The [H_3 O^+] of an aqueous solution is [4.38 Times 10^-9]. What is the pH of th
ID: 923927 • Letter: T
Question
The [H_3 O^+] of an aqueous solution is [4.38 Times 10^-9]. What is the pH of the solution? The hydronium ion concentration of a pH neutral aqueous solution is decreased by three orders of magnitude. Answer the following questions about the solution. Does the solution become acidic or basic? Does the pH increase or decrease? By how many pH units does the pH change? Does the molar concentration of hydroxide increase or decrease? By how many orders of magnitude does the molar concentration of hydroxide change? The [OH^-] of an aqueous solution is [9.10 Times 10^-3], What is the [H_3 O^+] in the solution? The [OH^-] of an aqueous solution is [9.89 Times 10^-4]. What is the pH of the solution? Draw a reaction coordinate (aka energy diagram) for both an exothermic and an endothermic reaction. Be sure to label the axes, the average energies of the reactants and the products, the, energy released or absorbed, and the activation energy.Explanation / Answer
[H+] = 4.38*10^-9
pH = -log[H+] = -log(4.38*10^-9) = 8.358
120-124)
pH = 7 or 10^-7 in [H+]
if
120if you decrease by 3 magnitudes, then it becoimes BASIC (10^-10 in H+ ions)
The pH will increase since pH = -log(H+) and log of H is being increases
the pH must change by 3 units i.e. 10^3 = 1000 or 10*10*10
[OH-] ions must increase, since [H+] decrease and this must be valid:
Kw = [H+][Oh-] = 10^-14
the OH- ions increase by magnitude of 3 or about 1000 times
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