They weigh a sample of 0.470 of hydrated nickel(II) chloride, NiCl2·xH2O. When heated, the mass of the remaining anhydrous salt is 0.256 grams. What is the formula of hydrate? What is the name of the hydrate? It is usually possible to remove the hydration water by heating the hydrate. You then heat the sample to remove water and the weight of the anhydrate is 3.52 g. Here are some other answers on how to determine the formula of a hydrate: 2) Note that after heating, you end up with anhydrous magnesium sulfate, MgSO4, and you are left with the same number of moles of anhydrous product that you had moles of the hydrated reagent. In other words, there is a molar ratio of 1:1 between the hydrated compound used and the anhydrous compound produced. Comment: Sodium carbonate forms three hydrates and the above is not one of them. This is a problem that has probably been designed in such a way that you cannot search for® possible answers through interTubez. Just say.` 1) Convert the 29.0 g of magnesium sulfate heptahydrate into moles: During the time I have compiled the examples (and problems) above and below, I have never addressed the following type of problem where the full formula of the hydrate is known and you will be asked how much anhydrate remains after the water is evacuated. When I realized the gap, I included three examples here (as opposed to their own separate file) and added another one to the issues. Therefore, the formula of barium chloride hydrate is #BaCl_2*2H_2O# Here is an example of how to do this: Suppose you want to determine the formula of barium chloride hydrate. You take a sample of the hydrate, weigh it and find that it has a mass of 4.13 g. Decimal percentage anhydrate in hydrate —> 161,441 / 287.5446 = 0.561447 (keep some extra digits) Comment: This is one of three sodium carbonate hydrates that exist.
socratic.org/questions/how-do-you-determine-the-formula-of-a-hydrate?source=search The steps you need to follow to determine the molecular formula of a hydrate are – calculate the mass of water that has been removed; -Use this value to determine the moles of water that were originally present in the hydrate; -use the mass of the anhydrate to determine the mole of the anhydrate; -determine the molar ratio between water and anhydrate; The most common CuSO4 hydrate is pentahydrate, but trihydrate exists. #(„moles of water“)/(„moles of anhydrate“) = 0.034/0.017=2# 2) The hydrate sample lost 54.3% of its mass (all water) and arrived at 105.988 g. This means that the 105,988 g represent 45.7% of the total mass. Hydrates are compounds that contain water of a certain mass in the form of #H_2O# in their molecular formula. These compounds often come in the form of a crystal, which can then be heated to remove water in the form of steam. An anhydrate is the substance that remains after water is removed from a hydrate by heating. Here is a video explaining how to find the empirical formula for copper sulfate. The residue obtained after heating, called anhydrous compound, has a different structure and texture and may have a different color than the hydrate. This means that for every mole of #BaCl_2 #2 moles of water, you have. #(4.13-3.52)# #“g“ * („1 mole of water“)/(„18.0 g“) = 0.034# #“Mole“# 6) How much water is there for each Na2CO3? The key is that there is a 1:1 molar ratio between Na2CO3 and CO2. (Also note that we assume that the gas is pure CO2 and there is no water vapor at all. All water remains liquid.
We also assume that no CO2 dissolves in the water.) They are now proceeding to the determination of the mole of anhydrous salt, #BaCl_2#2) The addition of HCl will cause the formation of CO2 gas by the entire CO32 ion. One mole of carbonation produces n mole of water. 2) Calculate the mass of anhydrous BaCl2 containing 1.0968 g of Ba: The first thing to do is to determine the moles of water that were in the sample. Na2CO3(s) + 2HCl(aq) —> 2NaCl(aq) + CO2(g) + H2O(l) The molar ratio between water and anhydrous salt is. . There are three different ways to solve this type of problem. The following is an example of each path. .