If 990. mL of water is added to 10.0 mL of 0.10 M HCl, what is the pH of the resultant solution?
回答 (3)
2017-10-23 11:26 am
✔ 最佳答案
Initial no. of moles of HCl = No. of moles of HCl in the resultant solutionM₁V₁ = M₂ V₂
(0.10 M) × (10.0 mL) = M₂ × (999 + 10.0 mL)
M₂ = 0.1 × (10.0/1000) = 0.0010 M
1 mole of HCl dissociates to give 1 mole of H⁺ ions.
In the resultant solution, [H⁺] = [HCl] = 0.0010 M
pH = -log[H⁺] = -log(0.0010) = 3.0
2017-10-23 11:40 am
Isn't that amazing -- dilution, adding water, makes the pH bigger!! (Better see why!)
2017-10-23 11:16 am
M1V1 = M2V2
M1 = 0.10
V1 = 10 mL
V2 = 1000 Ml
Solve for M2
Answer: 0.0001 M
M1 = 0.10
V1 = 10 mL
V2 = 1000 Ml
Solve for M2
Answer: 0.0001 M
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