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ra1l [238]
4 years ago
14

What is the final concentration of a solution prepared by diluting 35.0 ml of 12.0 m hcl to a final volume of 1.20 l? what is th

e final concentration of a solution prepared by diluting 35.0 ml of 12.0 m hcl to a final volume of 1.20 l?
Chemistry
1 answer:
Dafna1 [17]4 years ago
8 0
We know that, M1V1     =     M2V2
                        (Initial)          (Final)
where, M1 and M2 are initial and final concentration of soution respectively. 
V1 and V2 = initial and final volume of solution respectively

Given: M1 = 12 m, V1 = 35 ml and V2 = 1.2 l = 1200 ml

∴ M2 = M1V1/V2 = (12 × 35)/ 1200 = 0.35 m
Final concentration of solution is 0.35 m
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\begin{aligned} {\rm [OH^{-}]} &= \frac{K_{\rm w}}{[{\rm H_3O^{+}}]}\\ &\approx\frac{1^{-14}}{3.9\times 10^{-4}} && \rm {\leftarrow Only~under~25^{\circ}C.}\atop{}\\&\approx \rm 2.6\times 10^{-11}\; M\end{aligned}.

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