A chemist titrates 160.0 mL of a 0.3261 M sodium hydroxide (NaOH) solution with 0.3549 M HCl solution at 25 °C. Calculate the pH at equivalence. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH =
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First, we need to find the moles of NaOH in the solution. We can do this by multiplying the volume (in liters) by the molarity. \( \text{Moles of NaOH} = 0.160 \, \text{L} \times 0.3261 \, \text{M} = 0.052176 \, \text{moles} \) Show more…
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