A 1.252g sample of srcl2 h20 decomposed to give 1.167g of anhydrous SrCl2. what is the formula of the hydrate?
A 1.252g sample of srcl2 h20 decomposed to give 1.167g of anhydrous SrCl2. what is the...
A 5.000 g sample of NiSO4. __H2O decomposed to give 2.755 g of anhydrous NiSO4 a)Determine what the formula of the hydrate is? b) What is the full chemical name for the hydrate? _____________________________________ c) What is the molar mass of the hydrate? d) What is the mass % of water in the hydrate?
It is often possible to change a hydrate into an anhydrous compound by heating it to drive off the water (dehydration). A 30.74 gram sample of a hydrate of Ba(ClO4)2 was heated thoroughly in a porcelain crucible, until its weight remained constant. After heating, 26.49 grams of the anhydrous compound remained. What is the formula of the hydrate? Use a period instead of a dot in the formula of the hydrate.
It is often possible to change a hydrate into an anhydrous compound by heating it to drive off the water (dehydration). A 39.45 gram sample of a hydrate of BaI2 was heated thoroughly in a porcelain crucible, until its weight remained constant. After heating, 30.91 grams of the anhydrous compound remained. What is the formula of the hydrate?
please answer both questions and explain your answer and show
work!! thanks!!!!!
? H20 ). After heating, the 3. A student heats 4.20 g of nickel(II) acetate (?)-hydrate [Ni(C2H3O2)2 anhydrous salt weighs 2.98 g. What is the formula for the hydrate? 4. A student heats 4.20 g of calcium sulfate (?)-hydrate. After heating, the anhydrous salt weighs 3.94 g. What is the formula for the hydrate?
H20 MASS of H20 2.09 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula.
A student is given a sample of a manganese(II) chloride hydrate. She weighs the sample in a dry, covered crucible and obtains a mass of 24.747 g for the crucible, cover, and sample. Earlier she had found that the crucible and cover weighed 23.599 g. She then heats the crucible to drive off the water of hydration, keeping the crucible at red heat for about 10 minutes with the cover slightly ajar. She then lets the crucible cool, and finds...
use the information given to calculate the formula for
mass/molar mass of the anhydrous salt of your unknown sample(show
calculations)
B. Determine the Formula of an Unknown Hydrate Unknown sample number: 20 Nickel II Molecular formula of the unknown: 1. Mass of crucible + unknown hydrate Nisou "X"H60 (sulfate) 37.40g 36-3lg 1:09g 2. Mass of crucible 3. Mass of unknown hydrate( 1 - 2) 4. Mass of crucible + anhydrous salt a. after first heating b. after second heating 31.3919...
A sample containing a mixture of SrCl2·6H2O (MW = 266.62 g/mol) and CsCl (MW = 168.36 g/mol) originally weighs 1.9715 g. Upon heating the sample to 320 °C, the waters of hydration are driven off SrCl2·6H2O, leaving the anhydrous SrCl2. After cooling the sample in a desiccator, it has a mass of 1.6811 g. Calculate the weight percent of Sr, Cs, and Cl in the original sample. 1) wt% Sr 2) wt% Cs 3) wt% Cl
CHM 010 On-Line Lab, Formula of a Hydrate PURPOSE: To determine the formula of Cuso..x H20. In other words, to determine the value of "X". PROCEDURE: When copper(II) sulfate x hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as anhydrous copper(II) sulfate. The "x" represents a whole number of water molecules attached to...
CuSO4• 5H20 -------> Custy + D u 2) What is the color for anhydrous salt of copper (II) sulfate (CuSO4)? What is the color for ionic hydrate compound of copper (II) sulfate pentahydrate (CuSO4.5H2O)? 3) How would you test a colorless crystalline compound to determine whether it is a hydrate or not? 4) How many grams of CuSO4.5H20 are needed to prepare 50.0 mL of a 1.00 M CuSO4 solution? 5) Suppose you used the Procedure in this experiment to...