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You have 75.0 mL of a 2.50 M solution of Na2CrO4 (aq). You also have 125 mL of a 2.15 M solution of AgNO3 (aq).
Calculate the concentration of NO3 when the two solutions are added together.
What concentration of the salt NaC2H3O2 must be added to shift the equilibrium toward the reactants so that the [H3O+] concentration is reduced to pH = 5.5
How many grams of F2 are needed to produce 120. g of PF3 if the reaction has a 78.1% yield?
The ionization energies of rubidium and silver are 4.18 and 7.57 eV, respectively. Calculate the ionization energies of an H atom with its electron in the same orbitals as in these two atoms and account for the difference in values
Compute a wavelength of the yellow light emitted by a sodium lamp if the frequency of the radiation is 5.10*10^-14hz
Consider the molecule cyclohexane, which contains only hydrogen and carbon atoms. When a sample is burned in oxygen, 4.822 g of CO(2) and 1.650g of H(2)O are obtained. What is its simplest formula?
What is the molar mass of a gas that occupies a volume of 1.500 L at a pressure of 356 mm Hg, a temperature of 22.5 C and weighs 0.9847g
aluminum sulfate and sodium phosphate Express your answer as a chemical equation. Identify all of the phases in your answer.
The equlibrium constant (Kc) for the following reaction is 6.7 *10^-10 at 630 C N2(s)+O2(g)>2NO (g). What is the equlibrium constant for (Kc) the reaction 1/2 N2(g)+1/2O2(g)>NO(g)
How many grams of water can be cooled from 36 degrees celsius to 23 degrees celsius by the evaporation of 53g of water.
65.50 ml of 0.161 m hf is titrated with 0.1200 m naoh. what is thenbsp ph after 65.50 ml of base have been added? ka
Finding Kc from Products' Moles, Volume and Percent Reacted, The following reaction occurs at 1600 deg. C. Calculate the equilibrium constant Kc for the reaction.
If the pressure increases to 800. torr, how many moles of gas were added to the container? Assume a constant-volume container.
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