Explore BrainMass
Share

Explore BrainMass

    Titrations - rain water with NaOH

    This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!

    60. A 155 mL sample of rainwater is titrated using 0.0095 M NaOH solution. If 4.8 mL of the NaOH solution was required to reach the endpoint, what was the pH of the rainwater? The computer gave the following hint: Calculate the number of moles of NaOH to reach the endpoint. From this calculate the hydrogen ion concentration and the pH.

    © BrainMass Inc. brainmass.com October 9, 2019, 4:07 pm ad1c9bdddf
    https://brainmass.com/chemistry/chemical-measures-of-environmental-indicators/titrations-rain-water-naoh-22980

    Solution Preview

    Molarity of the solution = 0.0095M = 0.0095 moles/liter

    Amount of solution used to reach the end point = 4.8ml = 4.8*10^-3 liter

    Thus the number of moles of NaOH used up

    = ...

    Solution Summary

    Detailed explanations without skipping a step.

    $2.19