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Explain what is the mass in grams of one mole of any pure substance is called its molar mass is that true or false? And another one to....the isotope hydrogen-1 is the standard used for the relative scale of atomic masses? Is that true or false
A solution is made that is 1.5*10^-3 M in Zn(NO3)2 and 0.130 M in NH3. After the solution reaches equilibrium, what concentration of Zn^2+(aq) remains
At what pH would the given concentrations of Ce4+ (1.67*10^-4), Ce3+ (.185), Mn2+ (1.28x10^-5) and MnO4- (.148) be in equilibrium at 298 K. Chemical equation is 5Ce4+ + Mn2+ 4H2O => 5Ce3+ + MnO4- + 8H+. And E standard is .193V
What is the mole fraction of Kr if the partial pressure of Xe and Ar are 1.60 atm and 2.8 atm, respectively?
Based on the given ion concentration for water below,what is the alkalinity (in mg/L as CaCO3)Note :the ion concentration s in the table below are NOT given in mg/l as CaCO3.
Complete the following and write either the molecular, ionic, or net ionic equation. Unclude physical states. (b) CaCO3 + H2SO4
Depict the general trends in the second ionization energy of an element as a function of its atomic number, over the range Z=1-20. Label the minima as well as maxima on the graph with appropriate element symbol.
How many grams of hydrochloric acid are in 500.0 mL of a 5.000 M solution? 1. 36.50 g 2. 54.75 g 3. 73.01 g 4. 91.25 g
Use MO diagrams to place B2+, B2, and B2- in order of decreasing bond energy and decreasing bond length. A) Greatest bond energy Least bond energy B) Greatest Bond Length Least bond length
a solution is prepared by adding 8.28 grams of an unkown compound to 217 g of cyclohexane c6h12. this solution freezes
benzopinacol and benzopinacolone have nearly identical melting points, describe how you might prove that samples of the two compounds are different
If 29.8 mL of 0.102 M acid with a Ka of 0.000015 is titrated with 0.107 M NaOH solution, what is the pH of the titration mixture at halfway to the equivalence point?
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq).
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