Difference between revisions of "PH"
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: An [[acid]] will have a greater [[concentration]] of [[Hydrogen Ion (Chemistry)|Hydrogen ions]] the lower on the '''pH''' scale. | : An [[acid]] will have a greater [[concentration]] of [[Hydrogen Ion (Chemistry)|Hydrogen ions]] the lower on the '''pH''' scale. | ||
: An [[alkali]] will have a greater [[concentration]] of [[Hydroxide Ion (Chemistry)|Hydroxide ions]] the higher on the '''pH''' scale. | : An [[alkali]] will have a greater [[concentration]] of [[Hydroxide Ion (Chemistry)|Hydroxide ions]] the higher on the '''pH''' scale. | ||
| − | : A [[Neutral (Chemistry)|neutral]] [[solution | + | : A [[Neutral (Chemistry)|neutral]] [[solution]] will have an equal [[concentration]] of [[Hydrogen Ion (Chemistry)|Hydrogen ions]] and [[Hydroxide Ion (Chemistry)|Hydroxide ions]] and have a '''pH''' of 7. |
==Key Stage 4 Higher== | ==Key Stage 4 Higher== | ||
| Line 28: | Line 28: | ||
: An [[acid]] will have a greater [[concentration]] of [[Hydrogen Ion (Chemistry)|Hydrogen ions]] the lower on the '''pH''' scale. | : An [[acid]] will have a greater [[concentration]] of [[Hydrogen Ion (Chemistry)|Hydrogen ions]] the lower on the '''pH''' scale. | ||
: An [[alkali]] will have a greater [[concentration]] of [[Hydroxide Ion (Chemistry)|Hydroxide ions]] the higher on the '''pH''' scale. | : An [[alkali]] will have a greater [[concentration]] of [[Hydroxide Ion (Chemistry)|Hydroxide ions]] the higher on the '''pH''' scale. | ||
| − | : A [[Neutral (Chemistry)|neutral]] [[solution | + | : A [[Neutral (Chemistry)|neutral]] [[solution]] will have an equal [[concentration]] of [[Hydrogen Ion (Chemistry)|Hydrogen ions]] and [[Hydroxide Ion (Chemistry)|Hydroxide ions]] and have a '''pH''' of 7. |
: In [[acid]]s for a '''pH''' decrease of 1 there must be 10 times greater [[concentration]] of [[Hydrogen Ion (Chemistry)|Hydrogen ions]] in [[solution]]. | : In [[acid]]s for a '''pH''' decrease of 1 there must be 10 times greater [[concentration]] of [[Hydrogen Ion (Chemistry)|Hydrogen ions]] in [[solution]]. | ||
Revision as of 17:13, 28 June 2019
Contents
Key Stage 3
Meaning
A pH scale with the colours of Universal Indicator at those pH values and some examples of substances at those pH values.
The pH scale is a numbered list from 0 to 14 that is used to identify how acidic or basic a substance is.
About pH
- pH is written with a lower case p and an upper case H and refers to the 'power of Hydrogen' as there are free Hydrogen ions in an acid.
- Acids have a pH of less than 7 with the strongest acids being at pH 0.
- Bases have a pH greater than 7 with the strongest bases being at pH 14. Remember alkalis are a base dissolved in water.
- pH 7.0 is neutral.
Key Stage 4 Foundation
Meaning
The pH scale is a numbered list from 0 to 14 that is used to identify how acidic or basic a substance is.
About the pH Scale
- The pH of a solution is determined by the strength and concentration of Hydrogen ions in an acid or Hydroxide ions in an alkali.
- An acid will have a greater concentration of Hydrogen ions the lower on the pH scale.
- An alkali will have a greater concentration of Hydroxide ions the higher on the pH scale.
- A neutral solution will have an equal concentration of Hydrogen ions and Hydroxide ions and have a pH of 7.
Key Stage 4 Higher
Meaning
The pH scale is a numbered list from 0 to 14 that is used to identify how acidic or basic a substance is.
About the pH Scale
- The pH of a solution is determined by the strength and concentration of Hydrogen ions in an acid or Hydroxide ions in an alkali.
- An acid will have a greater concentration of Hydrogen ions the lower on the pH scale.
- An alkali will have a greater concentration of Hydroxide ions the higher on the pH scale.
- A neutral solution will have an equal concentration of Hydrogen ions and Hydroxide ions and have a pH of 7.
- In acids for a pH decrease of 1 there must be 10 times greater concentration of Hydrogen ions in solution.