Question

In a titration, a biochemist adds 5.00 mL of 0.010 M HCl to 10.00 mt. of 0.010 m NaOH. What is the pH at this point in the titration?

a.2.3
b.2.5
c.11.5
d.11.7

Answer 1

In a titration, the pH at the equivalence point is determined by the concentration and nature of the acid and base.

When 5.00 mL of 0.010 M HCl is added to 10.00 mL of 0.010 M NaOH, the resulting solution will have a neutral pH of 7.

Step-by-step explanation:

In a titration, the pH at a given point is determined by the concentration and nature of the acid and base involved. In this case, 5.00 mL of 0.010 M HCl is added to 10.00 mL of 0.010 M NaOH.

Since both HCl and NaOH are strong acids and bases, the resulting solution will be neutral at the equivalence point, which is when the moles of acid and base are equal.

To calculate the pH at this point, you need to determine the moles of the acid and base.

The moles of HCl can be found by multiplying the volume (in L) by the concentration, giving you 5.00 mL * 0.010 M = 0.050 mmol. The moles of NaOH can be found in the same way, giving you 10.00 mL * 0.010 M = 0.100 mmol.

Since the moles of acid and base are equal at the equivalence point, the concentration of hydronium ions (H3O+) will be equal to the concentration of hydroxide ions (OH-), resulting in a neutral pH of 7.