Question

an 18 ml sample of 0.20 m of hf is titrated with 0.36 m naoh. calculate the ph of the solution after 10 ml naoh is added. ka (hf)

Answer 1

The pH of the solution after adding 10 mL of NaOH to the sample of HF is infinity.

Step-by-step explanation:

To find the pH of the solution after adding 10 mL of NaOH to the 18 mL sample of 0.20 M HF, we need to calculate the concentration of HF and NaOH after the addition. First, calculate the moles of HF in the 18 mL sample:

Moles of HF = volume (L) x molarity = 0.018 L x 0.20 M = 0.0036 moles

Then, calculate the moles of NaOH added:

Moles of NaOH = volume (L) x molarity = 0.010 L x 0.36 M = 0.0036 moles

Since HF and NaOH react in a 1:1 ratio, the moles of HF remaining after the addition of NaOH is 0.0036 - 0.0036 = 0 moles. Therefore, the concentration of HF is 0 M. The pH of a 0 M solution is infinite, so the pH of the solution after adding 10 mL of NaOH is infinity.

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