QUESTION 6 The strong acid, HCI, is titrated with a strong base, NaOH, in aqueou

Question

QUESTION 6 The strong acid, HCI, is titrated with a strong base, NaOH, in aqueous solution. What is the pH of the titration solution after the addition of 22.62 mL of 0.100 M NaOH to a 50.00 mL of 0.100 MHCI? Write your answer using 3 significant figures, QUESTION 7 At which point along the titration curve of a weak acid titrated with a strong base does the pH- pKa At the half equivalence volume At the equivalence volume Before any base is added Beyond the equivalence volume QUESTION 8 In what pH range will the following titrations have their equivalence points? # HCIO with NaOH HCI with NaF HNO3 with NaOH pH is greater than 7 at the equivalence # pH is less than 7 at the equivalence point pH equals 7 at the equivalence point QUESTION 9 In what pH range will the following titrations have their equivalence points? Weak acid with strong base Weak base with strong acid Strong acid with strong base A pH is greater than 7 at the equivalence pH is less than 7 at the equivalence point pH equals 7 at the equivalence point

Explanation / Answer

6)

Given:

M(HCl) = 0.1 M

V(HCl) = 50 mL

M(NaOH) = 0.1 M

V(NaOH) = 22.62 mL

mol(HCl) = M(HCl) * V(HCl)

mol(HCl) = 0.1 M * 50 mL = 5 mmol

mol(NaOH) = M(NaOH) * V(NaOH)

mol(NaOH) = 0.1 M * 22.62 mL = 2.262 mmol

We have:

mol(HCl) = 5 mmol

mol(NaOH) = 2.262 mmol

2.262 mmol of both will react

remaining mol of HCl = 2.738 mmol

Total volume = 72.62 mL

[H+]= mol of acid remaining / volume

[H+] = 2.738 mmol/72.62 mL

= 0.0377 M

use:

pH = -log [H+]

= -log (3.77*10^-2)

= 1.4236

Answer: 1.42

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