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OpenStudy (anonymous):
Calculate the concentration (in molarity) of NaOH solution if 25.0mL of the solution are needed to neutralize 17.4 mL of a 0.132M HCL solution
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OpenStudy (rogue):
If you want to neutralize a certain amount of HCl, you need to have the same amount of NaOH. You can use the titration equation to find the molarity of NaOH required.\[M_A V_A = M_B V_B\]The A is for acid and B is for base by the way.\[17.4 mL \times 0.132 M = 25.0 mL \times M_B\]\[M_B = \frac {17.2 mL \times 0.132 M}{25.0 mL} = 0.0908 M\]So you need 0.091 M of NaOH to neutralize that amount of HCl.
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