PH=-log[H+]
pH=-log(1.4x10^-5)
pH=4.85
Answer:The metal complex formed would have the following formula [Cr(NO₂)₆]³⁻. The complex has a net negative charge and hence it can only be isolated as a salt with a positive cation so the formed complex could be isolated as potassium salt. The formula for salt would be K₃[Cr(NO₂)₆].
Explanation:
The metal ion given to us is Cr³⁺ (Chromium) in +3 oxidation state.
The electronic configuration for the metal ion is [Ar]3d³ so there are vacant 3d metal orbitals which are available and hence 6 NO₂⁻ ligands can easily attack the metal center and form a metal complex.
The charge on the overall complex can be calculated using the oxidation states of metal and ligand which is provided.
The (chromium ) Cr³⁺ metal has +3 charge and 6 NO₂⁻ (nitro) ligands have -6 charge and since the ligands will be providing a total of 6 - (negative) charge and hence only 3- (negative ) charge can be neutralized so a net 3- negative charge would be present on the overall complex which is basically present at the metal center :
charge on the complex=+3-6=-3
Let X be the Oxidation state of Cr in complex =[Cr(NO₂)₆]³⁻
X-6=-3
X=-3+6
X=+3
so our calculated oxidation state of Cr is +3 which matches with the provided in question.
As we can see that the overall metal complex has a net negative charge and hence and only positively charged cations can form a salt with this metal complex and hence only potassium K⁺ ions can form salt with the metal complex.
since overall charge present on the metal complex is -3 so 3 K⁺ ion would be needed to neutralize it and hence the formula of the metal salt would be K₃[Cr(NO₂)₆].
The increase in volume shift the equilibrium towards making more moles of gas, decrease in volume shift the equilibrium towards producing fewer moles of gas.
<h3>What is equilibrium?</h3>
The equilibrium of the gas is based on the pressure of the gas. With the increase in pressure, the equilibrium moves towards making fewer molecules of gas.
The gas equilibrium is proportional to the equilibrium K.
Increase in volume shift the equilibrium towards making more moles of gas, decrease in volume shift the equilibrium towards producing fewer moles of gas.
Learn more about equilibrium
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