KOH act as a nucleufeel
and react with benzil
OH
give electrones to benzil and berak the double bond.
Alkalies can neutralize both concentrated and dilute acids, but dilute acids are 'more easily' neutralized (i.e. require a smaller amount of alkali for the same amount of acid). It is a simple chemical reaction, the amount of alkali required to neutralize an acid can be calculated if you know how they react and the strengths of the acid and alkali. E.g. if you use Potassium Hydroxide (KOH) to neutralize Hydrochloric acid (HCL) the reaction is: KOH + HCL --) KCL + H2O So one molecule of KOH neutralizes one molecule of HCL If you have 1 molar KOH, then : 10 ml of dilute HCL (0.1 molar strength) will be neutralized by 1 ml of KOH 10 ml of a strong HCL (10 molar strength) will be neutralized by 100 ml of KOH Hope that helps.
ethanolic KOH can precipitate the impurities in solution
Del G of KOH = -379.07 Kj/mol hope it is of some use
I assume you mean ethanol + KOH? if so, in order to prevent co-precipitation of piperine and the resin acids, dilute ethanolic KOH is added to the concentrated extract to keep acidic materials in solution as their potassium salts (acid/base rxn occurs). basically it keeps impurities in solution, while piperine precipitates out.
Since they are both acids, you don't usually titrate one against the other. If you want to titrate something, you should use one acid and one base. If one of them is a weak acid/base, the other should be a strong acid/base.So if you want to titrate a solution of acetic acid, use a solution of a known concentration of sodium hydroxide (NaOH) or potassium hydroxide (KOH) instead. You can also use either of those two strong bases to titrate a solution of perchloric acid.
Alkalies can neutralize both concentrated and dilute acids, but dilute acids are 'more easily' neutralized (i.e. require a smaller amount of alkali for the same amount of acid). It is a simple chemical reaction, the amount of alkali required to neutralize an acid can be calculated if you know how they react and the strengths of the acid and alkali. E.g. if you use Potassium Hydroxide (KOH) to neutralize Hydrochloric acid (HCL) the reaction is: KOH + HCL --) KCL + H2O So one molecule of KOH neutralizes one molecule of HCL If you have 1 molar KOH, then : 10 ml of dilute HCL (0.1 molar strength) will be neutralized by 1 ml of KOH 10 ml of a strong HCL (10 molar strength) will be neutralized by 100 ml of KOH Hope that helps.
Potassium Hydroxide(KOH) is a base (it is "basic"). An acid will neutralize a base. Acetic acid can be used to neutralize KOH. Baking soda is a base, so it will not work to neutralize KOH.
KOH is used to prepare liquid soaps.
ethanolic KOH can precipitate the impurities in solution
KOH
we use ; KOH for absorbing CO2. 100 mg KOH and 200 ml purified water. Pyrogallic acid for absorbing O2 Cu2Cl2 with ammonium chloride for absorbing CO.
Del G of KOH = -379.07 Kj/mol hope it is of some use
KOH (potassium hydroxide) is used to determine if a fungal infection exists on the skin.
I assume you mean ethanol + KOH? if so, in order to prevent co-precipitation of piperine and the resin acids, dilute ethanolic KOH is added to the concentrated extract to keep acidic materials in solution as their potassium salts (acid/base rxn occurs). basically it keeps impurities in solution, while piperine precipitates out.
Since they are both acids, you don't usually titrate one against the other. If you want to titrate something, you should use one acid and one base. If one of them is a weak acid/base, the other should be a strong acid/base.So if you want to titrate a solution of acetic acid, use a solution of a known concentration of sodium hydroxide (NaOH) or potassium hydroxide (KOH) instead. You can also use either of those two strong bases to titrate a solution of perchloric acid.
When solving this type of problem, first use the ion charges to predict the formulas of the products. Then use coefficients to balance the equation. H3PO4 (aq) + 3 KOH (aq) --> K3PO4 (aq) + 3 H2O (l)
what acid do you use to test gold