What is [OH^-] in a solution of 1.25M NH3 and 0.78 M NH4 NO3 ? NH3(a q)+H2 O(l) ⇌NH4^+(a q)+OH^-

step 1 Here the equilibrium reaction is represented plus we have the ionization value, ionization of ba

What is [OH^-] in a solution of 1.25M NH3 and 0.78 M NH4 NO3...

What is $\left[\mathrm{OH}^{-}\right]$ in a solution of 1.25$M \mathrm{NH}_{3}$ and 0.78 $\mathrm{M} \mathrm{NH}_{4} \mathrm{NO}_{3} ?$ $$ \mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{NH}_{4}^{+}(a q)+\mathrm{OH}^{-}(a q) \quad K_{\mathrm{b}}=1.8 \times 10^{-5} $$

What is $\left[\mathrm{OH}^{-}\right]$ in a solution of 1.25$M \mathrm{NH}_{3}$ and 0.78 $\mathrm{M} \mathrm{NH}_{4} \mathrm{NO}_{3} ?$
$$
\mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{NH}_{4}^{+}(a q)+\mathrm{OH}^{-}(a q) \quad K_{\mathrm{b}}=1.8 \times 10^{-5}
$$

Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in which the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products over time. This concept is fundamental in analyzing reactions in solution, where reversible processes reach a balance that can be described mathematically.

Equilibrium Constant Expression

The equilibrium constant expression quantifies the relationship between the concentrations of reactants and products at equilibrium. By using the equilibrium constant (K), one can set up expressions that relate the ion concentrations in weak acid or base reactions, enabling the calculation of species concentrations under equilibrium conditions.

Common Ion Effect

The common ion effect occurs when a solution containing a common ion is added to an equilibrium system, leading to a shift in the equilibrium position. This effect reduces the degree of ionization of a weak acid or base by increasing the concentration of one of its products, thereby influencing the final concentrations of all species in the reaction.

Buffer Solutions

Buffer solutions consist of a weak acid and its conjugate base or a weak base and its conjugate acid. They resist significant changes in pH when small amounts of strong acids or bases are added. The presence of both components in the buffer allows it to neutralize added acids or bases, maintaining a relatively stable pH in the system.

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