The hybrid orbital of this molecule is 
. Hence, option C is correct.
<h3>What is hybridisation?</h3>
Hybridization is defined as the concept of mixing two atomic orbitals to give rise to a new type of hybridized orbitals.
In this compound, a hybrid orbital makes I-O bonds. Due to hybridization iodate should have tetrahedral geometry but because of the presence of lone pair of electrons the shape of 
the ion is pyramidal.
The hybrid orbital of this molecule is . Hence, option C is correct.
Learn more about hybridisation here:
brainly.com/question/23038117
#SPJ1
Answer:
1.12g/mol
Explanation:
The freezing point depression of a solvent for the addition of a solute follows the equation:
ΔT = Kf*m*i
<em>Where ΔT is change in temperature (Benzonitrile freezing point: -12.82°C; Freezing point solution: 13.4°C)</em>
<em>ΔT = 13.4°C - (-12.82) = 26.22°C</em>
<em>m is molality of the solution</em>
<em>Kf is freezing point depression constant of benzonitrile (5.35°Ckgmol⁻¹)</em>
<em>And i is Van't Hoff factor (1 for all solutes in benzonitrile)</em>
Replacing:
26.22°C = 5.35°Ckgmol⁻¹*m*1
4.90mol/kg = molality of the compound X
As the mass of the solvent is 100g = 0.100kg:
4.9mol/kg * 0.100kg = 0.490moles
There are 0.490 moles of X in 551mg = 0.551g, the molar mass (Ratio of grams and moles) is:
0.551g / 0.490mol
= 1.12g/mol
<em>This result has no sense but is the result by using the freezing point of the solution = 13.4°C. Has more sense a value of -13.4°C.</em>
Answer:
Hydrogen and Chlorine
Explanation:
They are both an example in univalent atoms, because of their nature to form only one single bond.
I wasn't able to find another example, hope it helped! :)
Answer:
Explanation is in the answer
Explanation:
The pH of the buffer solution does not change appreciably because the strong acid (free H⁺) reacts with conjugate base of buffer producing more weak acid. pH formula of buffers is (Henderson-Hasselbalch formula):
pH = pKa + log ( [A⁻] / [HA] )
The addition of strong acid decreases [A⁻] increasing [HA]. pH change just in the log of the ratio of [A⁻] with [HA], that is a real little effect over pH of the buffer solution.
