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the charge in KMno4 is zero . it has no unpaired electrons but it is still dark in colored due to charge transfer in KMnO4. from Ayushi Sharma
Wiki User
∙ 12y ago
Wiki User
∙ 13y agoThe charge would be 2-
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But wouldn't you want to use KMnO4 as the example? In reality it is MnO4-1.
Wiki User
∙ 10y agoThe molar mass of potassium permanganate is 158,034.
Wiki User
∙ 12y agoThe question makes no sense. It's like asking how many buckets there are in water.
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How many moles of KMnO4 are present in 75.0 mL of a 0.0950 M solution?
Molarity = moles of solute/Liters of solution ( 75.0 ml = 0.075 Liters ) Algebraically manipulate, moles of solute = Liters of solution * Molarity Moles KMnO4 = (0.075 Liters)(0.0950 M) = 7.13 X 10 -3 moles KMnO4 ------------------------------------
How many moles are in 100g of KMnO4?
1 mol = 118.94 1 mol / 118.94 = 1.70 / x G = 202.10g
How do you find molar concentration of chemical compounds?
The Stoichiometry of molar concentration follows this simple formula: Mol = Volume (dm³) × Molar Concentration (mol/dm³) Hence: Molar Concentration (mol/dm³) = Number of moles (mol)/ Volume (dm³)
What is the molarity of 0.1 normal KMnO4?
The formula mass of KMnO4 is 158.0Amount of KMnO4 = mass of sample / molar mass = 100/158.0 = 0.633 molThere are 0.633 moles in 100g of potassium permanganate.
What is the mass of 2.55 mol of KMnO4?
Number of moles= Mass/molar mass (g/mol) Hence Mass= mol × molar mass Mol=2.55 Molar mass of KMnO4= 39+55+(16×4)= 158g/mol Where K=39, Mn=55 and O =16 Hence Mass of KMnO4 in 2.55 mols of the compound= 2.55×158= 402.9g.
How many moles of KMnO4 are present in 75.0 mL of a 0.0950 M solution?
Molarity = moles of solute/Liters of solution ( 75.0 ml = 0.075 Liters ) Algebraically manipulate, moles of solute = Liters of solution * Molarity Moles KMnO4 = (0.075 Liters)(0.0950 M) = 7.13 X 10 -3 moles KMnO4 ------------------------------------
How many grams of potassium permanganate are in 2.20 moles?
This mass is 347,67 for KMnO4.
How many moles are in 100g of KMnO4?
1 mol = 118.94 1 mol / 118.94 = 1.70 / x G = 202.10g
How many grams of potassium permanganate KMnO4 are in 2.55 moles?
The compound potassium permanganate has chemical formula KMnO4 Molecular mass of KMnO4 = 39.1 + 54.9 + 4(16.0) = 158.0 Mass of KMnO4 = amount of KMnO4 x Molecular mass of KMnO4 = 2.55 x 158.0 = 403g
Can you dissolve .35 moles of Potassium Permanganate (KMnO4) into 500 mL of water?
The solubility of potassium permanganate in water at 2o 0C is 64 g/l (or 32 g/0,5 L).The molar mass of KMnO4 is 158,034 g and 0,35 moles KMnO4 is equal to 55,312 g.So it is not possible to dissolve o,35 moles KMnO4 in 0,5 L.
How do you find molar concentration of chemical compounds?
The Stoichiometry of molar concentration follows this simple formula: Mol = Volume (dm³) × Molar Concentration (mol/dm³) Hence: Molar Concentration (mol/dm³) = Number of moles (mol)/ Volume (dm³)
What is the molarity of 0.1 normal KMnO4?
The formula mass of KMnO4 is 158.0Amount of KMnO4 = mass of sample / molar mass = 100/158.0 = 0.633 molThere are 0.633 moles in 100g of potassium permanganate.
What is the mass of 2.55 mol of KMnO4?
Number of moles= Mass/molar mass (g/mol) Hence Mass= mol × molar mass Mol=2.55 Molar mass of KMnO4= 39+55+(16×4)= 158g/mol Where K=39, Mn=55 and O =16 Hence Mass of KMnO4 in 2.55 mols of the compound= 2.55×158= 402.9g.
If you have 17.34 moles of potassium permanganate how many kilograms of the substance do you have?
Potassium permanganate = KMnO4 Molar mass of KMnO4 K = 1 * 39.10 g = 39.10 g Mn = 1 * 54.94 g = 54.94 g O = 4 * 16.00 g = 64.00 g Total = 158.04 g/mol 17.34 mol KMnO4 * (158.04 g/1 mol KMnO4) = 2740.41 g KMnO4 Convert the grams to kilograms. 1 kg = 1000 g 2740.41 g * (1 kg/1000 g) = 2.74041 kg Therefore, 17.34 moles of potassium permanganate is equal to about 2.74 kilograms.
Chemical symbol for permanganate?
The formula for potassium permanganate is KMnO4
What are kmno4?
acidicness number of kmno4
How many mols in 100g of KMnO4?
0.006327754
