I think it maybe 59.7852%
Answer:
The hydronium ion concentration can be found from the pH by the reverse of the mathematical operation employed to find the pH. [H3O+] = 10-pH or [H3O+] = antilog (- pH) Example: What is the hydronium ion concentration in a solution that has a pH of 8.34? On a calculator, calculate 10-8.34, or "inverse" log ( - 8.34).
Explanation:
Hope it helps!
The last option is correct
Answer:
6,45mmol/L of NaOH you need to add to reach this pH.
Explanation:
CH₃COOH ⇄ CH₃COO⁻ + H⁺ <em>pka = 4,74</em>
Henderson-Hasselbalch equation for acetate buffer is:
5,0 = 4,74 + log₁₀![\frac{[CH_{3}COO^-]}{[CH_{3}COOH]}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BCH_%7B3%7DCOO%5E-%5D%7D%7B%5BCH_%7B3%7DCOOH%5D%7D)
Solving:
1,82 = <em>(1)</em>
As total concentration of acetate buffer is:
10 mM = [CH₃COOH] + [CH₃COO⁻] <em>(2)</em>
Replacing (2) in (1)
<em>[CH₃COOH] = 3,55 mM</em>
And
<em>[CH₃COO⁻] = 6,45 mM</em>
Knowing that:
<em>CH₃COOH + NaOH → CH₃COO⁻ + Na⁺ + H₂O</em>
Having in the first 10mmol/L of CH₃COOH, you need to add <em>6,45 mmol/L of NaOH. </em>to obtain in the last 6,45mmol/L of CH₃COO⁻ and 3,55mmol/L of CH₃<em>COOH </em>.
I hope it helps!
Answer:
<em>hope</em><em> </em><em>you</em><em> </em><em>like</em><em> </em><em>this</em><em> </em><em> </em>
<em>pls</em><em> </em><em>mark</em><em> </em><em>me</em><em> </em><em>as</em><em> </em><em>BRAINLIEST</em><em> </em><em> </em>
<em>stay</em><em> </em><em>at</em><em> </em><em>home</em><em> </em><em>stay</em><em> </em><em>safe</em><em> </em>
Explanation:
Ammonia is a versatile laundry additive, vanquishing stains and dissolving grease as well as whitening whites and softening your bath towels. But its fumes and dangerous reactions when mixed with other household cleaners mean you need to be careful when using it.
