equation. Identify all of the phases in your answer
How many moles of NaF must be added to 100.00mL of 0.15 M HF to prepare a buffer with pH=3.30. Ka(HF)=7.1*10^-4
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