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anonymous
 one year ago
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
anonymous
 one year ago
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

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taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1So 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
 one year ago
Best ResponseYou've already chosen the best response.1Since 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
 one year ago
Best ResponseYou've already chosen the best response.1Just 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

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1So 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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