What Is the Correlation Between the pH and Absorption of Chemicals with Varing Concentration?

Literature review

What is the correlation between the pH and absorption of chemicals with varing concentration?

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pH/ Acids and alkalis

The rationale for chosing this topic is that it can be applied to everyday life, ie. Household items and food and the pH of them. For example, the ‘pH of tothpaste is approximately 9 and the pH of lemon juice is approximately 2.0’_{3. (ThoughtCo, 2018)}. The dangers of these household items can be quite severe used in large volumes, however when used in small volumes items such as lemon juice are not very harmful.

Acids

Acids are aqueous or gaseous substances that ‘Dissociate’ separate into simpler substances/atoms or molecules. An example of this is hydrogen chloride, which is a gas that has a ‘Covalent Structure’, this gas dissolves in water and forms hydrogen⁺ and chlorine^– ions. The equation for this would be:

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‘HCl_(g) + H₂O —- > H⁺_(aq) + Cl^–_(aq)’

Hydrogen chloride gas + Water —- > Hydrogen⁺ ions + Chlorine^– ions.

_{(RSC.org, 2018)}

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Hydrgoen was discovered to be an unstable element when it is alone and can simply be defined as a proton. In electrolysis reactions hydrogen ions combine with ‘Polar water molecules’ which in turn will then form stable ions called ‘oxonium ions’. An equation to show this is:

‘H⁺_(aq) + H₂O_(l) —- > H₃O⁺_(aq)

Hydrogen + Water —- > Hydronium _{(RSC.org, 2018)}

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In addition, when hydrogen chloride as an aqueous solution is further dissolved in a volume of water, scientists have speculated that there is a chemical reaction taking place. The equation for the process is:

HCl_(aq) + H₂O_(l) —- > H₃O⁺_(aq) + Cl^–_(aq)

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Hydrogen chloride + Water —- > Hydronium + Chlorine _{(RSC.org, 2018)}

The definition of an acid is: ‘A compound containing hydrogen that dissociates in water to form hydrogen ions’ _{(Annets et al., 2017).}

Other common acids also react the same way, they dissociate and separate into simpler substances/ atoms or molcules, the amount they dissociate can vary from greater to lesser, but in water they all form oxonium ions. Therefore, this information explains why acids only portray their acidic properties when they have been diluted into a volume of water. _{(RSC.org, 2018).}

 Acids are substances that: form hydrogen gas when reacted with metals, neturalise bases and produce salt and water, and they release carbon dioxide if they are reacted with ‘Carbonates’. _{(RSC.org, 2018).}

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‘Acids provide H⁺ ions in a solution’. Acids can therefore be defined or described as ‘proton donors’. From this the assumption can be made that alkalis are ‘proton acceptors’ as they are chemical opposites to acids. _{(RSC.org, 2018).}

Acid dissociation constant

The rate at which an acid dissociates varies with different acids. For example this could mean that more of the acidic molecules produce H⁺ ions and fhs ‘equilibrium position is further to the right’. An equation to show this for a general acid with the formula HA:

By following ‘Le Chatelier’s principle’, by adding more water to the acid , the ionisation of the acid will increase.

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Therefore the ‘acid dissociation constant’ can be shown as this:

However, the concentration of the water being used is unlikely to vary very much as water is a neutral liquid, often around pH 7. Therefore, by taking this into consideration, the water constant is ‘incorperated’ into Kc, which can be shown in this equation:

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The values of

In this equation K can be defined as the ‘acid dissociation consatnt’

The ‘greater the degree of ionisation’ that is found, the stronger the acid will be. Therefore the value of K₂ will increase.

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When acids have the same concentration, the ‘greater the degree of ionisation’ of the acid being used, the more ions that are present in that acid. Therefore this will mean that the conductivity of the acid is higher. _{(RSC.org, 2018)}

Some examples of acid dissociated constants are:

The reason that the value of K_a for trichloroethanoic acid is 10,000 times bigger than the value of K_a for ethanoic acid is because chlorine is an ‘electronegative atom’, this means that electrons are attracted to the chlorine nucleus. This weakens the O-H bond as the hydrogen ions are much easier to form. The more hydrogen ions found in a solution, the stronger the acidity of the solution.

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Some examples of strong acids are sulfuric acid and nitric acids, these are common inorganic acids and they have high values of K_a as they acids are ‘fully ionised in a dilute solution’. _{(RSC.org, 2018)}

pK_a = -log K_{a (RSC.org, 2018)}       OR pK_a = -log K_{a (Chemguide.co.uk, 2018)}

The smaller the calculated or written value of pK_a , the sronger the acidity of a solution._{(RSC.org, 2018)}

K_a has the units of: (mol dm^-3) whereas, pK_a does not have any units. _{(Chemguide.co.uk, 2018)}

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pK_a is often used as it is easier to identify trends and patterns than using the K_a. _{(Chemguide.co.uk, 2018)}

Examples of strong and weak acids:

Hydrochloric acid is a strong acid as in a dilute solution it is completely dissociated. An equation for this is:

HCl_(aq) —- > H⁺_(aq) + Cl^–_(aq)

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Hydrochloric acid —- > Hydrogen + chlorine

However, in comparison both phenol and ethanoic acid can be described as weak acids as they never ‘completely ionised’ and therefore the dilution of the solution does not matter. Equations for both of these weak acids:

Phenol: C₆H₅H_(aq) —- > C₆H₅O^–_(aq) + H⁺_(aq)

Ethanoic acid: CH₃COOH_(aq) —- >CH₃COO^–_(aq) + H⁺_(aq)

There are many weak acids which are produced and occur naturally and therefore their origin is organic, such as:

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• Methanoic acid- This is found in the string of an ant. This chemical was originally called formic acid.
• Ethanoic acid- This acid has a very strong smell. This chemical was originally called acetic acid.
• Butanoic acid- This acid off a smell of ‘rancid’ dairy products such as butter and cheese.

Strong acids are acids which are fully dissociated into simpler ions in a dilute solution.

Concentrated acids contain ‘serveral moles of substance’ for each dm³ of solution. For example, ‘ordinary lab’ hydrochloric acid has ‘approximately 10 mol dm^-3 of HCl_(aq). Another example is sulfuric acid which has approximately 18 mol dm^-3 of aqueous H₂SO₄. _{(RSC.org, 2018)}

Alkalis

Alkalis have a pH of 7-14, the higher the pH the stronger the alkalinity is of the solution. Weak alkalis, also referred to as soluble bases, such as ammonia have a pH of 10-11. However, strong alkalis, which are also referred to as soluble bases, such as sodium hydroxide have a pH of 13- 14. These pH levels show as blue/purple colours in solutions when using universal indicator. _{(Docbrown.info.,2018)}

Alkalis form hydroxide ions (OH^–_(aq)) in water. Such as:

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• Sodium hydroxide (NaOH) forms Na⁺_(aq) and OH^–_(aq) ions.
• Calcium hydroxide Ca(OH)₂ forms Ca²⁺_(aq) and 2OH^–_(aq) ions.

‘An alkali is a base which is soluble in water’. _{(Docbrown.info.,2018)}

Ionic theory of acids and alkalis

Liquid water consists of ‘covalent H₂O moleucles’, it also contains small quantities of H⁺ and OH^– ions from the ‘self-ionistion of water’. However, these ions are of equal concentration therefore, this makes the water neutral.

Acidic solutions contain more H⁺ ions than OH^– ions. Alkalis are the opposite to acids, therefore alkali solutions contain more OH^– than H⁺ ions. _{(Docbrown.info.,2018)}

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When acids and alkalis react the molecular formula equation is often for neutralisation:

Acid+ Alkali —- > Salt + Water         Examples:

• HCl_(aq) + NaOH_(aq) —- > NaCl_(aq) + H₂O_(l)

Hydrochloric acid + Sodium hydroxide —- > sodium chloride + water

However, the ionic equation for neutralisation reacts is:

Hydrogen ion + Hydroxide ion —- > water          Which can be shown as:

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H⁺_(aq) + OH^–_(aq) —- > H₂O_(l)

This is because all when acids and water are reacted together it produces hydrogen ions. And when alkalis (soluble bases) and water are reacted together they produce hydroxide ions. Therefore, the remaining ions i.e. Na⁺_(aq) and Cl^–_(aq) become salt crystals i.e. NaCl_(s) when the salt ions evapourate from the water. _{(Docbrown.info.,2018)}

‘Bases are substances which react and therefore neutralise acids to produce salts and water.’

Some bases are not soluble in water, examples of this include:

• CuO- Copper (II) Oxide
• MgO- Magnesium Oxide

After a neutralisation reaction, the ‘salt solutions consist of a combination of both positive and negative ions’. _{(Docbrown.info.,2018)}

Brownsted-Lowry Theory

In this theory a ‘Brownstead-Lowry acid’ can be referred to as a ‘proton donor’. And as alkalis are the opposite, a ‘Brownstead-Lowry alkali’ can be referred to as a ‘proton acceptor’.

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Water is a neutral oxifde as it has a pH of 7, however it is an ‘amphoteric oxide ’ as it accepts and donates protons.

If water acts like a base, a proton acceptor, ‘ reacted with a stronger acid such as the hydrogen chloride gas’, the equation for this is:

HCl(g) + H2O(l) —- > H3O+(aq) + Cl-(aq)

Hydrogen chloride gas + water —- > hydronium + chlorine

If water acts as an acid, a proton donator, reacted with a ‘weal but stronger base such as the alkaline gas ammonia’, the equation for this is:

NH3(aq) + H2O(l)  NH4+(aq) + OH-(aq) _{(Docbrown.info.,2018)}

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Indicators

‘Indicators are coloured dyestuffs’

There are many types of indicator such as: universal indicator, bromothylmol blue, methyl orange and phenolphthalein. _{(RSC.org, 2018)}

In acids each indicator reacts differently:

• Universal indicator- red/pink
• Bromothylmol blue- yellow
• Methyl orange- red
• Phenolpthalein- colourless

In alaklis each indicator reacts differently once again, for example:

• Universal indicator- purple
• Bromothylmol blue- blue
• Methyl orange- yellow
• Phenolpthalein- pink

Universal indicator is also referred to as a ‘rainbow indicator’ or ‘mixed indicator’ as it as a combination of the single chemical indicators. Universal indicator is often used to find the pH of chemicals and a colour sheet or chart is used to match the colours. Some examples of different substances and the colour they are when universal indicator is added are: _{(RSC.org, 2018)}

• Dilute hydrochloric acid- Red
• Boric acid solution- Yellow
• Tap/Drinking water- Green
• Sodium bicarbonate solution- Blue
• Sodium hydroxide solution- Purple

A comparison table to show the different indicators and the colour they change a chemical to, dependant on its pH.

_{(RSC.org, 2018)}