What is the molarity of HCL in a solution if it is prepared when 7.31 mL of 1.74

Question

What is the molarity of HCL in a solution if it is prepared when 7.31 mL of 1.740 M HCL is mixed with 2.69 Ml of water? Remember that the volume of the dilute solution (V2) is the sum of the volume of the acid used pljus the volume of the water used. Sumit Answer you have entered that answer before incorrect. Tries 2/99 Previous Tries Threaded view Charonological View Sorting/Filtering options Export? Preference on what is marked as NEW Mark NEW posts no longer new NEW Anonymous 1 Reply (Mon Mar 7 04: 37:56 pm 2016 (MST)) Please help. Not sure how to complete this problem. NEW Hanna Caban (hjc48:nau) Reply (Mon Mar 7 04: 46:22 pm 2016 (MST)) Your 're going to want to use M1V11 = M2V2, but you have to remember that V2 is going to be 8.43 + 1.57 (volume of water and the solution) I hope this helps. Current discussion settings: Display All post Not new. Once marked not NEW Change? Threaded View choronogical view sorting/Filtering options Exports? Preferences on what is marked as NEW Mark NEW posts no longer new.

Explanation / Answer

HCl : M1=1.740, V1=7.31mL.

2.69 mL of water added to the HCl

The Total volume after dilution = 7.31+2.69

= 10 mL.

M1V1 = M2V2

1.740x7.31 = M2 x 10

M2 = 1.740 x 7.31/10

= 12.7194/10

= 1.27 M.

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