a. pH = 12.711
b. pH = 1.769
pH is the degree of acidity of a solution that depends on the concentration of H⁺ ions. The greater the value the more acidic the solution and the smaller the pH.
pH = - log [H⁺]
So that the two quantities between pH and [H⁺] are inversely proportional because they are associated with negative values.
A solution whose value is different by n has a difference in the concentration of H⁺ ion of 10ⁿ.
The pH value of a reaction between strong acid HCl and strong base NaOH can be estimated from the rest of the reaction product
1. If the remainder of the reaction product is obtained the remaining strong base of NaOH then the pH is sought from the concentration of OH⁻ / [OH⁻] by using the formula pH = 14-pOH
[OH ⁻] = b. Mb where
b = number of OH⁻
Mb = strong base concentration
2. If the rest of the reaction results obtained the remaining strong acid HCl, the pH is sought from the concentration of H⁺ / [H⁺] by using the formula
[H⁺] = a. M
a = valence of acid / amount of H⁺ released
M = acid concentration.
3. if both of them run out of reaction, then pH = 7
We complete the answer choices
Calculate the pH of the resulting solution if 34.0 mL of 0.340 M HCL (aq) is added to
a) 44.0mL of 0.340 M NaOH (aq).
b) 24.0mL of 0.440 M NaOH (aq)
a. mole HCl = 34.0mL x 0.340 M = 11.56 mmol
mol NaOH = 44.0 ml x 0.340 M = 14.96 mmol
The remaining moles: 14.96 - 11.56 = 3.4 mmol
[OH-] = mmol / total volume
[OH-] = 3.4 / 44 + 34
[OH-] = 0.0513
pOH = - log 5.13.10-2
pOH = 1,289
pH = 14-1.289 = 12.711
b. mole HCl = 34.0mL x 0.340 M = 11.56 mmol
mol NaOH = 24.0mL x 0.440 M = 10.56 mmol
The remaining moles: 11.56 -11.56 = 1 mmol
[H+] = mmol / total volume
[H+] = 1 / 24 + 34
[H+] =0.017
pH = - log 0.017
pH = 1.769
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Keywords : pH, acid, base, HCl,NaOH
