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find the specific solubilities (in g/100g H2O) in both cold and hot water for AgCl, PbCl2, and Hg2Cl2.
A 100.0 g copper sample (specific heat = 0.385 J/goC) at 100.0oC is added to 50.0 g water at 26.5oC. What is the final temperature of the copper-water mixture?
You are asked to prepare 150 mL of a 0.059 M solution of silver nitrate. How many grams of silver nitrate do you need to weigh out.
Consider a 53.5 g sample of H2O(g) at 117°C. What phase or phases are present when 134 kJ of energy is removed from this sample.
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.
Consider the reversible reaction: A(g) 2B(g) At equilibrium, the concentration of A is 0.381 M and that of B is 0.154 M. What is the value of the equilibrium constant, Keq?
A car battery contains 1.0 L of 4.3 M sulfuric acid. Using the value in your answer to question E., calculate how many TUMS® tablets would be required to neutralize all the sulfuric acid in a car battery.
How many grams of Cu(OH)2 can be produced from the reaction of 0.500g Cu with 30.0 mL of 3.0M NaOH? what is the limiting reagent?
A reaction of one liter of chlorine gas with 3 liters of fluorine gas yields 2 liters of a gaseous product. All gas volumes are at the same temperature and pressure. What is the formula of the gaseous product?
Determine the mass of the steel bar if the final temperature of the system is twenty one degree Celsius?
Determine the pH at the point in which the acetate ion concetration equals the acetic acid concentration. (that is where the acetic acid is 50% ionized)
25 mL of 0.3 M HCl are diluted to 500 mL. What is the molarity of the resulting HCl solution.
Calculate the molecular rms speeds of He atoms at 10, 100, 1000 K in units of meters per second and miles per hour.
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