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Home / Finding Ph of Solution With Two Acids

Finding Ph of Solution With Two Acids

When we talk about the pH ("potential of hydrogen" or "power of hydrogen") of a solution we are basically discussing the measure of hydrogen ion concentration in a solution. pH in other words is a scale that is used to specify the acidity or basicity of an aqueous solution. Acidic solutions which contain higher concentrations of H+ ions are generally measured to have lower pH values than basic or alkaline solutions.

If the temperature is 25 °C and the solution has a pH of less than 7 then it is acidic. Likewise, solutions with a pH greater than 7 are basic. If a solution has a pH of 7 at this temperature then they are are neutral (For example, pure water which tends to dissociate slightly into equal concentrations of hydrogen and hydroxyl (OH−) ions. The concentration of the dissociated hydrogen ions in pure water is 10-7 moles per litre. Solutions are categorized as acidic or basic based on their hydrogen ion (H+) concentration compared to pure water.

The pH of an aqueous solution is based on the pH scale which typically ranges from 0 to 14 in water. In any case, students can keep these points in mind.

  • Acidic solutions have lower hydroxide concentrations and high hydronium concentrations. Acidic solutions have a hydrogen ion concentration greater than 10-7 moles per litre.
  • Basic solutions have high hydroxide concentrations and lower hydronium concentrations. alkaline (Basic) solution has a lower concentration of H+ ion that is less than 10-7 moles per litre.
  • The concentration of hydrogen ions in a solution is expressed in terms of pH.

Additionally, some indicators (universal indicator paper, etc ) may be used to measure pH. It is solely based on the fact that the indicators colour changes with pH. A visual comparison of the colour of a test solution with a defined colour chart is done. This helps to determine the pH accurately to the nearest whole number.  pH can also be measured using an electronic pH meter.

Mixture of Two Strong Acids

The strong acids completely dissociate in the given solvent. The strength of an acid and the concentration of acid are two different terms.

Acid strength: It measures the degree of ionization of acid in the aqueous solution. The greater the number of cations and anions are dissociated in the aqueous solution the stronger the acid is.

Acid concentration: It measures the number of available acid ions when it is dissolved in a solvent.The concentration is a ratio of solute to the solvent content in the solution. So the concentration of hydrogen ion is the same as that of the acid concentration. The concentration of the hydrogen ion in the mixture is the sum of the acid concentration divided by the total volume.

Consider a mixture of two strong acids

Say N1, V1 is the strength and volume of the first strong acid and N2, V2 is the strength and volume of the second acid.

The concentration of the hydrogen ion in acid 1 is N1V1 and in acid 2 is N2V2

Total hydrogen concentration = N1V1 + N2V2

Total volume of solution = V1 + V2

[H+] = = N 1 V 1 + N 2 V 2 V 1 + V 2 =\frac{N1V1+N2V2}{V1+V2}

From which pH of the solution can be calculated using the formula

p H = − l o g 10 [ H + ] pH = -log_{10}\left [ H^{+} \right ] .

Mixture of Two Strong Bases

The strong bases are completely ionized in the given solution. So the concentration of the hydroxide ion is the same as that of the base concentration. The concentration of the hydroxide ion in the mixture is the sum of the base concentration divided by the total volume.

consider a mixture of two strong bases,

Say, N1, V1 is the strength and volume of the first strong base and N2, V2 of the is the strength and volume of the second base.

The concentration of the hydroxide ion in the first strong base is N1V1 and in the second base is N2V2

Total hydroxide ion concentration = N1V1 + N2V2

The total volume of the solution = V1 +V2

[OH–] = = N 1 V 1 + N 2 V 2 V 1 + V 2 =\frac{N1V1+N2V2}{V1+V2} [H+] = = 1 0 − 14 [ O H − ] =\frac{10^{-14}}{[OH^{-}]}

From which pH of the solution can be calculated

Also Read: Study the pH Change

Mixture of a Strong Acid and a Strong Base

On mixing a strong acid and strong base neutralization (pH = 7) takes place. The resulting solution may be an acid or base depending on the Concentration.

Say, N1, V1 is the strength and volume of the strong acid and N2, V2 is the strength and volume of the strong base.

  • If, N1V1> N2V2, resulting solution will be acidic, with [H+] = = N 1 V 1 − N 2 V 2 V 1 + V 2 =\frac{N1V1-N2V2}{V1+V2}
  •  If, N1V1˂ N2V2, resulting solution will be basic, with [OH–] = = N 2 V 2 − N 1 V 1 V 1 + V 2 =\frac{N2V2-N1V1}{V1+V2}

Weak Acid

Weak acids ionize partly, and Ostwald's dilution law can be applied to calculate pH.

H A ⇌ H + + A − HA\rightleftharpoons H^{+}+A^{-}

Initial concentration, moles/l, C 0 0

At equilibrium, moles /l C(1-α) Cα Cα

So, Acid Ionization constant = K a = [ H + ] [ A − ] H A = ( C α + C α ) c ( 1 − α ) = c α 2 ( 1 − α ) Ka=\frac{[H+][A-]}{HA}=\frac{(C\alpha +C\alpha)}{c(1-\alpha)}=\frac{c\alpha^{2}}{(1-\alpha)}

(i) For very weak electrolytes, since α <<< 1, (1 – α ) = 1

.·. K a = C α 2 α = K a c = K a V Ka=C\alpha^{2\;\;\;\;\;}\alpha = \sqrt{\frac{Ka}{c}}=\sqrt{KaV}

(ii) Concentration [H+] of ion = C α = C K a = K a V C\alpha = \sqrt{CKa}=\sqrt{\frac{Ka}{V}}

iii) p H = − log ⁡ C K a = 1 2 ( − log ⁡ K a − log ⁡ C ) pH=-\log\sqrt{CKa}=\frac{1}{2}(-\log Ka -\log C) ;

p H = 1 2 ( p K a − log ⁡ C ) pH=\frac{1}{2}(pKa -\log C) Increasing dilution, increases ionization and pH

Mixture of strong acid and weak monoprotic acid

Let C1 and C2 be the concentrations of the strong and weak acids. If α is the degree of dissociation in the mixture, then the hydrogen ion concentration = [H+] = C1+ C2*α.

The degree of dissociation of the weak acid will be less than the pure acid because of the higher [H+] from the strong acid. This is referred to as levelling effect. If the [H+] is less than 10-6 mole/l, hydrogen ion concentration from water also is to be added.

Mixture of two Weak Monoprotic Acids

Say the two weak acids HA1 and HA2, have concentrations C1, C2 and degree of ionization α1 and α2.

–

Initial concentration, moles/l

At equilibrium, moles /l C1(1- α1) C1α1+ C2α2 C1α1 C2(1- α2) C1α1+ C2α2 C2α2

So, K a = [ H + ] [ A − ] [ H A ] K a 1 = c 1 α 1 ( c 1 α 1 + c 2 α 2 ) C 1 ( 1 − α ) K a 2 = C 2 α 2 ( 1 α 1 + C 2 α 2 ) C 2 ( 1 − α 2 ) Ka=\frac{[H+][A-]}{[HA]}\;\;\;\;\;\;\;\;Ka1=\frac{c1\alpha 1(c1\alpha 1+c2\alpha 2)}{C1(1-\alpha)}\;\;\; Ka2=\frac{C2\alpha 2(1\alpha 1+C2\alpha 2)}{C2(1-\alpha2)}

Since α is small, Ka1 = (C1α1+ C2α2) α1 Ka2 = (C1α1+ C2α2)α2

α 1 = K a 1 ( C 1 α 1 + C 2 α 2 ) α 2 = K a 2 ( C 1 α 1 + C 2 α 2 ) \alpha 1 = \frac{Ka1}{(C1\alpha 1+C2\alpha 2)}\;\;\;\;\alpha2=\frac{Ka2}{(C1\alpha1+C2\alpha2)} [H+] = C1α1+ C2α2 = = C 1 K a 1 + C 2 K a 2 =\sqrt{C1 Ka1+ C2 Ka2}

Related Topics

  • Chemical Equilibrium
  • Ionic Equilibrium – Degree of Ionization and Dissociation
  • Equilibrium Constant – Characteristics and Applications
  • Le Chatelier's Principle on Equilibrium
  • Solubility and Solubility Product
  • Acid and Base
  • pH Scale and Acidity
  • Hydrolysis, Salts, and Types
  • Buffer Solutions

Finding Ph of Solution With Two Acids

Source: https://byjus.com/jee/ph-and-solutions/