QUESTION 9 L of 1.0 M HCI solution is mixed with 1 L of 1.0 M NaOH solution. Wha

Question

QUESTION 9 L of 1.0 M HCI solution is mixed with 1 L of 1.0 M NaOH solution. What would be the pH of the final solution? acidic (i.e, less than pH-7) basic (i.e., greater than pH-7) O neutral (i.e., pH-7) can't tell because more information is needed. QUESTION 10 1 L of 2.0 M CH3COOH solution is mixed with 1 L of 2.0 M NaOH solution. What would be the pH of the final solution? Assume that Kb for CH3co0 is 10-8 acidic (i.e, pH is less than 7.) basic (G.e, pH is greater than 7) neutral(i.e., pH-7) can't tell because more information is needed.

Explanation / Answer

Ans 9:- neutral (pH = 7)

moles of HCl =1L×1M=1mol

Moles of NaOH= 1L×1M=1mol

Since equal number of strong acid HCl And strong Base NaOH are reacting so the are going to neutralize each other completely So we have a neutralized solutions with pH 7.

Ans 10 :- basic (pH is greater than 7)

Since CH3COOH is a weak acid and NaOH is strong base and we are adding them in the same amount and concentration so obviously solution will have basic nature cause NaOH whould be more effective due to strong basic nature as compared to the weak acid CH3COOH.

Related Questions

Navigate

• Browse (All)
• Browse Q
• Subjects

---

---

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