chemistry-class-11-unit-07-chapter-05-ionic-equillibrium-l-5-8-txbujcodroy

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Solution </primary>
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- $\mathrm{HCl} \rightarrow \mathrm{H}^{+}+\mathrm{Cl}^{-}$
- $H_2O$ ia a weak electrolyte
- $\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{H}^{+}+\mathrm{OH}^{-}$
- $\left[\mathrm{H}^{+}\right]_{\mathrm{HCl}} \gg\left[\mathrm{OH}^{-}\right]$
- $\left[\mathrm{H}^{+}\right]>\left[\mathrm{OH}^{-}\right]$
- The solution of HCl in $\mathrm{H}_2 \mathrm{O}$ is acidic

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<footer style = "font-size: 18px">Solution $\rightarrow$ Solution $\rightarrow$ <span style = "color:blue"> Solution </span> $\rightarrow$ Salt of weak acid and strong base $\rightarrow$ Salt of strong  acid and weak base </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Salt of weak acid and strong base </primary>
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- Weak acid -$CH_3COONa$-strong base
- $CH_3COONa\rightarrow CH_3COO^- + Na^+$
- $Na^+$ $\xrightarrow {H_2O}$ $Na^+ (aq)$
- $CH_3COO^{-} + H_2O$ $\rightleftharpoons CH_3COOH+OH^{-}$
- Solution is basic
- Generally, the salt of weak acid and strong base is always basic

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![image](https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-11-unit-07-chapter-05-ionic-equillibrium-l-5_8-txbujcodroy-29.jpg)

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<footer style = "font-size: 18px">Solution $\rightarrow$ Solution $\rightarrow$ <span style = "color:blue"> Salt of weak acid and strong base </span> $\rightarrow$ Salt of strong  acid and weak base $\rightarrow$ Quantitative estimation of acid and base </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Salt of strong  acid and weak base </primary>
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- Weak base$\rightarrow$ $NH_4Cl$ $\rightarrow$strong acid
- $NH_4Cl \rightarrow NH_4^+ + Cl^-$
- $Cl^{-} + H_2O \rightarrow Cl^{-}(aq)$
- $NH_4^{+} + H_2O \rightleftharpoons NH_3(aq) + H_3O^+ (aq)$
- Solution is an acidic solution

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![image](https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-11-unit-07-chapter-05-ionic-equillibrium-l-5_8-txbujcodroy-30.jpg)

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<footer style = "font-size: 18px">Solution $\rightarrow$ Salt of weak acid and strong base $\rightarrow$ <span style = "color:blue"> Salt of strong  acid and weak base </span> $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ Quantitative estimation of acid and base </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Quantitative estimation of acid and base </primary>
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- Quantitative estimation $\rightarrow$ pH scale
- $pH = -loga_{H^+}$
- $a_{H^+}$ - actual concentration of $H^+$
- $a_{H^+}=\gamma_{H^+}[H^+]$
- $\gamma_{H^+} $-activity coefficient

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![image](https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-11-unit-07-chapter-05-ionic-equillibrium-l-5_8-txbujcodroy-31.jpg)

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<footer style = "font-size: 18px">Salt of weak acid and strong base $\rightarrow$ Salt of strong  acid and weak base $\rightarrow$ <span style = "color:blue"> Quantitative estimation of acid and base </span> $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ Quantitative estimation of acid and base </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Quantitative estimation of acid and base </primary>
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- $10^{-4} \hspace{0.5mm}M \hspace{0.5mm}HCl \hspace{0.5mm}solution$
- $HCl \quad \xrightarrow[H_2O] H^{+}(aq)+Cl^{-}(aq)$
- $\quad \quad \quad  10^{-4} {M} \quad \quad 10^{-4} {M}$
- $pH=-log(10^{-4})$
- $pH=4$

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![image](https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-11-unit-07-chapter-05-ionic-equillibrium-l-5_8-txbujcodroy-34.jpg)

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<footer style = "font-size: 18px">Quantitative estimation of acid and base $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ <span style = "color:blue"> Quantitative estimation of acid and base </span> $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ Quantitative estimation of acid and base </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Quantitative estimation of acid and base </primary>
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- $10^-3 \hspace{0.5mm}M \hspace{0.5mm}HCl$
- $pH=-log(10^{-3})$
- $pH=3$
- $10^{-4} \hspace{0.5mm}M \hspace{0.5mm}HCl$,
- $pH=4$
- $10^{-3} \hspace{0.5mm}M \hspace{0.5mm}HCl$
- $pH=3$
- Higher the pH, lower the acid strength

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![image](https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-11-unit-07-chapter-05-ionic-equillibrium-l-5_8-txbujcodroy-35.jpg)

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<footer style = "font-size: 18px">Quantitative estimation of acid and base $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ <span style = "color:blue"> Quantitative estimation of acid and base </span> $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ Quantitative estimation of acid and base </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Quantitative estimation of acid and base </primary>
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- $pOH=-log[OH^{-}]$
- $10^{-4} \hspace{0.5mm}M \hspace{0.5mm}NaOH$
- $NaOH \rightarrow Na^+ + OH^-$
- $\quad \quad \quad  \quad \quad \quad \quad 10^{-4}$
- $pOH=-log[10^{-4}]=4$

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![image](https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-11-unit-07-chapter-05-ionic-equillibrium-l-5_8-txbujcodroy-36.jpg)

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<footer style = "font-size: 18px">Quantitative estimation of acid and base $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ <span style = "color:blue"> Quantitative estimation of acid and base </span> $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ Ionic equilibrium </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Quantitative estimation of acid and base </primary>
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- Weak electrolyte
- $10^{-4}$ M $\hspace{0.5mm }CH_3COOH$
- $CH_3COOH \rightleftharpoons CH_3COO^- + H^+$
- The concentration of $H^+$  can not be $10^{-4}M$ as $CH_3COOH$ is weak electrolyte

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![image](https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-11-unit-07-chapter-05-ionic-equillibrium-l-5_8-txbujcodroy-37.jpg)

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<footer style = "font-size: 18px">Quantitative estimation of acid and base $\rightarrow$ Quantitative estimation of acid and base $\rightarrow$ <span style = "color:blue"> Quantitative estimation of acid and base </span> $\rightarrow$ Ionic equilibrium $\rightarrow$ Ionic equilibrium </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Equilibrium constant </primary>
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- $HA \rightleftharpoons H^{+} + A^{-}$
- $K_a=\frac{\left[H^{+}\right]\left[A^{-}\right]}{[H A]}$
- $K_a=\frac{\left[H^{+}\right]\left[H^{+}\right]}{[H A]}$
- $\left[\mathrm{H}^{+}\right]^2=K_a \times\left[HA\right]$
- $\left[\mathrm{H}^{+}\right]=\sqrt{\mathrm{Ka} \times\left[\mathrm{HA}\right]}$

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<footer style = "font-size: 18px">Ionic equilibrium $\rightarrow$ Ionic equilibrium $\rightarrow$ <span style = "color:blue"> Equilibrium constant </span> $\rightarrow$ Equilibrium constant $\rightarrow$ Equilibrium constant </footer>

### <Success style="font-size:25px"> Ionic Equilibrium L-5 </Success>
### <primary style="font-size:24px"> Equilibrium constant </primary>
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- pOH of a weak base
- $\mathrm{NH}_3+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{NH}_4^{+}+\mathrm{OH}^{-}$
- $\left.K_b=\frac{\left[\mathrm{NH}_4^{+}\right]\left[\mathrm{OH}^{-}\right]}{\left[\mathrm{NH}_3\right][\mathrm{H}}\right]$
- $K_b=\frac{\left[\mathrm{OH}^{-}\right]^2}{\left[\mathrm{NH}_3\right]}$
- $\left[\mathrm{OH}^{-}\right]=\sqrt{\mathrm{K}_b \times\left[\mathrm{NH}_3\right]}$

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<footer style = "font-size: 18px">Equilibrium constant $\rightarrow$ Equilibrium constant $\rightarrow$ <span style = "color:blue"> Equilibrium constant </span> $\rightarrow$ Thank you $\rightarrow$  </footer>