It's not necessary for a substance to change it's normality as it is volume and mass dependent. Until and unless any external substances are added to a solution, it's unlikely for the solution to change it's normality/molarity.

The solution containing 1/10 (one tenth) of one gram equivalent weight of substance dissolved in 1 litre of volume is called decinormal solution. It is represented as N/10 or 0.1N .

The requisites for a substance to be a primary solution are:

• It should be in available in pure state ,
• Its composition should be constant during storage and weighing,
• It should be readily soluble in water and not be decomposed by water,
• It should have high equivalent weight and should not be hygroscopic or deliquescent.

An example of redox titration is titration of oxalic acid solution against KMno₄solution in acidic medium.

It is called so because ,during titration ,oxidation occur on one of the species and reduction on the other species, making it redox reaction and thus redox titration.

Solution:

Molecular weight of oxalic acid= 126

Equivalent weight of oxalic acid =63

Volume of solution to be prepared ,V =250ml

Conc.of solution to be prepared, N=0.1N

Now ,

We have

Mass of oxalic acid (g)=Equivalent weight volume normality 1000

= 632500.11000

1.575g

solution:

volume v₁= 50ml

concentration n₁= 0.5N

volume v₂=?

concentration n₂=o.1N

Now we have

molar equivalent of seminormal solution= molar equivalent of deci normal solution

or, 0.5* 50= 0.1*v

or, 250= v

Thus, volume of water should be added=250-50 =200 ml

The main difference between equivalence and endpoint is thatthe equivalence point is a point where the chemical reaction comes to an end while the endpoint is the point where the colour change occurs in a system.

oxalic acid is taken as primary standard solution because it is highly stable as it is weak acid and can be obtained in pure form. also because it is non-hygroscopic, non- deliquescent and hass high molecular mass which leads to less error and highly precise data can be observed.

Deci- Normal solution ---->The solution containing 1/10 mole of solute in 1 liter of solution is called normal solution.

Deci-molar solution(M10):The solution containing 110 th mole of solute in 1 liter of solution is known as decinormal solution.

Normality	Molarity
1. It is the number of gram equivalents of solute dissolved per litre solution.	1. It is the number of gram molecules of solute dissolved per litre its solution.
2. In general, Normality(N) = (g/L)/eq. wt	2. Molarity(M) = (w*1000)/(v* mol. wt)

Normality = Molarity x n

here N is acidity for base and basicity for acid.

so Normality = 2 x 3

since H3PO4 has 3 displaceable hydrogen.

Normality = 6 N

equivalent weight is the weight of a substance especially in grams that combines with or is chemically equivalentto eight grams of oxygen or one gram of hydrogen.

The number of moles of a solute dissolved in 1 L (1000 ml) of the solutionis known as the molarity of the solution.

we know,

Molarity * mol. wt = %(w/v) * 10

Molarity = 93*10/98 ==> 9.489

No, they are not. A primary standard is a reagent that is extremely pure,stable,has no waters of hydration and has high molecular weight.Lots of standard solutions are only secondary standard solutions because their concentration changes with time or because it is impossible to produce the exact concentration.

solution:let, the amount of Na2Co3 in the mixture = x gmNaHCo3 present in mixture = (1-x) gmMolar mass of Na2Co3 = 2*23+12+3*16 = 106 gm/molesimilarly, molar mass of NaHCo3 = 84 gm/moletherefore, moles of Na2Co3 in x gm = x/106 and moles of NaHCo3 in (1-x) gm = (1-x)/84According to the question,x/106 = (1-x)/84 so, x = 0.558gmThus the number of moles of Na2Co3 and NaHCo3 are 0.00526 moleAgain by reaction,


Na2CO3+2HCl2NaCl+H2O+CO2

Na2CO3+2HCl2NaCl+H2O+CO2
NaHCO3+HClNaCl+H2O+CO21 mole ofNa2CO3
...

In titration, normality factor is the ratio of the amount of substance taken to the amount of substance to be taken to prepare a standard solution.

It is also taken as the ratio of experimental weight to the theoretical weight of the amount of substance with respect to preparation of solution.

Titration error is defined as the difference between the measured endpoint and equivalence point of the titration

The acidity of base is the number of monobasic acid(s), required to neutralize one molecule of the base.

In other words, it is the number of replaceable OH group(s) present in the base.

The process of determination of the strength of acids by carrying out neutralization titration with standard alkali is called acidimetry.