Sulphuric Acid (H2SO4) is used in the redox titration process because it provides the H(+) ions necessary for the reaction to occur more quickly whilst the sulphate(-) ions barely react during the reaction. Therefore, sulfuric acid is added to make the solution acidic.

Potassium Permanganate is a flexible and potent oxidant which can be used by overt or indirect titration to classify many compounds. Since the function of the indicator is to detect endpoints, a separate indicator for permanganate titration is not needed. …

Potassium permanganate is a strong oxidising agent and in the presence of sulfuric acid it acts as a powerful oxidising agent. In acidic medium the oxidising ability of KMnO4 is represented by the following equation.

After complete consumption of oxalic acid ions, the end point is indicated by a pink colour due to excess of unreacted potassium permanganate (pink in colour). Potassium permanganate reacts with sulphuric acid and forms manganous sulphate which works as catalyst for reduction of MnO4- .

The acid used in this titration is dilute sulphuric acid. Nitric acid is not used as it is itself an oxidising agent and hydrochloric acid is usually avoided because it reacts with KMnO4 according to the equation given below to produce chlorine and chlorine which is also an oxidising agent in the aqueous solution.

Why do we take 0.02 N H2SO4 for the titration? We use sulfuric acid to provide hydrogen ions to the solution to acidify it. Also, the sulfate ion is a difficult ion to oxidize in usual redox titrations, so you do not normally get byproducts.

Normality

Normality Formula

1. Normality = Number of gram equivalents × [volume of solution in litres]-1
2. Number of gram equivalents = weight of solute × [Equivalent weight of solute]-1
3. N = Weight of Solute (gram) × [Equivalent weight × Volume (L)]
4. N = Molarity × Molar mass × [Equivalent mass]-1

0.02 N NaOH Add 0.80g sodium hydroxide (NaOH) pellets to 1000 mL deionized, degassed water. Mix gently to dissolve pellets. Cool to room temperature.

Making 1 N solution of NaOH To make 1 N solution, dissolve 40.00 g of sodium hydroxide in water to make volume 1 liter. For a 0.1 N solution (used for wine analysis) 4.00 g of NaOH per liter is needed.

Normality Calculation of NaOH To make a 1N solution of NaOH, 40 grams of NaOH are dissolved in 1 L. Likewise, for a 0.1 N solution of NaOH, divide by a factor of 10 and 4 grams of NaOH per liter is needed.

The normality of a solution is the gram equivalent weight of a solute per liter of solution. For example, the concentration of a hydrochloric acid solution might be expressed as 0.1 N HCl. A gram equivalent weight or equivalent is a measure of the reactive capacity of a given chemical species (ion, molecule, etc.).

13

pOH (The pH scale for bases) can be found by taking the negative logarithm of OH− concentration. pOH = −log[. 05M] = 1.3.

Hence, the pH of 0.1 M NaOH is 13.

10.0

Question: The pH of an aqueous 0.00100 M solution of NaOH is: 3 9 11 1 7 7.

pH = 5.91. Great, the salt is acidic and we got a logical answer. Good Luck.

5.6 x

-Therefore the pH of the ammonium chloride solution is 5.35. -So, the correct option is B.