A solution is prepared by mixing 50mL of 0.100 HCL and 10 mL of 0.200M NaCl. What is the molarity of chloride ion in this solution? I'm a slow learner so.. I need a step by step guide on how to do this please..

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A solution is prepared by mixing 50mL of 0.100 HCL and 10 mL of 0.200M NaCl. What is the molarity of chloride ion in this solution? I'm a slow learner so.. I need a step by step guide on how to do this please..

Chemistry
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Do u know what molarity is ?
yes, isn't it equal to mol/L?

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Molarity = moles of solute / volume of the whole solution
yeah exactly !!!!
ok.. that is what I have to find out for Cl- what i did so far is do the chemical equation,which i'm not sure if right,, NaCl + HCl -> Na+ + H+ + Cl-
volume of the whole solution so should I add the 0.01 and 0.05?
We are asked to find the molarity of Cl^- ions right? For that we need to find the total moles of Cl^-1 ions. We get Cl^-1 ions from the solutions right? \[NaCl --------> Na ^{+ } + Cl ^{-1}\] \[HCl--------> H ^{+} + Cl ^{-}\] Yeah to find the total volume u have to add up 0.01 and 0.05
yes, right. total volume will be 0.06L..then what?
yeah now we have to find the total moles of Cl^- ions in both the solution
i need to use the value of the given molarities right? so will it be in NaCl: 0.200 x 0.01?
for HCl: 0.100 x 0.05?
yp
now u have to add up the moles from both solutions and put it on the molarity equation
okay... so total volume: 0.06 #of moles of Cl= (0.200 x 0.01) + (0.05 x 0.100) = 0.007 so 0.06/0.007 which is equal to 0.12 M?
moles divided by the volume not the other way round !!!!
oh yeah, i typed it wrong sorry lol I put 0.007/0.06 on my paper it's right i think :D the book says 0.117
yp yp that's the answer :)
thank you :)
no problem :)

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