anonymous
  • anonymous
What volume of concentrated hydrochloric acid (12.0 M HCl) is required to make 2.0 liters of a 3.0 M HCl solution? 5.0 liters 0.24 liters 0.50 liters 6.0 liters
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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jamiebookeater
  • jamiebookeater
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taramgrant0543664
  • taramgrant0543664
So step one is to determine the moles of HCl to do this use the formula: n=cv Where n is the number of moles, c is the concentration which is equal to 3.0M and v is the volume in litres which is the 2.0L Plug your numbers in and solve for n
taramgrant0543664
  • taramgrant0543664
Since we have the moles from the above step we can then use the same formula except we are going to use it to find v So v=n/c Where v is the volume you are solving for, n is the moles that we found above and c is the concentration which is the 12.0M
taramgrant0543664
  • taramgrant0543664
Just to clarify in the first step I should have said that we needed to find the moles of the 3.0M HCl as both concentrations are for HCl

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Rushwr
  • Rushwr
So basically the steps would be; 1. Finding the number of moles in the final solution That would be 3x 2= 6 moles ( use n=C x V) 2. Since we are given the concentration of the HCl we have to use we can easily find the volume . Use n= C x V n= 6 moles. because the no. of final solution should be the same We know n and C . Now it's just the matter of substituting the values and obtaining V ( V= 0.5L )

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