Answer :
Final answer:
The amount of moles of H3O+ or OH- to be added to adjust pH from 8.330 to 7.940 may vary, it essentially involves adding more H3O+ ions to make the solution more acidic or adding OH− ions to make it more basic. Calculations involving logarithms may be necessary in computing pH.
Explanation:
The subject question involves pH adjustment which is a key concept in Chemistry, especially acid-base chemistry. To adjust the pH of a solution from 8.330 to 7.940, you would need to add H3O+ or OH−. This is because pH is a measure of the H+ ion concentration (or OH- ion concentration indirectly) in a solution.
However, the amount of moles of H 3O +or OH − to be added can vary depending on the initial concentration of the base solution and its volume. In such cases, you can use the equation: pH = -log[H3O+] = -log[1.8 × 10-5] = 4.74. For example, moles of H3O+ in a 100 mL 1.8 × 10-5 M HCl solution would be: 1.8 × 10-5 moles/L x 0.100 L = 1.8 x 10-6 moles.
In essence, addition of more H3O+ ions would decrease pH (make the solution more acidic), while addition of OH− ions would increase pH (make the solution more basic). Please note that it might be necessary to perform some calculations which involve the use of logarithms in pH computations.
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