## Presentation on theme: "How is pH defined? The pH of a solution is the negative logarithm of the hydrogen-ion concentration. The pH might be represented mathematically, making use of the."— Presentation transcript:

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1 How is pH defined? The pH of a solution is the negative logarithm of the hydrogen-ion concentration. The pH may be represented mathematically, making use of the following equation: pH = –log In pure water or a neutral solution, = 1 × 10–7M, and the pH is 7. pH = –log(1 × 10–7) = –(log 1 × log 10–7) = –(0.0 + (–7.0)) = 7.0 If the of a solution is higher than 1 × 10–7M, the pH is less than 7.0. If the of the solution is much less than 1 × 10–7M, the pH is better than 7.0. In pure water or a neutral solution, = 1 × 10–7M, and the pH is 7. pH = –log(1 × 10–7) = –(log 1 × log 10–7) = –(0.0 + (–7.0)) = 7.0. If the of a solution is greater than 1 × 10–7M, the pH is less than 7.0. If the of the solution is much less than 1 × 10–7M, the pH is better than 7.0.">

2 Sample problem: Calculating pHWhat is the pH of a solution via a hydrogen-ion concentration of 4.2 × 10–10M? (contd.) 3 Sample problem: Calculating pHCalculate the pH of a solution through a hydroxide concentration of 1.2 × 10–3M. 4 5 How are and also connected in an aqueous solution?The reactivity in which water molecules produce ions is referred to as the self-ionization of water. This reaction have the right to be written as a basic dissociation. H2O(l) ⇄ H+(aq) + OH–(aq) The self-ionization of water occurs to a really tiny level. In pure water at 25°C, the concentration of hydrogen ions is just 1 × 10–7M. The concentration of OH– is likewise 1 × 10–7M because the numbers of H+ and also OH– ions are equal in pure water. Any aqueous solution in which and are equal is a neutral solution. and also connected in an aqueous solution" title="The reactivity in which water molecules develop ions is called the self-ionization of water. This reactivity deserve to be created as an easy dissociation. H2O(l) ⇄ H+(aq) + OH–(aq) The self-ionization of water occurs to a really tiny degree. In pure water at 25°C, the concentration of hydrogen ions is just 1 × 10–7M. The concentration of OH– is also 1 × 10–7M bereason the numbers of H+ and also OH– ions are equal in pure water. Any aqueous solution in which and are equal is a neutral solution.">

6 For aqueous solutions, the product of the hydrogen-ion concentration and also the hydroxide-ion concentration amounts to 1.0  10–14. = 1.0  10–14 This equation is true for all dilute aqueous solutions at 25°C. The product of the concentrations of the hydrogen ions and the hydroxide ions in water is referred to as the ion-product continuous for water (Kw). Kw = × = 1.0 × 10–14 A solution in which is better than is an acidic solution. In acidic services, the is better than 1 × 10–7M. A fundamental solution is one in which is less than . The of a straightforward solution is less than 1 × 10–7M. Basic remedies are additionally known as alkaline solutions. = 1.0  10–14. This equation is true for all dilute aqueous remedies at 25°C. The product of the concentrations of the hydrogen ions and the hydroxide ions in water is called the ion-product consistent for water (Kw). Kw = × = 1.0 × 10–14. A solution in which is higher than is an acidic solution. In acidic services, the is greater than 1 × 10–7M. A fundamental solution is one in which is much less than . The of a basic solution is much less than 1 × 10–7M. Basic options are additionally well-known as alkaline options.">

7 You can usage this equation to transform between pH and pOHKw = pH + pOH Kw always equals 14 So.. pH + pOH = 14 You can usage this equation to transform between pH and also pOH 7 8 Sample problem: Calculating pHCalculate the pH of a solution via a pOH of 12. 8 9 Sample problem: Calculating pHCalculate the pOH of a solution through a pH of 9. 9 10 Sample problem: Calculating pHCalculate the hydrogen ion concentration of a solution through a pH of 8.5.

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10 11 Sample problem: Calculating pHCalculate the hydrogen ion concentration of a solution with a pOH of 13.5. 11 