Write All Each Equation With Absolute Without Absolute Value Given For The Conditions Y=|x + 5| If X

After 30.0 mL of KOH have been added, the pH of the solution is approximately 0.830.

To determine the pH before any base has been added, we need to consider the dissociation of the weak acid HA.

Volume of weak acid HA = 60.0 mL = 0.0600 L

Concentration of weak acid HA = 0.281 M

Since the weak acid HA is a monoprotic acid, it will dissociate as follows:

HA ⇌ H+ + A-

Since the concentration of HA is 0.281 M and the volume is 0.0600 L, we can calculate the initial concentration of H+ ions using the equation: [H+] = [HA].

Therefore, the initial concentration of H+ ions is 0.281 M.

To find the pH, we can use the equation: pH = -log[H+].

Taking the logarithm of 0.281 gives us:

pH = -log(0.281)

pH = 0.550

So, before any base has been added, the pH of the solution is approximately 0.550.

After 30.0 mL of KOH have been added, the primary species left in the solution will be the conjugate base A- (from the dissociation of HA) and the excess OH- ions from the KOH.

To calculate the pH after 30.0 mL of KOH have been added, we need to determine the amount of excess OH- ions and calculate the new concentration of H+ ions.

Given:

Volume of KOH added = 30.0 mL = 0.0300 L

Concentration of KOH = 0.400 M

Since KOH is a strong base, it will completely dissociate to form OH- ions.

The moles of OH- ions added can be calculated as follows:

moles of OH- = concentration of KOH × volume of KOH added

moles of OH- = 0.400 M × 0.0300 L

moles of OH- = 0.0120 mol

Since the weak acid HA and OH- ions react in a 1:1 ratio, the moles of H+ ions neutralized by OH- ions are also 0.0120 mol.

To find the new concentration of H+ ions, we subtract the moles of H+ ions neutralized from the initial concentration:

[H+] = [HA] – moles of H+ neutralized / total volume

The total volume is the sum of the volumes of the weak acid HA and KOH added:

Total volume = Volume of HA + Volume of KOH added

Total volume = 0.0600 L + 0.0300 L

Total volume = 0.0900 L

[H+] = 0.281 M – 0.0120 mol / 0.0900 L

[H+] = 0.281 M – 0.133 M

[H+] = 0.148 M

Finally, we can calculate the pH using the equation: pH = -log[H+]:

pH = -log(0.148)

pH ≈ 0.830

So, after 30.0 mL of KOH have been added, the pH of the solution is approximately 0.830.

To learn more about volume, refer below:

brainly.com/question/1578538

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