Answer:
14.91 mL
Explanation:
<em>Assuming the weak acid is monoprotic</em>, we can solve this problem using the equation:
Where subscript 1 stands for the Volume and Concentration of the weak acid, while 2 stands for those of NaOH.
We <u>input the data</u>:
- 25.00 mL * 0.1084 M = 0.1817 M * V₂
And solve for V₂:
Answer:
It would probably be, something that can take up moisture to test it.
Explanation:
(to see if it can evaporate)
Answer:
7.00
Explanation:
When the solutions are mixed, the HCl dissociates to form the ions H+ and Cl-. The ion H+ will react with the NH3 to form NH4+. The stoichiometry for this is 1 mol of HCl to 1 mol of H+ to 1 mol of Cl-, and 1 mol of H+ to 1 mol of NH3 to 1 mol of NH4+.
First, let's find the number of moles of each one of them, multiplying the concentration by the volume:
nH+ = 0.15 M * 25 mL = 3.75 mmol
nNH3 = 0.52 M * 25 mL = 13 mmol
So, all the H+ is consumed, and the neutralization is completed, thus pH will be the pH of the solvent (water), pH = 7.00.
