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Example Questions
Example Question #91 : Solutions And States Of Matter
How many milliliters of solution is needed to dissolve 5 grams of to prepare a solution of concentration 10M?
In order to calculate the number of milliliters, we must first determine the number of moles in 5 grams of using its molecular weight as a conversion factor:
Using the concentration units as a conversion factor and the number of moles calculated, the number of milliliters can be calculated:
Example Question #11 : Other Solution Concepts
A solution was prepared by diluting 10mL of a 0.500M salt solution to 20mL. What would be the final concentration of this solution?
Use the dilution formula:
Rearranging this equation gives:
Plugging in the values gives:
Therefore, after diluting the solution to 20mL, the solution concentration would be lowered from 0.50M to 0.25M.
Example Question #51 : Solutions
Which of the following is a weak electrolyte?
Solutes that dissociate completely in a solution are called strong electrolytes. Weak electrolytes stay paired to some extent in solutions. As a result, strong electrolytes include ionic compounds and strong acid and bases.
Example Question #13 : Other Solution Concepts
Which of the following definitions is false?
Solubility product, , is the product of ion concentrations at equilibrium in a supersaturated solution of salt.
Ion-product constant of water, , is the product of equilibrium concentration of and ions in an aqueous solution at .
Molality is the number of moles of solute in a solution divided by the number of kilogram of solvent.
The van't Hoff factor, i, is the number of ions that a compound produces in a solution.
Solubility product, , is the product of ion concentrations at equilibrium in a supersaturated solution of salt.
Solubility product, , is the product of ion concentrations at equilibrium in a saturated solution of salt. All other definitions are true.
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