Ca(OH)2 + 2HCl = Cacl2 + 2H2O
The general equation for an acid-base reaction is: acid + base → salt + water. This represents the neutralization reaction that occurs when an acid and a base react to form a salt and water.
The equation that best describes an Arrhenius acid-base reaction is: acid + base → salt + water. The acid donates a proton (H+) to the base, forming water as a product. This reaction results in the formation of a salt, which is a compound composed of ions.
H+ (aq) + OH− (aq) H2O H+ (protons) from the acid, OH− from the base, they neutralise each other and water is the product.
In a weak base-strong acid titration, the balanced chemical equation is: Base (B) Acid (H) Conjugate Acid (BH) This equation represents the reaction between the weak base (B) and the strong acid (H), resulting in the formation of the conjugate acid (BH).
To calculate the change in pH in a chemical reaction, you can use the Henderson-Hasselbalch equation. This equation relates the pH of a solution to the concentration of the acid and its conjugate base. By knowing the initial concentrations of the acid and base, as well as the equilibrium concentrations after the reaction, you can calculate the change in pH.
The general equation for an acid-base reaction is: acid + base → salt + water. This represents the neutralization reaction that occurs when an acid and a base react to form a salt and water.
The equation that best describes an Arrhenius acid-base reaction is: acid + base → salt + water. The acid donates a proton (H+) to the base, forming water as a product. This reaction results in the formation of a salt, which is a compound composed of ions.
H+ (aq) + OH− (aq) H2O H+ (protons) from the acid, OH− from the base, they neutralise each other and water is the product.
An acid-base reaction involves the transfer of a proton (H+ ion) from an acid to a base. The net ionic equation for an acid-base reaction typically shows the ions involved in the reaction with charges omitted for species that exist in the same form on both sides of the equation. This net ionic equation highlights only the species directly involved in the reaction, excluding spectator ions.
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In a weak base-strong acid titration, the balanced chemical equation is: Base (B) Acid (H) Conjugate Acid (BH) This equation represents the reaction between the weak base (B) and the strong acid (H), resulting in the formation of the conjugate acid (BH).
A typical example is:NaOH + HCl = NaCl + H2O
The equation involved is a neutralization reaction. HCl + NaOH -> NaCl + H2O In this reaction, acid and base react to produce a salt.
Since HCl is a strong acid and Ba(OH)2 is a strong base, the reaction that takes place is a simple neutralization reaction. The reaction is represented by the net ionic equation: H+(aq) + OH-(aq) ---> H2O This is the equation whenever any strong acid and strong base react.
To calculate the change in pH in a chemical reaction, you can use the Henderson-Hasselbalch equation. This equation relates the pH of a solution to the concentration of the acid and its conjugate base. By knowing the initial concentrations of the acid and base, as well as the equilibrium concentrations after the reaction, you can calculate the change in pH.
The acid-base chemical reaction that is irreversible is the reaction between a strong acid and a strong base.
This is an acid - base reaction: CaO + 2H+ + ( 2NO3- ) --> Ca2+ + H2O + ( 2NO3- )