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A 50.0 mL sample of aqueous Ca(OH)2 requires 32.66 mL of a .812 M nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.
How many milliliters of a 533 mL solution of 1.3 M K3PO4 must be used to make 316 mL of a solution that has 0.79 moles of K+?
Important information about Liquid Crystals, Are there differences between the cholesteryl benzoates and the cholesteryl esters having long carbon chains?
sucrose solution is allowed to react for 195 minutes then determine the mass of sucrose that is hydrolyzed?
The atomic mass of element X is 33.42 amu. A 21.83-g sample of X combines with 80.32 g of another element Y to form a compound XY. Calculate the atomic mass of Y.
The system CO2(g) + H2(g) *) H2O(g) + CO(g) is at equilibrium at some temperature. At equilibrium a 4.00 L vessel contains 1.00 mole CO2, 1.00 mole H2, 2.40 moles H2O, and 2.40 moles CO.
What percentage error would be introduced in a 35.0 mL sample of liquid if the air bubble comes out of the tip of the buret while the liquid sample is being transferred?
Write the equation for the formation of ethyl acetate, What is the purpose of sulfuric acid? What happens if water is removed from the reaction mixture.
Sulfuric acid (H2SO4) is a very strong diprotic acid. If 0.022 moles of sulfuric acid is mixed with water to make 607 mililiter of solution, what is the molarity of H+.
Explain Solid State Chemistry, 1) Write the balanced chemical equation for Fe2O3+2Al?2Fe+Al2O3 using the lowest possible whole number coefficients.
At a pressure of 1.00 atm and a temperature of 20 degree Celsius, 1.72 g CO2 will dissolve in 1 L of water. How much CO2 will dissolve if the pressure is raised to 1.35 atm and the temperature stays the same?
Exactly 100 pounds of cane sugar (dextrose), C12H22O11, were accidentally discharged into a small stream saturated with oxygen from the air at 25 celcius.
The pressure in an automobile tire is 1.83 atm at 26.0°C. What will be the pressure if the temperature warms up to 37.0°C.
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