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A solution is prepared by dissolving 18.4 g ammonium sulfate in enough water to make 100.0 mL of stock solution. A 11.00 mL sample of this stock solution is added to 50.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.
A 5.00 g sample of KBr at 25.0°C dissolves in 25.0 mL of water also at 25.0°C. The final equilibrium temperature of the resulting solution is 18.1°C.
Compounds containing carbon-carbon triple bond undergo the Diels-Alder reaction. Formulate the product formed by the reaction
It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n=1 to n=∞.
If 1.50 g of X reacts with 3.54 g of M to produce 4.22 g of a compound with the formula M4X3, and the atomic mass of M is 48.5 amu.
A sample containing 4.80 g of gas has a volume of 15.0 L. Pressure and temperature remain constant. What is the new voume if 0.500 mole gas is added?
How many grams of Cl2 can be prepared from the reaction of 15.0g of MnO2 and 30.0g of HCl according to MnO2 + 4HCl >> MnCl2 + Cl2 + 2H2O
How many grams of CaH2 are needed to generate 19.0 L of H2 gas if the pressure of H2 is 780. torr at 15 C?
A solution contains an unknown mass of dissolved silver ions. when potassium chloride is add to the solution.,a white precipitate forms.
The half-life of a certain radioactive element is 1,250 years. What percent of the atoms remain after 7,500 years?
The simplest formula of a substance is found to be CH2O, and its approximate molar mass is found by experiment to be 93 g•mol-1. What is its exact molar mass?
You have been provided with a 0.1M aqueous solution of glycine at pH 9.0. Calculate how much (in ml) of 5M NaOH solution that you must add to 1 L of this 0.1M glycine solution in order to bring its pH to exactly 9.80
Your starting mixture contains both KCl and KClO3. Suppose that your starting mixture weighed 2.040 grams total, and suppose that you dertermined during your reaction that you produced 0.0072 mols of O2
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