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chawki
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Homework Statement
Homework Equations
How many Ca2+ ions are there in 0.05 moles of Ca(NO3)2?
The Attempt at a Solution
how do we calculate the number of ions?
PhaseShifter said:Where is the 2 coming from, and why aren't you using the mass of calcium nitrate?
To calculate the number of Ca2+ ions in 0.05 moles of Ca(NO3)2, you first need to determine the molar mass of Ca(NO3)2, which is 164.09 g/mol. Next, multiply the number of moles (0.05) by Avogadro's number (6.02 x 10^23) to get the total number of molecules. Since Ca(NO3)2 contains two Ca2+ ions per molecule, you can then multiply the total number of molecules by 2 to get the number of Ca2+ ions, which in this case would be 6.02 x 10^23 x 2 = 1.204 x 10^24 Ca2+ ions.
The units for the concentration of Ca2+ ions in 0.05 moles of Ca(NO3)2 would be moles per liter (mol/L). This is because concentration is typically expressed as the amount of solute (in this case, Ca2+ ions) per unit volume of solution (in this case, 1 liter).
No, the formula for calculating the number of Ca2+ ions in 0.05 moles of Ca(NO3)2 is specific to this compound. Other compounds will have different formulas for calculating the number of ions present.
Yes, knowing the molar mass of Ca(NO3)2 is necessary in order to calculate the number of Ca2+ ions in 0.05 moles of Ca(NO3)2. This is because the molar mass is used to convert moles of the compound to molecules, which is a necessary step in the calculation.
Yes, the same formula can be used to calculate the number of Ca2+ ions in other concentrations of Ca(NO3)2 as long as you know the concentration (in moles) and the molar mass of the compound. The only change would be the number of moles of Ca(NO3)2 used in the calculation, depending on the concentration given.