Question

Calculate the amount of 0.1 M base needed to neutralize 10,000 liters of pH 6.0 water. The base is Sodium Hydroxide - NaOH.

a) 10 moles
b) 100 moles
c) 1000 moles
d) 10000 moles

Answer 1

The amount of 0.1 M NaOH needed to neutralize 10,000 liters of pH 6.0 water is 1000 moles.

Step-by-step explanation:

To calculate the amount of 0.1 M NaOH needed to neutralize 10,000 liters of pH 6.0 water, we need to determine the concentration of H3O+ ions in the water. Given that [H3O+] = 10-12M, we can use the formula [H3O+] = Kw/[OH-] to find the concentration of OH- ions. From this, we can determine the amount of base needed.

Using the equation HCl(aq) + NaOH(aq) -> NaCl(aq) + H2O, we can calculate the number of moles of NaOH needed by multiplying the volume of base required for neutrality (10,000 L) by the known concentration of NaOH (0.1 M).

So, the amount of 0.1 M NaOH needed to neutralize 10,000 liters of pH 6.0 water is 1000 moles (c).