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How many naphthalene molecules does a naphthalene C10H8 mothball that has a mass of 1 gram contain?
To determine the number of naphthalene molecules in a 1-gram naphthalene mothball, you would first calculate the number of moles of naphthalene using its molar mass (C10H8) and then use Avogadro's number to convert moles to molecules. Given that naphthalene's molar mass is 128.17 g/mol, you would find that there are approximately 6.022 x 10^21 molecules in a 1-gram naphthalene mothball.
What solvent would you use to measure the density of naphthalene acid?
To measure the density of naphthalene acid, a suitable solvent would be a non-polar solvent such as toluene or hexane. These solvents can dissolve naphthalene acid effectively without interfering with its properties. Additionally, using a non-polar solvent helps prevent any potential reactions or solubility issues that might arise with polar solvents. Ensure that the solvent does not alter the measurement accuracy of the density.
Would salt be more soluble in polar solvents?
Yes, salt is more soluble in polar solvents because salt is an ionic compound that dissolves well in substances with opposite charges, such as polar solvents. The positive and negative ions in salt are attracted to the partial charges in polar solvents, allowing for better solubility.
Would glycerol be soluble in polar or non polar solvents?
Glycerol is soluble in polar solvents due to its three hydroxyl (-OH) groups, which can form hydrogen bonds with water and other polar substances. This makes glycerol highly hydrophilic (water-attracting) and allows it to dissolve well in polar solvents. In contrast, glycerol is not soluble in non-polar solvents, as these do not provide the necessary interactions for dissolution.
What is the empirical formula of azulene?
It has a molecular formula of C10H8 so that would make an empirical formula of C5H4.
In which of these solvents would naphthalene C10H8 be most soluble?
Naphthalene would be most soluble in non-polar solvents such as benzene or hexane because it is a non-polar molecule. Polar solvents like water would not dissolve naphthalene well due to the lack of strong intermolecular interactions between the polar water molecules and the non-polar naphthalene molecules.
What would be a good solvent at room temperature for naphthalene C10H8 Water ethanol or pentane?
Pentane would be a good solvent at room temperature for naphthalene (C10H8) as it is non-polar and can dissolve non-polar compounds like naphthalene effectively. Water and ethanol are polar solvents and would not dissolve naphthalene well.
How many naphthalene molecules does a naphthalene C10H8 mothball that has a mass of 1 gram contain?
To determine the number of naphthalene molecules in a 1-gram naphthalene mothball, you would first calculate the number of moles of naphthalene using its molar mass (C10H8) and then use Avogadro's number to convert moles to molecules. Given that naphthalene's molar mass is 128.17 g/mol, you would find that there are approximately 6.022 x 10^21 molecules in a 1-gram naphthalene mothball.
What solvent would you use to measure the density of naphthalene acid?
To measure the density of naphthalene acid, a suitable solvent would be a non-polar solvent such as toluene or hexane. These solvents can dissolve naphthalene acid effectively without interfering with its properties. Additionally, using a non-polar solvent helps prevent any potential reactions or solubility issues that might arise with polar solvents. Ensure that the solvent does not alter the measurement accuracy of the density.
What solvent would carbon tetrachloride be more soluble?
Carbon tetrachloride is more soluble in non-polar solvents such as chloroform or carbon disulfide due to its non-polar nature. These solvents have similar chemical properties that allow for greater solubility of carbon tetrachloride compared to polar solvents.
Would salt be more soluble in polar solvents?
Yes, salt is more soluble in polar solvents because salt is an ionic compound that dissolves well in substances with opposite charges, such as polar solvents. The positive and negative ions in salt are attracted to the partial charges in polar solvents, allowing for better solubility.
Would glycerol be soluble in polar or non polar solvents?
Glycerol is soluble in polar solvents due to its three hydroxyl (-OH) groups, which can form hydrogen bonds with water and other polar substances. This makes glycerol highly hydrophilic (water-attracting) and allows it to dissolve well in polar solvents. In contrast, glycerol is not soluble in non-polar solvents, as these do not provide the necessary interactions for dissolution.
In which solvent 1-3 DiChloro-2Propanol is not soluble?
It is soluble in water, as would be expected (the molecule has a dipole moment), so I would guess that it would be poorly soluble in nonpolar solvents such as hexane or carbon tetrachloride. This is just a guess though...
What is the empirical formula of azulene?
It has a molecular formula of C10H8 so that would make an empirical formula of C5H4.
Which pigment was LEAST soluble in the organic solvent?
To determine which pigment was least soluble in an organic solvent, one would typically refer to a chromatography experiment where pigments are separated based on their solubility. Generally, more polar pigments tend to be less soluble in organic solvents compared to nonpolar ones. For example, chlorophyll a and b are usually more soluble than carotenoids in organic solvents, suggesting that carotenoids might be the least soluble. Without specific data, it's difficult to identify the exact pigment, but typically, the more polar compounds are less soluble in nonpolar organic solvents.
What is the study of fat?
the study of fat would fall under the category of biochemistry because fats are generally soluble in organic solvents
Is iron soluble in alcohol?
Iron is not soluble in alcohol. Iron is a metallic element that does not dissolve in alcohol, which is a polar solvent. If you need to dissolve iron in a solution, you would typically use an acid or other specialized solvents.
