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Measuring pH and pOH

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What is “pH”? The term “pH” refers to the measurement of the strength of an acid or base. “pH” comes to us from “portenz of hydrogen” – portenz means strength and the hydrogen’s chemical symbol is H. (p + H = pH) pH is measured using the pH scale which runs numerically from 0 to 14. 0 – 7 is the region of acids (acidic solutions) 7 is perfectly neutral (as pure water would be) 7-14 is the region of bases (alkaline solutions)

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The pH Scale The pH scale ranges from A pH of 7 is perfectly neutral like pure water. 0 – 7 is the region of acids (acidic solutions) 7 is perfectly neutral (as pure water would be) 7-14 is the region of bases (alkaline solutions) The pH scale is based on a logarithm to the base 10 which means that each step along the pH scale represents a change in the strength of the acid or base by 10x. So, for acids, an acid with a pH of 3 is ten times stronger than an acid of pH 4. (101) An acid with a pH of 2 is one thousand times stronger than an acid of pH 5. (103 = 10 x 10 x 10) Bases operate by the same rule of measure.

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pIC of the pH Scale

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Ion Product of Water Kw = [H+] [OH-] Kw = 1.0 X 10-14

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Calculations For each concentration given, calculate the pH or pOH. State whether the solution is acidic or basic. 1. [H+] = 1.0 X 10-13 2. [OH-] = 1.0 X 10-12

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**Calculating pH (Part I)**

pH measures the amount of hydrogen ions in a solution. (Recall the link between dissociation and acid/base strength from previous lecture.) When an acid is placed in a solution, it releases the hydrogen (H+) ions and these ions attach themselves to the water molecules (H2O) to make the hydronium ion (H3O+). The more hydronium ions that are made – the more H+ ions that must have been released – the stronger the acid. H+ + H2O H3O+ This means that to measure the pH of an acid, we are actually measuring the number of hydronium ions rather than the number of hydrogen ions because the hydrogen ions quickly form hydroniums.

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**Calculating pH (Part II)**

The formula for calculating ph is: pH = – log10[H3O+] The square brackets around the hydronium means that you are using the Molar concentration of hydronium ions in the solution. The next step is figuring out how to use your calculator to solve problems using this logarithmic relationship.

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Calculate pH Calculte the pH of each solutions below. 1. [H+] = 1.0 X [OH-] = 1.0 X 10-12

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pOH The pH measures the strength of an acid but it does not do the same for a base. A base is a hydrogen ion acceptor A base in water it forms the hydroxide ion (OH–) because it takes an H+ from the water. H2O – H+ OH– The strength of a base is to measured by the number of hydroxide ions in solution since the base molecules steal H+ ions from the water and quickly turn the water molecules into hydroxide ions (OH–).

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**Calculating the pOH The formula for pOH is: pOH = – log10[OH–]**

Again, the squared brackets tells you the value within them is the concentration of the hydroxide ions in the solution being measured. Calculate the pOH of each. 1. [OH-] = 1.0 X 10-13 2. [OH-] = 3.4 X 10-9

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**Connecting pH to pOH pH + pOH = 14**

pH measures the strength of an acid and pOH measures a base. Why then do we use pH to measure a base on the pH scale? We convert pOH into pH because of the relationship between the two values – it is shown below: pH + pOH = 14 When given the concentration of hydroxide ions in a base – we find the pOH and use the relationship above to convert the pOH into a pH value.

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**Calculating pH and pOH from each other.**

The pOH of a solution is 3. What is the pH? Acidic or basic? The pH of a solution is 5.5. What is the pOH. Acidic or basic? Calculate the pH and pOH of each. A. [H+] = 2.4 X 10 -8 B. [OH+] = 4.8 X

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Chapter 19 Notes, part III pH and [H + ]. Hydrogen and hydroxide in H 2 O Working with the Arrhenius acid definition, we say that acids are: –HX H +

Chapter 19 Notes, part III pH and [H + ]. Hydrogen and hydroxide in H 2 O Working with the Arrhenius acid definition, we say that acids are: –HX H +

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