Iodic Acid Formula

Names of acids are given from their anion and therefore the ion attached to the hydrogen. Iodic Acid may be a compound. It’s a white water-soluble solid. It features iodine within the oxidation number +5. And it’s one among the foremost stable oxo-acids of the halogens. Two classes of iodic acids are available. Its robustness contrasts with the instability of acid and acid. During this chapter, students will undergo a study of iodic acid formula, its preparation, and various properties.

Iodic Acid Formula

The molar mass of iodic acid is 175.91 g/mol. Its density is 4.62 g/cm³. When acid heated, samples dehydrate to provide iodine. On further heating, the iodine further decomposes. And it gives a mixture of iodine, oxygen and lower oxides of it. Its conjugate base is iodate. And therefore the melting of acid is 110 °C. The utilization of acid is often to synthesize sodium or potassium iodate for increasing the iodine content of salt. The solubility in water of it is 269 g/100 mL (20 °C).

• Molecular Formula = HIO₃
• The Simplified molecular-input line-entry system (SMILES) = OI(=O)=O

The use of it is in cleaning and washing. It also includes cleaning products utilized in the house, laundry detergents, soaps, de-greasers, spot removers, etc. It’s also utilized in modifiers like drycleaning, laundry, soap, window/floor, etc. Also, it’s utilized in industrial manufacturing, manufacturing food and Pesticide. The property value of hydrogen bond donor and hydrogen bond acceptor are 1 and 3 respectively.

Preparation of Iodic Acid

Production of acid with oxidizing iodine I2 with strong oxidizers like aqua fortis HNO3, chlorine Cl2, chloric acid HClO3 or peroxide H2O2. Reactions are as follows:

• I₂ + 6 H₂O + 5 Cl₂ ⇌ 2 HIO₃ + 10 HCl
• 3I₂ + 10 HNO₃ ⇌ 6 HIO₃ + 10 NO + 2 H₂O
• I₂ + HClO₃ ⇌ HIO₃ + NO + H₂O
• I₂ + H₂O₂ ⇌ 2 HIO₃ + NO + H₂O

Another method for the preparation of it is by treating hypoiodous acid with a base: 3HIO + 2OH¯ → HIO3+ 2H₂O + I¯

Properties of Iodic Acid

The reduction of it forms several things. Reduction to it occurs when there’s plenty of reducers. If there’s plenty of iodic acids, reduction to iodine occurs. Within the case of tons of chlorides, reduction to iodine occurs and it’s a yellow liquid. It may be a relatively strong acid with a pKa of 0.75. It’s strongly oxidizing in acidic solution, less so in basic solution. When acid acts as an oxidizer, then the merchandise of the reaction is either iodine or iodide ion.

Under some special conditions, it is reduced to iodine trichloride. It’s a golden yellow compound in solution and no further reduction occurs. Within the absence of chloride ions, when there’s an excess amount of reductant, then all iodate is converted to iodide ion. When there’s an excess amount of iodate, then a part of the iodate is converted to iodine. It should be utilized in the preparation of ionization to make alkyl halides.

For purification, dissolve acid within the minimum volume of hot dilute HNO₃, filter and evaporate during a vacuum until crystals are formed. And then we collect the crystals and wash them with a touch cold H₂O and dry them in the air within the dark

Solved Examples for Iodic Acid Formula

Q] Name iodine oxides with their formula and oxidation states.

Solution: Their formulas are,

Iodide = HI ( -1 Oxidation state)

Hypoiodous acid =HIO (+1 Oxidation state)

Iodous acid = HIO2 (+3 Oxidation state)

Periodic acid = HIO₄ or H₅IO6 (+7 Oxidation state)