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Buffer solution cannot cope with excessive addition of base or acid

How buffer mantains the body pH. It makes use of the equilibrium rule, more specifically Le chatelier’s principle.

I learnt about solubility product and also Ksp. When Ksp is high, the more soluble the salt is but it will still be sparingly soluble. When Ksp is low, the lower the solubility is also.

I learnt about the common ion effect and how to predict preciptation. If the concentration value is lower than the (solubility product)Ksp, it will not have any precipitate but if it is higher then there will be precipitate.

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I learnt the Brønsted-Lowry Theory where acids are proton donors bases are proton acceptors.

Kw (Ionic Product of Water)  at 298K = 1x10-14 mol2dm-6

pH  can be calculated using− log10 [H+] or pH + pOH = 14

Ka (acid dissociation constant) = [H+]^2 / [HA]

pKa used for weak acids, more pKa means less Ka means weaker acid

I also learnt the acid-base graphs and buffer solution. theacid bas graphs are used to determine the equivalent point and end point and the buffer solution is a solution where pH does not change significantly when small amounts of acid or base are added.

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•Buffer Solution is a solution in which pH doesnt change significantly when a small amount of acid or alkalis are added (used to keep pH constant)

•Two types of buffer sloution: acid buffer solution and base buffer solution

• if it is acid, use weak acid + the salt of the weak acid

• if base is used, use weak base + salt of the weak base

1. Formula to find pH

2. solubility product constant-> product of concentration of each ion

3. If the concentration value is bigger than solubility product then precipitate will form

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Reviewed about buffer solutions how it works and its reaction and formulae we also revised on the applications and how to calculate the ph lastly we leaarnt about KPC and KSP

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Buffer Solution:
- A solution in which the pH does not change even if small amounts of acid or alkali are added (Will not work if large amounts are added)
- a mixture of weak acid/base and its salts

Ksp:
- Used to predict the formation of a precipitate
- Greater Ksp, more soluble
- Smaller Ksp, less soluble
- Only for sparingly soluble salts
- If the Ksp value is greater than the standard value, a precipitate will form

I need to understand the concepts better

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i learnt about buffer solutions, and ksp

buffer solutions maintain ph of solution even when small amounts of acid or base is added. It does not work on large amounts. It is a mix of weak acid and its salt or using a base and its salt.

ksp is the product of concentration of ions in a saturated solution of sparingly soluble salt under standard conditions. ionic concentration is raised to the power of their relative concentrations (coefficient?). If Ksp is higher than the solubility product, that means ppt will form.

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I learnt about the Buffer Solution, which is :

a solution in which pH does not change when small amounts of acid or alkali is added

used to make the pH constant

a mixture of weak acid/base and its salt

Furthermore, i learnt how to calculate the solubility of a product. Ksp, is called the solubility product, which is the product of the concentrations of each ion in a saturated solution of sparingly soluble salt. Overall, the lesson was not too hard to understand

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buffer solution
- solution in which pH doesn’t change
- even when small amounts of acids or alkalis are added
- 1 type is a mixture of weak acid & its salts
- pH depends on ratio of concentration of acid to the concentration of its conjugate base

calculations
- [H+] = Ka x ([acid]/[base])
- pH = pKa + lg([acid]/[base])

solubility product
- product of concentration of each ion in a saturated solution of a sparingly soluble salt a5 298K, raised to the power of their relative concentrations
- Ksp = [C^y+ (aq)]^a [A^x- (aq]^b
- can be used to predict precipitation
- if Ksp is higher than solubility product, ppt will form

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I learned that a buffer solution is used to keep the pH constant when a small amount of acid and alkali is added and is made up of a weak acid and its salt, or a weak base and its salt. It will not work if too much of a base or acid is added as there will be too many H+ or OH- ions in the solution. I also learned that Ksp is the product of concentrations of each ion in a saturated solution of a sparingly soluble salt at RTP, and a smaller value would mean it is less soluble, and that kpc is the equilibrium constant that connects the concentration of a solute partitioned between two immiscible solvents.

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Buffer Solution
- Maintains pH
- Works only if a small amount of acid/base is added
- Mixture of weak acid & salt OR Mixture of weak base & salt

Ksp
- Predict formation of precipitate
- Directly proportional to solubility
- Only for slightly soluble salts
- If Ksp becomes greater than standard value, will form a precipitate

I need to try remember everything correctly.

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Buffer solution

a solution in which pH doesn't change significantly when a small amount of acid or base is added

used to keep the pH constant

mixture of weak acid and its salt

mixture of weak base and its salt

Limitation of buffer solutions

pH will still change significantly if a large amount of acid/alkali is added

[H+] = Ka x [acid]/[salt]

pH = pKa + log ([salt]/[acid])

Ksp (solubility product):

product of the concentrations of each ion in a saturated solution

only for slightly soluble salts

smaller Ksp = less soluble

used to predict formation of precipitate

if value of Ksp becomes greater than the standard value, it will form a precipitate

I need to revise more on how to predict formation of precipitate, understand the concepts better and attempt past year questions. The lecture was clear and elaborate.

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New topic !!

Solubility product is only applicable to sparingly products (AgCl, Ca(OH)2)

Dissolving AgCl forms a reversible reaction between the solid AgCl and dissolved Ag+ and Cl- ions

Ksp = [Ag+][Cl-]

Solubility product = the product of the concentrations of each ion in a saturated solution of a sparingly soluble salt at 298K, raised to the power of their relative concentrations

The value of Ksp denotes the extent to which a salt is dissolved. Greater Ksp = more soluble, Smaller Ksp = less soluble

Ksp can be used to predict the formation of precipitates

If value of Ksp is greater than standard value of Ksp, a precipitate will be formed.  if value of Ksp is smaller than standard value, no precipitate is formed

Common ion effect = using LCP

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buffer solution
- pH stays relatively the same if small amounts of acids or alkalis are added
- maintains pH
- weak acid and salt of weak acid / weak base and salt of weak base
- large reserve of salt allows the change to be neglectable
- cannot cope with the addition of large amounts of acids or alkalis

pH of buffer solution
- use Ka to find [H+] and find pH from there
- pH = pKa + log [salt]/[acid]

maintaining body pH
- CO2 + H2O  <=>  H+ + HCO3-

Ksp
- solubility product
- used for sparingly soluble products ex. AgCl
- product of concentrations of each ion in a saturated solution of a sparingly soluble salt at 298K, raised to the power of their relative concentrations
- smaller Ksp = less soluble

predicting the formation of a ppt
- if value of solubility product calculated is greater than the given Ksp, then ppt will be formed

common ion effect
- addition of a substance with a common ion will cause the equilibrium to shift accordingly

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i learnt that:

buffer solution is used to make the pH constant

it is a mixture between a weak acid and its salts or a weak base and its salts

it is a solution where a pH does not change

excessive amounts of acid or alkalis will increase the pH significantly

i also learnt calculations regarding buffer solution and how buffer can maintain the body pH

using ksp to predict the formation of a precipitate

greater ksp = more precipitate

i also learnt about predicting solubility

overall the lesson was detailed and easy to understand

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Buffer Solution
- a solution in which pH does not change significantly when a small amount of acids or alkalis are added
- it is used to keep the pH constant
- mixture of a weak acid and its salt
- mixture of a weak base and its salt

Limitation of buffer solutions
- no buffer solution can cope with excessive addition of acids and alkalis, as the pH will change significantly when very large amounts of acid or alkali are added.

Moreover, I learnt
- how to calculate the pH of buffer solution
- buffer to maintain body pH ( HCO3- used to maintain body temperature )
- how to calculate the solubility of a product
- Ksp is the solubility product, so if smaller Ksp, lower solubility of salt and how to predict the formation of the precipitate by using Ksp.

The lecture was clear and concise, but I still need to revise more on this chapter to ensure that I understand everything.

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buffer solutions
- a solution in which pH does not change significantly when a small amount of acid / alkali is added
- used to keep the pH constant
- does not work if too much acid / alkali is used

there are 2 types:
- weak acid (CH3COOH) + salt weak acid (CH3COONa)
- weak base (NH3) + salt of weak base (NH3Cl)

Ksp
- to predict the formation of a precipitate
- the higher Ksp, solubility increase

common ion effect
- reduction in solubility of a dissolved salt when a solution of a compound that has an ion in common with the dissolved salt
- results in ppt.

I need to practice more questions related to this chapter. However, the teaching was clear and understandable.

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Buffer Solution

A solution in which the pH does not change significantly when small amounts of acids or alkalis are added

Keeps pH constant

Must be in large reserve supply

Any change (addition of H+ or OH-) is deemed to be negligible due to the relatively small amount

Ksp

Solubility product of the concentrations of each ion in a sparingly soluble salt solution

Kpc

Eq constant which relates the concentration of a solute partitioned between two immiscible solvents at a specific temperature.

Teaching was elaborate and informative. I would need to revise more on their applications.

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Learned about:
-Buffer solution [Solution in which the pH does not change that much when small amount of acids and alkali are added]Example: Weak base with its salt mixture
-Buffer solution is used to keep the pH constant
-Buffer solution wouldn't work if too much acid or base is added
-Ksp: solubility product (product concentration of each ion)
-Predicting the precipitate formation using Ksp

The lecture was easy to understand and I was able to understand it.

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On lecture 14, i have learnt further about Buffer Solution, Ksp.

Before that, i have reviewed upon Kw and Kc and the two assumptions for Ka. (how much the acid is dissociated.) (Low Ka = weaker acid)

I learnt that buffer solution is a solution which pH does not change significantly when a small amount of acids and alkalis are added. It is a mixture of weak acid and its salts / weak base and its salts.

I also reviewed on some questions regarding buffer solution and how buffer can maintain body pH.

Then, i learnt about Solubility Product (Agcl for example) and reviewed some sample questions.

Lastly, I was also introduced to common ion effect and Kpc.

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We learnt about buffer solution which is a solution which doesn't experience a lot of pH change when acid or base is added. We also revised on Kw, Ka and the formula to find pH.

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uhm a bit busy rn study for mock test so this isnt very complete

review about
- equations
- assumptions needed to be made
study bout
- weak/strong acid/base as buffer solution
- limitations
- calculating ph of buffer solution
- predicting solubility

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-Learnt about buffer solution(Weak acid/base and salt)

-Buffer solution is used in keeping the pH constant

-Buffer solution does not work if too much acid/alkali is added

-Learnt about Ksp (Used to determine solubility)

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-- review all the formulas
-- Buffer solution

Solution in which pH does not change (significantly) when a small amount of acids or alkalis are added

To keep pH constant

Example of buffer solution

Weak base and its salts (mixture) = ammonia and ammonium chloride

Weak acid and its salts (mixture) = ethanoic acid and sodium ethanoate

How buffer solution works

CH3COOH →(reversible) CH3COO- + H+

CH3COONa →(reversible) CH3COO- + Na+

When adding H+

Addition of H+ ions shifts the position of equilibrium to the left

H+ ions combine with CH3COO- ions to form more CH3COOH

Large amount of CH3COO- ensures the concentration of CH3COOH molecules in solution does not change significantly

Large amount of CH3COOH ensures that the concentration of CH3COOH molecules in solution does not change significantly

pH does not change significantly

No buffer solution can cope with excessive addition of acids or alkalis. If very large amount of acids or alkalis are added, pH will change

Ksp = solubility product (product conc. of each ion)

prediction of the formation of precipitate by the use of Ksp

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Learnt what is buffer solution
What is its function
Calculate pH of buffer solution
Its property

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Recall:
1) assumptions in using Ka constants
• We take the initial value of [HA] and assume that its dissociation is so small that it is negligible.
• The dissociatuon of water is negligible.

2) Acid dissociation constant: >Ka, better weak acid, <Ka, weak acid

Buffer solution: a solution that resists changes in pH when small quantities of an acid or an alkali are added to it (apple thief analogy)

*No buffer solutions can cope with excessive additions of acids or alkali.

Watch videos on partition coefficient.

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Buffer solution
- Is a mixture of 2 components that will keep the pH constant.
- The acid buffer is a mixture of weak acid and its salt.
- The base buffer is a mixture of weak base and its salt.
- Must always refer to equation that has reversible reaction.
- Solubility product is the product of the concentrations of each ion in a saturated solution of a sparingly soluble salt at 298k, raised to the power of their relative concentrations.
- The higher the Ksp, the more soluble.

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Buffer solutions
- A solution where pH does not change significantly
- To keep pH constant
- Weak acid + salt of weak acid
- Weak base + salt of weak base
- Will not work if put too much acid / base
- Ksp = solubility product

Practice textbook ques

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Buffer Solution : mixture of weak acid/base + its salt. It is a solution that can maintain its pH if small amount of acid/base are added.
pH = pKa + log[salt/acid]
Solubility of product, Ksp : the product concentration of each ion. Predicting whether a precipitate will form or not, formed if > Ksp

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From this lecture, I learnt about

buffer solution: a solution in which pH does not change significantly when a small amount of acids or alkalis are added. pH will change if excessive acids or alkalis is added. Buffer solution is also used to maintain body pH.

buffer solution 1) weak acid + salt of the weak acid 2) weak base + salt of the weak base.

how to calculate for pH of buffer solution, pH = pKa + log10([salt]/[acid]). Assumption: [A-] from the dissociation of HA is too small/negligible. [A-] is from the salt KA.

solubility product, Ksp: the product of the concentration of each ion.

how to predict whether or not a precipitate will be formed, >Ksp ppt formed.

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Revised on Kw, Ka, pH and calculations

> buffer solutions only work with small pH changes

>how buffer solution works

>calculation of buffer solution pH (pH=pKa  + log [salt ion]/[acid])

>Ksp and solubility

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Revised on Kw, Ka and its formulas
-Learn about buffer solution and its limitation
-Two types of buffer solution which are weak acid and its salt and weak base and its salts
-How to calculate the pH
-Buffer to maintain body pH (could cause comatose if production of H+ ions left unchecked)
-Solubility of products: its definition and formula
-Predicting solubility use LCP and if the solubility is higher then a precipitate will, if the solubility is lower then more ions will be found in the solution

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Revised on:
- Kw, Ka, and how to find and use them to calculate pH.

- Buffer solutions and how they work. (Reversible reactions to counter small increase or decrease of pH)

Learnt:
- Applications of buffer solutions.

- How to calculate pH of buffer solutions. (pH = pKa + log( [salt ions] / [acid] )

- Ksa and how to calculate it (Ksa = [ions])

- Trends and how to predict Ksa (Ksa is used for sparingly soluble salts, higher Ksa means more soluble)

- Common ion effect (If another salt with an ion that is the same as the ions in the solution is added, precipitate may form. Determine by getting the conc. of the ions. If greater than Ksp, precipitate is formed.)

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- The video reviewed the past equations that we had already revised before ++ the assumptions we take in calculations.
- Also, reviewed acid-base, weak-strong combinations and a brief explanation on their graphs
- Also learnt about how buffer solutions work with weak acids and salts of weak acids, as the salt of weak acids can acts as a reserve of the ions in order for the equilibrium of the equation in which the weak acids dissociate in, to have enough of the weak ions in order for the POE of the equilibrium equation to shift to the left, or to make the amt of weak acid ion produced when OH- is added (POE shifts to the right) seem insignificant, so not much pH change.
- Limitations of Buffer Solutions, how it cannot cope with excess hydrogen/hydroxide ions
- Buffer solutions formed with bases work more or less the same way as acidic buffer solutions, just this time in the other way bc it produces hydroxide ions instead of hydrogen ions).
- Calculating the pH of Buffer solutions:
pH = -log [H+]
[H+] = Ka x [acid]/[salt]
- log[H+] = -log [ Ka x [acid]/[salt] ]
pH = pKa - log( [acid] / [salt ] )
pH = pKa + log( [salt] / [acid ] )
* New assumption that the value of A from the acid is too small ++ the other two assumptions.

- Ksp is the solubility product, so if the smaller Kspis , lower solubility of salt

- also learnt how to predict the formation of the precipitate by using Ksp.

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Revised on Kw, Ka and its formulas

Learn about buffer solution and its limitation

How to calculate the pH

Buffer to maintain body pH (could cause comatose if production of H+ ions left unchecked)

Solubility of products: its definition and formula (only for sparingly soluble salts)

Smaller Ksp, lower solubility of salt

Predicting precipitate formation using Ksp

the lecture was clear but the last few topics were discussed too fast.

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Revised on :
- Kw
- Ka
- how to calculate pH
- what is buffer solution
- base buffer & acid buffer
- how buffer solutions work ( using equations )

Learnt about :
- how the pH in the human body is maintained by buffers ( carbonic anhydrase as catalyst )
- calculating pH of buffer solutions ( pH = pKa + log10 ( [salt] / [acid] )
- solubility product ( for sparingly soluble salts only )
- calculation examples for solubility product
- predicting ppt ( if greater than Ksp, ppt forms. if lesser than Ksp, ppt not formed )

Need to revise more on :
- predicting ppt.
- calculating pH of buffer solution

Teaching :
detailed and clear, but the ending was a bit rushed

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Buffer Solution :
- a solution in which pH does not change significantly when a small amount of acids or alkalis are added
- used to keep pH constant
- mixture of weak acid/base & its salts

Limitations : if very much alkali/acid added, pH will change

Calculating pH of buffer solution
pH = pKa + log10([salt]/[acid])
Assumption : [A-] from dissociation of HA is negligible , [A-] from salt KA

HCO3- used to maintain body temperature

How to calculate solubility of product

How to predict if ppt will be formed (greater than Ksp)

Need to work more and revise more on how to calculate and memorise formulas

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Buffer solution is a mixture of 2 components that will keep the pH constant. Acid buffer is a mixture of weak acid and its salt. Base buffer is a mixture of weak base and its salt. Always refer to equation that has reversible reaction. Solubility product is the product of the concentrations of each ion in a saturated solution of a sparingly soluble salt at 298k, raised to the power of their relative concentrations. The higher the Ksp, the more soluble.

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What I learnt today :
-We revised on the equations of Kw, Ka, and pKa.
-We revised the assumptions made on Ka : initial conc. of [HA] is used and [H+] in water is ignored.
- The higher the Ka, the better the weak acid and the lower the pKa.
-The Ka formula is used only for weak acid.
-What does Ka tell : How much the acid is being dissociated.
Buffer solution
-A solution in which a pH does not change significantly when small amount of acid/alkalis are added.
- pH=pKa + log10 ([salt]/[acid])
Solubility Product
- Ksp
- It is the product of the concetrations of each ion in a sturated solution of a sparingly soluble salt at 298K, raised to the power of their relative conc.
-Only used for slightly soluble salt
-When calculating, remember to divide using the total volume of the substances, not just the individual.
-If the value is greater than the given Solubility Product, then precipitate will be formed. If it is lower, no precipitate is formed.

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Today I revised Kw, PH, Ka and PKa

Ka = [H+]^2/HA (Acid Dissocitaion Constant)
Assumptions have to made when using Ka.
- concentration of H+ in water will be ignored
- The initial concentration of HA will be taken even if there is
- If there is a salt, take the conentration of the A- form the salt instead of the HA
dissociation. This isbecause the dissocitaion in HA is very small
When Ka increases, it is a better weak acid
When PKa decreases, it is a better weak acid
Vice versa for both

Buffer Solutions
-A solution in which PH does not change significantly.
weak acid + salt weak acid
Ch3COOH <-> CH3COO- + H+
&
CH3COO+Na- -> CH3COO- + Na+

The weak acid will not dissociate completely by the salt will. This makes the CH3COO- ions in the weak acid very little evn though there is alot of mols of weak acid. This is so when there is a small increase or decraese of CH3COO- ions, there is almost no change as there is alot of CH3COO- ions from the salt of the waek acid.

weak vase + salt of weak base
NH3 + H20 <-> NH4+ + OH-
NH4Cl -> CH4+ + Cl-

Limitation of Buffer Solutions

No Buffer solution can cope with the excess addition of acids or alkili if very large amounts of acid are added.

Buffer to maintain body pH

CO2 + H20 <=> H+ + HC03-(hydrogencarbonate ion)
It is used to maintain the body pH at 7.35 or 7.45

SOLUBILITY PRODUCT

Ksp
An equilibrium is stablished when an undisolved iuonic compound is in contact with a saturated solution of its ions. The ions move from the solid to the saturated solution at the same rate as they move from the soltuion to the solid.
-It is sparingly soluble.

eg. Ksp = [Ag+]^n[Cl-]^n

The larger Ksp means that the compound is more soluble as more ions are there. But all are sparingly soluble meaning that precipitate will still be formed.

COMMON ION EFFECT

when the compound added has a similar ion as the product, the precipitate of the existing ion will increase as there is more of the product ion causing LCP to take effect.