Search results
Results From The WOW.Com Content Network
The modern commercial production of potassium carbonate is by reaction of potassium hydroxide with carbon dioxide: [3] 2 KOH + CO 2 → K 2 CO 3 + H 2 O. From the solution crystallizes the sesquihydrate K 2 CO 3 ·1.5H 2 O ("potash hydrate"). Heating this solid above 200 °C (392 °F) gives the anhydrous salt.
It is manufactured by treating an aqueous solution of potassium carbonate or potassium hydroxide with carbon dioxide: [1] K 2 CO 3 + CO 2 + H 2 O → 2 KHCO 3. Decomposition of the bicarbonate occurs between 100 and 120 °C (212 and 248 °F): 2 KHCO 3 → K 2 CO 3 + CO 2 + H 2 O. This reaction is employed to prepare high purity potassium carbonate.
Enthalpy change of solution in water at 25 °C for some selected compounds [2] Compound ΔH o in kJ/mol; hydrochloric acid: −74.84 ammonium nitrate +25.69 ammonia: −30.50 potassium hydroxide: −57.61 caesium hydroxide: −71.55 sodium chloride +3.87 potassium chlorate +41.38 acetic acid: −1.51 sodium hydroxide: −44.50
Potassium hypochlorite is produced by the disproportionation reaction of chlorine with a solution of potassium hydroxide: [2] Cl 2 + 2 KOH → KCl + KOCl + H 2 O. This is the traditional method, first used by Claude Louis Berthollet in 1789. [3] Another production method is electrolysis of potassium chloride solution.
3 in solution represents 1 molar equivalent, while 1 mole of CO 2− 3 is 2 molar equivalents because twice as many H + ions would be necessary to balance the charge. The total charge of a solution always equals zero. [8] This leads to a parallel definition of alkalinity that is based upon the charge balance of ions in a solution.
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).
It can be prepared by treating a potassium-containing base such as potassium hydroxide or potassium carbonate with acetic acid: . CH 3 COOH + KOH → CH 3 COOK + H 2 O. This sort of reaction is known as an acid-base neutralization reaction.
Where HV is the hydroxyl value; V B is the amount (ml) potassium hydroxide solution required for the titration of the blank; V acet is the amount (ml) of potassium hydroxide solution required for the titration of the acetylated sample; W acet is the weight of the sample (in grams) used for acetylation; N is the normality of the titrant; 56.1 is ...