Team_Digby.edited.docx Week 6 Grief, Crisis and Suicidality.pptx mentoring and coaching Griffith,Bill graded.docx For starters, calculate how many moles of aluminium chloride would be needed in order to get a #1.0 * 10^(-3)# #"M"# solution in #"1.75 L"# of solution. As you know, molarity tells you the number of moles of solute present in #"1 L"# of solution. This means that #"1 L"# of #1.0 * 10^(-3)# #"M"# aluminium chloride solution will contain #1.0 * 10^(-3)# moles of aluminium chloride, the solute. In your case, the solution will contain
So, you know that you must dissolve #1.75 * 10^(-3)# moles of aluminium chloride in enough water to make the volume of the solution equal to #"1.75 L"#. Now, aluminium chloride is a soluble ionic compound, which implies that it dissociates completely in aqueous solution to produce aluminium actions and chloride anions
Notice that every #1# mole of aluminium chloride dissolved in water produces #color(red)(3)# moles of chloride anions. This implies that your solution will contain
The answer must be rounded to two sig figs, the number of sig figs you have for the molarity of the solution.
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