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State equations that show what happens when the subsequent solid ionic compounds dissolve in water. Include states in your answers.
MgCl2
Al(NO3)3
sodium carbonate
period of periodic table,there are atom with a negative electron affinity identify of these atoms and explain why the electron affinity is negative.?
How many moles of Ba
Calculate the partial pressure (in atm) of HBr at equilibrium when 5.00 atm of CH3Br and 5.00 atm of H2O react at 1000 K according to the following chemical equation
Calculation of stoichiometric points of inflection on a titration curve is very useful in choosing indicators that will change color (have an end point) at the equivalence point. How does an end point differ from an equivalence point
At standard temperature and pressure (0 and 1.00 ), 1.00 of an ideal gas occupies a volume of 22.4 . What volume would the same amount of gas occupy at the same pressure and 30
If 22.22 mL of a 1.50 M Ni(NO3)2 solution is diluted to exactly 250.0 mL, what will be the concentration of the dilute solution
Formic acid has a Ka TEN times larger than that of acetic acid. In solutions with the same molarity, the formic acid solution will have this many times the [H+] of the acetic acid.
A beaker with 1.50×102mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.20mL of a 0.330\it M \rm HCl solution to the beaker.
What volume of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1.00 L of a buffered solution at a pH of 3.50? Present answer in mL units and use 4 significant figures.
Define A hemoglobin subchain contains 146 amino acids. Explain how many DNA base pairs are required to code for all the amino acids in the subchain
Hypochlorous acid, HOCl, is a weak monoprotic acid. Using the information for this acid in Appendix F, calculate the pH (round to one decimal) and the percent ionization _2 _(round to two decimals) of a 0.1M solution of the acid at 250C.
The mole fraction of potassium nitrate in an aqueous solution is .0194. The density of the the solution is 1.0627 g/mL. Calculate the molarity of the solution.
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