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If you meant #"g/mL"#, then it requires little effort. #"1 cm"^3# is known to be equivalent to #"1 mL"#, so you're done. If you meant #"mL"#, it's not the same units back, so it's not a proper conversion; you're inputting a density and getting back a volume. Regardless, you would do this:
It depends on the substance whose volume you know. > If you have a pure liquid or a solid, you use its density to calculate its mass and then divide the mass by the molar mass. If you have a solution, you multiply the molarity by the volume in litres. MOLES FROM VOLUME OF PURE LIQUID OR SOLID There are two steps: Multiply the volume by the density to get the mass. Divide the mass by the molar ...
This tells you that every #color(darkorange)("1 mL")# of aluminium has a mass of #color(blue)("2.70 g")#. All you have to do now is use the density of aluminium as a conversion factor to go from cubic centimenters of aluminium to grams
The density of gold is #19.3 g##/##cm^3#. What is the volume, in #cm^3#, of a sample of gold with mass #0.715# #kg#?
Which solution contains the biggest amount, in mol, of chloride ions? A. 20 cm3 of 0.50 mol dm−3 NH4Cl B. 60 cm3 of 0.20 mol dm−3 MgCl2 C. 70 cm3 of 0.30 mol dm−3 NaCl D. 100 cm3 of 0.30 mol dm−3 ClCH2COOH
A 15.00 mL solution of potassium nitrate (KNO3) was diluted to 125.0 mL, and 25.00 mL of this solution were then diluted to 1.000 x 10^3 mL. The concentration of the final solution is 0.00383 M. What is the molarity of the original solution?
8.23 * 10^(22) The idea here is that you need to use the density of water at 4^@"C" and the volume of the sample to find its mass, then use water's molar mass to find how many moles of water you get in this sample. So, density is defined as mass per unit of volume. In this case, a density of "`1.00 g/mL" tells you that every milliliter of water has a mass of "1.00 g". This means that "2.46 mL ...
color(purple)("The mercury metal has a mass of 48.3g." To calculate the mass of the object, we have to use the following formula: - Density will have units of g/(mL) when dealing with a liquid or units of g/(cm^3) when dealing with a solid. The mass has units of grams, g. The volume will have units of mL or cm^3 We are given the density and volume, both of which have good units so all we have ...
what is the molarity of 20.0 ml of a KCl solution that reacts completely with 30.0 ml of a 0.400... How can molarity and osmolarity be calculated from mass per unit volume? How can molarity be used as a conversion factor?
(1 g)/(1 mL) The density of pure water is 1 gram per 1 milliliter or one cubic cm. By knowing the density of water we can use it in dilution equations or to calculate the specific gravity of other solutions. It can also help us determine what other substances are made of using the water displacement experiment. This is done by observing how much water is displaced when an object is submerged ...