[OH⁻] in aqueous solution A is = 4.3*10⁻⁴ M and [H₃0⁺] in aqueous solution of B is 7.3*10⁻¹⁰ M, pH of which solution will be less ? Which solution will be more basic? Solve the given problem.
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we know, in distilled water , PH + POH = 14
so, [H3O+] × [OH-] = 10^-14
[ note :- [H+] = [H3O+] ]
so, For solution A, [H3O + ] = 10^-14/[OH-]
= 10^-14 /(4.3 × 10^-4)
= 2.32 × 10^-11 M
For solution B, [H3O + ] = 7.3 × 10^-10 M
Since the hydronium ion concentration of solution B is more, so its pH will be less.
The solution having the more pH will be more basic.here we see,
pH of solution A > pH of solution B.
[ because we know, pH = -log[H3O+] , hence higher the concentration of H3O+ , lower will be value of pH, here concentration of B is greater than concentration of A . therefore A will have more pH ]
As solution A will have more pH so it will be more basic.
so, [H3O+] × [OH-] = 10^-14
[ note :- [H+] = [H3O+] ]
so, For solution A, [H3O + ] = 10^-14/[OH-]
= 10^-14 /(4.3 × 10^-4)
= 2.32 × 10^-11 M
For solution B, [H3O + ] = 7.3 × 10^-10 M
Since the hydronium ion concentration of solution B is more, so its pH will be less.
The solution having the more pH will be more basic.here we see,
pH of solution A > pH of solution B.
[ because we know, pH = -log[H3O+] , hence higher the concentration of H3O+ , lower will be value of pH, here concentration of B is greater than concentration of A . therefore A will have more pH ]
As solution A will have more pH so it will be more basic.
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