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A solution is created by measuring 3. 60 x 10-3 moles of NaOH and 5. 95 x 10-4 moles of HCl into a container and then water is added until the final volume is 1. 00 L. What is the pH of this solution? Please answer as quickly as possible

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Snor1ax

Answer: 11.478

Explanation:

M   =   MBVB- MAVA/VA + VB

      = number of moles of base - number of moles of acid/total volume

      = 3.6*10^-3 - 5.95*10^-4/1

      = 0.0036-0.000595   = 0.003005

[OH^-]   = M = 0.003005M

POH  = -log[OH^-]

         = -log0.003005

         = 2.522

PH   = 14 - POH

       = 14 - 2.522  

       = 11.478

Therefore, the pH of the solution is 11.478

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