Determine the ph of a solution when 24.9 mL of 0.023 M HNOs is mixed with 19.4 m

Question

Determine the ph of a solution when 24.9 mL of 0.023 M HNOs is mixed with 19.4 mL of A) 0.0080 M NaoH. Number pH 2.03 B) distilled water. Number pH-189 C) 0.0060 M HCI Incorrecit The total moles of Ht in the final solution are found by summing the moles of H' added to the solution with the moles of H' in the original solution. When calculating the H' concentration of the mixed solution, you may have subtracted the moles of H added to the solution instead Number PH1.99 D) 0.096 M KOH. Number pH12.46

Explanation / Answer

C)
find concentration of H+ in mixture
Concentration of mixture = (n1*C1*V1+ n2*C2*V2) / (V1+V2)
where C1 --> Concentration of 1 component
V1-->volume of 1 component
C2 --> Concentration of other component
V2-->volume of other component
n1 --> number of particle from 1 molecule of 1st component
n2 --> number of particle from 1 molecule of 2nd component

use:
C = (n1*C1*V1+ n2*C2*V2) / (V1+V2)
C = (2*0.3023*24.9+3*0.006*19.4)/(24.9+19.4)
C = 0.3477 M
So,
[H+] = 0.3477 M

use:
pH = -log [H+]
= -log (0.3477)
= 0.459

Answer: 0.459

Related Questions

Navigate

• Browse (All)
• Browse D
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.